Q 1. Which of the following pair of substances contain element and compound within a pair ?(A) \(\mathrm{O}_{2}, \mathrm{CH}_{4}\)(B) \(\mathrm{H}_{2}, \mathrm{O}_{2}\)(C) \(\mathrm{N}_{2}, \mathrm{CO}_{2}\)(D) \(\mathrm{Na}, \mathrm{CO}\);

(d) All of these;

(c) \(\mathrm{C}\) and \(\mathrm{D}\);

(b) B only;

(a) A, C, D;

Q 2. Many countries use Fahrenheit scale for expressing temperature of atmosphere If temperature in any such country is measured \(41^{\circ} \mathrm{F}\) then what is its value in celcius scale and would you expect hot or cold atmosphere in that country?;

(d) \(41^{\circ} \mathrm{C}\), hot;

(c) \(5^{\circ} \mathrm{C}\), cold;

(b) \(25^{\circ} \mathrm{C}\), normal;

(a) \(15^{\circ} \mathrm{C}\), cold;

Q 3. 1 litre of a hydrocarbon weighs as much as one litre of \(\mathrm{CO}_{2}\) at same \(\mathrm{P}\) and \(\mathrm{T}\). Then the molecular formula of the hydrocarbon is:;

(D) \(\mathrm{C}_{3} \mathrm{H}_{6}\);

(C) \(\mathrm{C}_{2} \mathrm{H}_{4}\);

(B) \(\mathrm{C}_{2} \mathrm{H}_{6}\);

(A) \(\mathrm{C}_{3} \mathrm{H}_{8}\);

Q 4. The number of significant figures for the three numbers \(161 \mathrm{~cm}, 0 161 \mathrm{~cm}, 0 0161 \mathrm{~cm}\) are;

(d) 3,3 and 3 respectively;

(c) 3,3 and 4 respectively;

(b) 3,4 and 4 respectively;

(a) 3,4 and 5 respectively;

Q 5. Irrespective of the source, pure sample, of water always yields \(88 89 \%\) mass of oxygen and \(11 11 \%\) mass of hydrogen This is explained by the law of;

(d) constant volume;

(c) constant composition;

(b) multiple proportions;

(a) conservation of mass;

Q 6. The average atomic mass of neon based on following data is: \({ }^{20} \mathrm{Ne}\) \({ }^{21} \mathrm{Ne}\) Relative abundance \({ }^{22} \mathrm{Ne}\);

(a) \(0.33 \mathrm{u}\);

(b) \(20.187 \mathrm{u}\);

(c) \(6.729 \mathrm{u}\);

(d) \(18.058 \mathrm{u}\);

Q 7. Which of the following statements indicates that law of multiple proportion is being followed;

(d) At constant temperature and pressure \(200 \mathrm{~mL}\) of hydrogen will combine with \(100 \mathrm{~mL}\) oxygen to produce \(200 \mathrm{~mL}\) of water vapour.;

(c) When magnesium burns in oxygen, the amount of magnesium taken for the reaction is equal to the amount of magnesium in magnesium oxide formed.;

(b) Carbon forms two oxides namely \(\mathrm{CO}_{2}\) and \(\mathrm{CO}\), where masses fo oxygen which combine with fixed mass of carbon are in the simple ration \(2: 1\).;

(a) Sample of carbon dioxide taken from any source will always have carbon and oxygen in the ratio \(1: 2\).;

Q 8. \(10 \mathrm{~g}\) of hydrogen and \(64 \mathrm{~g}\) of oxygen were filled in a steel vessel and exploded Amount of water produced in this reaction will be:;

(a) \(3 \mathrm{~mol}\);

(b) \(4 \mathrm{~mol}\);

(c) \(1 \mathrm{~mol}\);

(d) \(2 \mathrm{~mol}\);

Q 9. A 5 molar solution of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is diluted from 1 litre to a volume of 10 litres, the normality of the solution will be :;

(a) \(1 \mathrm{~N}\);

(b) \(0.1 \mathrm{~N}\);

(c) \(5 \mathrm{~N}\);

(d) \(0.5 \mathrm{~N}\);

Q 10. In a compound \(\mathrm{C}, \mathrm{H}\) and \(\mathrm{N}\) atoms are present in \(9: 1: 3 5\) by weight Molecular weight of compound is 108 Molecular formula of compound is;

(a) \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{~N}_{2}\);

(b) \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{~N}\);

(c) \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{~N}_{2}\);

(d) \(\mathrm{C}_{9} \mathrm{H}_{12} \mathrm{~N}_{3}\).;

Q 1. Which of the following statements about a compound is incorrect?;

(a) A molecule of a compound has atoms of different elements.;

(b) A compound cannot be separated into its constituent elements by physical methods of separation.;

(c) A compound retains the physical properties of its constituent elements.;

(d) The ratio of atoms of different elements in a compound is fixed.;

Q 2. A sample was weighted using two different balances The results were (i) \(3.929 \mathrm{~g}\) (ii) \(4.0 \mathrm{~g}\) How would the weight of the sample be reported?;

(a) \(3.93 \mathrm{~g}\);

(b) \(3 \mathrm{~g}\);

(c) \(3.9 \mathrm{~g}\);

(d) \(3.929 \mathrm{~g}\);

Q 3. A complex of iron contains \(45.6 \%\) iron by mass. Find out the number of iron atoms in \(5.00 \mathrm{~g}\) of this complex number of iron atoms \(=x^{*} 10^{\wedge} 22\) find the \(x\);

(A) 2.1;

(B) 2.2;

(C) 2.3;

(D) 2.4;

Q 4. Given \(\mathrm{P}=0 0030 \mathrm{~m}, \mathrm{Q}=2 40 \mathrm{~m}, \mathrm{R}=3000 \mathrm{~m}\), Significant figures in \(\mathrm{P}, \mathrm{Q}\) and \(\mathrm{R}\) are respectively;

(a) \(2,2,1\);

(b) \(2,3,4\);

(c) \(4,2,1\);

(d) \(4,2,3\);

Q 5. The percentage of copper and oxygen in samples of \(\mathrm{CuO}\) obtained by different methods were found to be the same The illustrate the law of;

(a) constant proportions;

(b) conservation of mass;

(c) multiple proportions;

(d) reciprocal proportions;

Q 6. What is the average atomic mass of bromine from the following data : (abundance is in \%) Isotope & Mass & Abundance \\ \({ }^{79} \mathrm{Br}\) & 78.9183361 & 50.69 \\ \({ }^{81} \mathrm{Br}\) & 80.916289 & 49.31;

(a) 79.9;

(b) 76.6;

(c) 75.9;

(d) 69.9;

Q 7. The number of molecules in 8 96 litre of a gas at \(0^{\circ} \mathrm{C}\) and 1 atm pressure is approximately;

(a) \(6.023 \times 10^{23}\);

(b) \(12.04 \times 10^{23}\);

(c) \(18.06 \times 10^{23}\);

(d) \(24.08 \times 10^{22}\);

Q 8. Which has the maximum number of molecules among the following?;

(a) \(44 \mathrm{~g} \mathrm{CO}_{2}\);

(b) \(48 \mathrm{~g} \mathrm{O}_{3}\);

(c) \(8 \mathrm{~g} \mathrm{H}_{2}\);

(d) \(64 \mathrm{~g} \mathrm{SO}_{2}\);

Q 9. With increase of temperature, which of these changes?;

(a) Molality;

(b) Weight fraction of solute;

(c) Molarity;

(d) Mole fraction;

Q 10. The empirical formula of an acid is \(\mathrm{CH}_{2} \mathrm{O}_{2}\), the probable molecular formula of acid may be :;

(a) \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}_{4}\);

(b) \(\mathrm{CH}_{2} \mathrm{O}\);

(c) \(\mathrm{CH}_{2} \mathrm{O}_{2}\);

(d) \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\);

Q 1. Choose the correct combination & Element & Compound & Mixture \\;

(a) & Ammonia & Sodium & Air \\;

(b) & Water & Sugar & Aqueous sugar solution \\;

(c) & Hydrogen & Oxygen & Water \\;

(d) & Silver & Water & Air;

Q 2. Two students performed the same experiment separately and each one of them recorded two readings of mass which are given below Correct reading of mass is \(3 0 \mathrm{~g}\) On the basis of given data, mark the correct option out of the following statements Students & \multicolumn{2}{c}{ Readings } \\ & (i) & (ii) \\ A & 3.01 & 2.99 \\ B & 3.05 & 2.95;

(a) Results of both the students are neither accurate nor precise.;

(b) Results of student \(\mathrm{A}\) are both precise and accurate.;

(c) Results of student \(\mathrm{B}\) are neither precise nor accurate.;

(d) Results of student B are both precise and accurate.;

Q 3. The sum of the masses of reactants and products is equal in any physical or chemical reaction. This is in accordance with law of:;

(A) Multiple proportion;

(B) Definite composition;

(C) Conservation of mass;

(D) Reciprocal proportion;

Q 4. If the density of a solution is \(3 12 \mathrm{~g} \mathrm{~mL}^{-1}\), the mass of \(1 5 \mathrm{~mL}\) solution in significant figures is \(\qquad\);

(a) \(4.7 \mathrm{~g}\);

(b) \(4680 \times 10^{-3} \mathrm{~g}\);

(c) \(4.680 \mathrm{~g}\);

(d) \(46.80 \mathrm{~g}\);

Q 5. The law of definite proportions was given by -;

(a) John Dalton;

(b) Humphry Davy;

(c) Proust;

(d) Michael Faraday;

Q 6. What is the mass of an atom of oxygen (in gm)?;

(a) \(2.656 \times 10^{-23}\);

(b) \(1.567 \times 10^{-22}\);

(c) \(2.0 \times 10^{-22}\);

(d) \(3.5 \times 10^{-23}\);

Q 7. What is the molarity of \(0 2 \mathrm{~N} \mathrm{Na}_{2} \mathrm{CO}_{3}\) solution?;

(a) \(0.1 \mathrm{M}\);

(b) \(0 \mathrm{M}\);

(c) \(0.4 \mathrm{M}\);

(d) \(0.2 \mathrm{M}\);

Q 8. The weight of one molecule of a compound \(\mathrm{C}_{60} \mathrm{H}_{122}\) is;

(a) \(1.2 \times 10^{-20}\) gram;

(b) \(1.4 \times 10^{-21}\) gram;

(c) \(5.025 \times 10^{23} \mathrm{gram}\);

(d) \(6.023 \times 10^{23}\) gram;

Q 9. \(6 02 \times 10^{20}\) molecules of urea are present in \(100 \mathrm{ml}\) of its solution The concentration of urea solution is (Avogadro constant, \(\mathrm{N}_{\mathrm{A}}=6 02 \times 10^{23} \mathrm{~mol}^{-1}\) );

(a) \(0.02 \mathrm{M}\);

(b) \(0.01 \mathrm{M}\);

(c) \(0.001 \mathrm{M}\);

(d) \(0.1 \mathrm{M}\);

Q 10. A gaseous hydrocarbon gives upon combustion \(0 72 \mathrm{~g}\) of water and \(3 08 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) The empirical formula of the hydrocarbon is :;

(a) \(\mathrm{C}_{2} \mathrm{H}_{4}\);

(b) \(\mathrm{C}_{3} \mathrm{H}_{4}\);

(c) \(\mathrm{C}_{6} \mathrm{H}_{5}\);

(d) \(\mathrm{C}_{7} \mathrm{H}_{8}\);

Q 1. Choose the correct statement;

(a) The particle \(s\) in liquids are more closely held than gases but less free to move than solids.;

(b) The particles of solids are arranged in orderly fashion but they can move as freely as liquids.;

(c) The particles of gases are far apart as compared to solids and liquids and their movement is easy and fast.;

(d) The particles of gases moves faster than liquids only when the gases are heated.;

Q 2. 0 00016 can be written as A in scientific notaiton Here, A refers to;

(a) \(1.6 \times 10^{-4}\);

(b) \(24.50 \times 10^{-9}\);

(c) \(2.450 \times 10^{-8}\);

(d) \(24.50 \times 10^{-7}\);

Q 3. A \(0.50 \mathrm{~g}\) mixture of \(\mathrm{Cu}_{2} \mathrm{O}\) and \(\mathrm{CuO}\) contains \(0.425 \mathrm{~g}\) of \(\mathrm{Cu}\). What is the mass of \(\mathrm{CuO}\) (in g) in the mixture?\n\[\n(\mathrm{Cu}=63.5 \mathrm{u}, \mathrm{O}=16 \mathrm{u})\n\];

(D) 0.23;

(C) 0.27;

(B)0.22;

(A) 0.21;

Q 4. In which of the following number all zeros are significant?;

(a) 0.0005;

(b) 0.0500;

(c) 50.000;

(d) 0.0050;

Q 5. Which one of the following pairs of compounds illustrate the law of multiple proportions?;

(a) \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{Na}_{2} \mathrm{O}\);

(b) \(\mathrm{MgO}\) and \(\mathrm{Na}_{2} \mathrm{O}\);

(c) \(\mathrm{Na}_{2} \mathrm{O}\) and \(\mathrm{BaO}\);

(d) \(\mathrm{SnCl}_{2}\) and \(\mathrm{SnCl}_{4}\);

Q 6. If the mass of the one atom is found to be \(2 324784 \times 10^{-23} \mathrm{~g}\), then this atom can be ?;

(a) Oxygen;

(b) Carbon;

(c) Fluorine;

(d) Nitrogen;

Q 7. The molar solution of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is equal to :;

(a) \(\mathrm{N} / 2\) solution;

(b) \(\mathrm{N}\) solution;

(c) \(2 \mathrm{~N}\) solution;

(d) \(3 \mathrm{~N}\) solution;

Q 8. The simplest formula of a compound containing \(50 \%\) of element \(\mathrm{X}\) (atomic mass 10 ) and \(50 \%\) of element \(\mathrm{Y}\) (atomic mass 20) is;

(a) \(\mathrm{XY}\);

(b) \(\mathrm{XY}_{3}\);

(c) \(\mathrm{X}_{2} \mathrm{Y}\);

(d) \(\mathrm{X}_{2} \mathrm{Y}_{3}\);

Q 9. Two solutions of a substance (non electrolyte) are mixed in the following manner. \(480 \mathrm{ml}\) of \(1.5 \mathrm{M}\) first solution \(+520 \mathrm{ml}\) of \(1.2 \mathrm{M}\) second solution. What is the molarity of the final mixture?;

(a) \(2.70 \mathrm{M}\);

(b) \(1.344 \mathrm{M}\);

(c) \(1.50 \mathrm{M}\);

(d) \(1.20 \mathrm{M}\);

Q 10. Which of the following is the correct empirical and molecular formulae of a compound, if the molecular mass of a compound is 80 and compound contains \(60 \%\) of C, \(5 \%\) of \(\mathrm{H}\) and \(35 \%\) of \(\mathrm{N}\) ?;

(a) \(\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{~N} ; \mathrm{C}_{4} \mathrm{H}_{4} \mathrm{~N}_{2}\);

(b) \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{~N}_{2} ; \mathrm{C}_{6} \mathrm{H}_{8} \mathrm{~N}_{4}\);

(c) \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{~N}_{2} ; \mathrm{C}_{4} \mathrm{H}_{8} \mathrm{~N}_{4}\);

(d) \(\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{~N} ; \mathrm{C}_{2} \mathrm{H}_{2} \mathrm{~N}\);

Q 1. A mixture contains two or more substances in \(\qquad\) which are called its \(\qquad\);

(a) fixed ratio, compounds;

(b) fixed ratio, elements;

(c) any ratio, components;

(d) any ratio, elements;

Q 2. Which of the following substances cannot be separated in to its constituents by physical methods?;

(a) Sugar and water solution;

(b) Salt and sugar;

(c) Solid glucose;

(d) Both (a) and (b);

Q 3. \(10 \mathrm{~mL}\) of gaseous hydrocarbon on combustion, gives \(40 \mathrm{~mL}\) of \(\mathrm{CO}_{2}(\mathrm{~g})\) and \(50 \mathrm{~mL}\) of \(\mathrm{H}_{2} \mathrm{O}\) (vapour). The hydrocarbon is:;

(A) \(\mathrm{C}_{4} \mathrm{H}_{5}\);

(B) \(\mathrm{C}_{8} \mathrm{H}_{10}\);

(C) \(\mathrm{C}_{4} \mathrm{H}_{8}\);

(D) \(\mathrm{C}_{4} \mathrm{H}_{10}\);

Q 4. The correctly reported answer of addition of \(29 4406,3 2\) and 2 25 will have significant figures;

(a) 3;

(b) 4;

(c) 2;

(d) 5;

Q 5. The molecular weight of \(\mathrm{O}_{2}\) and \(\mathrm{SO}_{2}\) are 32 and 64 respectively At \(15^{\circ} \mathrm{C}\) and \(150 \mathrm{~mm} \mathrm{Hg}\) pressure, one litre of \(\mathrm{O}_{2}\) contains ' \(\mathrm{N}\) ' molecules The number of molecules in two litres of \(\mathrm{SO}_{2}\) under the same conditions of temperature and pressure will be :;

(a) \(\mathrm{N} / 2\);

(b) \(1 \mathrm{~N}\);

(c) \(2 \mathrm{~N}\);

(d) \(4 \mathrm{~N}\);

Q 6. What is the mass of 1 molecule of \(\mathrm{CO}\);

(a) \(2.325 \times 10^{-23}\);

(b) \(4.65 \times 10^{-23}\);

(c) \(3.732 \times 10^{-23}\);

(d) \(2.895 \times 10^{-23}\);

Q 7. Volume of water needed to mix with \(10 \mathrm{~mL} 10 \mathrm{~N} \mathrm{HNO}_{3}\) to get \(0 1 \mathrm{NHNO}_{3}\) is :;

(a) \(1000 \mathrm{~mL}\);

(b) \(990 \mathrm{~mL}\);

(c) \(1010 \mathrm{~mL}\);

(d) \(10 \mathrm{~mL}\);

Q 8. Empirical formula of hydrocarbon containing \(80 \%\) carbon and \(20 \%\) hydrogen is :;

(a) \(\mathrm{CH}_{3}\);

(b) \(\mathrm{CH}_{4}\);

(c) \(\mathrm{CH}\);

(d) \(\mathrm{CH}_{2}\);

Q 9. Which of the following statements are correct? (i) Both solids and liquids have definite volume. (ii) Both liquids and gases do not have definite shape. (iii) Both solids and gases take the shape of the container.;

(a) (i) and (iii);

(b) (ii) and (iii);

(c) (i) and (ii);

(d) (i), (ii) and (iii);

Q 10. Assertion : Significant figures for 0 200 is 3 whereas for 200 it is 1 Reason : Zero at the end or right of a number are significant provided they are not on the right side of the decimal point.;

(a) Assertion is correct, reason is correct; reason is a correct explanation for assertion.;

(b) Assertion is correct, reason is correct; reason is not a correct explanation for assertion;

(c) Assertion is correct, reason is incorrect;

(d) Assertion is incorrect, reason is correct.;

Q 1. Which one of these is not a pure compound?;

(a) \(\mathrm{O}_{3}\);

(b) \(\mathrm{H}_{2} \mathrm{O}_{2}\);

(c) \(\mathrm{H}_{2} \mathrm{O}\);

(d) Sucrose solution;

Q 2. Which of the following is an example of a heterogeneous substance?;

(a) Bottled water;

(b) Table salt;

(c) Pieces of copper;

(d) Candle;

Q 3. The empirical formula of a hydrocarbon containing \(80 \%\) carbon and \(20 \%\) hydrogen is:;

(A) \(\mathrm{CH}\);

(B) \(\mathrm{CH}_{2}\);

(C) \(\mathrm{CH}_{3}\);

(D) \(\mathrm{CH}_{4}\);

Q 4. The number of significant figures in \(10 3106 \mathrm{~g}\) is;

(a) 2;

(b) 3;

(c) 1;

(d) 6;

Q 5. Number of \(g\) of oxygen in \(32 2 \mathrm{~g} \mathrm{Na}_{2} \mathrm{SO}_{4} \cdot 10 \mathrm{H}_{2} \mathrm{O}\) is;

(a) 20.8;

(b) 2.24;

(c) 22.4;

(d) 2.08;

Q 6. Calculate the volume at STP occupied by \(240 \mathrm{gm}\) of \(\mathrm{SO}_{2}\);

(a) 64;

(b) 84;

(c) 59;

(d) 73;

Q 7. One kilogram of a sea water sample contains \(6 \mathrm{mg}\) of dissolved \(\mathrm{O}_{2}\) The concentration of \(\mathrm{O}_{2}\) in the sample in ppm is;

(a) 0.6;

(b) 6.0;

(c) 60.0;

(d) 16.0;

Q 8. The empirical formula of a compound is \(\mathrm{CH}_{2}\) One mole of this compound has a mass of 42 grams Its molecular formula is :;

(a) \(\mathrm{C}_{3} \mathrm{H}_{6}\);

(b) \(\mathrm{C}_{3} \mathrm{H}_{8}\);

(c) \(\mathrm{CH}_{2}\);

(d) \(\mathrm{C}_{2} \mathrm{H}_{2}\);

Q 9. Choose correct option based on following statements Here \(\mathrm{T}\) stands for true statement and \(\mathrm{F}\) for false statement (i) Homogeneous mixture has uniform composition throughout. (ii) All components of a heterogeneous mixture are observable to naked eyes. (iii) All solutions are homogeneous in nature. (iv) Air is an example of heterogeneous mixture.;

(a) TTFF;

(b) TFTF;

(c) FFTT;

(d) TFFF;

Q 10. Assertion : 1 231 has three significant figures Reason : All numbers right to the decimal point are significant.;

(a) Assertion is correct, reason is correct; reason is a correct explanation for assertion.;

(b) Assertion is correct, reason is correct; reason is not a correct explanation for assertion;

(c) Assertion is correct, reason is incorrect;

(d) Assertion is incorrect, reason is correct.;

Q 1. One fermi is;

(a) \(10^{-15} \mathrm{~cm}\);

(b) \(10^{-13} \mathrm{~cm}\);

(c) \(10^{-10} \mathrm{~cm}\);

(d) \(10^{-12} \mathrm{~cm}\);

Q 2. Difference in density is the basis of;

(a) ultrafiltration;

(b) molecular sieving;

(c) molecular attraction;

(d) gravity separation;

Q 3. What percentage of oxygen is present in the compound \(\mathrm{CaCO}_{3} \cdot 3 \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) ?;

(A) \(40.54 \%\);

(B) \(35.56 \%\);

(C) \(15.40 \%\);

(D) \(41.95 \%\);

Q 4. Choose the correct option that represents the result of the given calculation to the appropriate number of significant figures: \[ \frac{43.0 \times 0.0243}{0.340 \times 4} \];

(a) 0.768;

(b) 0.77;

(c) 0.76;

(d) 0.7683;

Q 5. The number of moles of oxygen in one litre of air containing \(21 \%\) oxygen by volume, under standard conditions are;

(a) 0.0093 mole;

(b) 0.21 mole;

(c) 2.10 mole;

(d) 0.186 mole;

Q 6. At S T P the density of \(\mathrm{CCl}_{4}\) vapours in \(\mathrm{g} / \mathrm{L}\) will be nearest to:;

(a) 6.87;

(b) 3.42;

(c) 10.26;

(d) 4.57;

Q 7. The mass of a molecule of water is;

(a) \(3 \times 10^{-25} \mathrm{~kg}\);

(b) \(3 \times 10^{-26} \mathrm{~kg}\);

(c) \(1.5 \times 10^{-26} \mathrm{~kg}\);

(d) \(2.5 \times 10^{-26} \mathrm{~kg}\);

Q 8. A compound contains \(54 55 \%\) carbon, \(9 09 \%\) hydrogen , \(36 36 \%\) oxygen The empirical formula of this compound is;

(a) \(\mathrm{C}_{3} \mathrm{H}_{5} \mathrm{O}\);

(b) \(\mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}_{2}\);

(c) \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\);

(d) \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}\);

Q 9. Read the following and choose the incorrect statements (i) Both weight and mass are same quantities used for measurement of amount of matter present in a substance (ii) Mass and weight of a substance vary from one place to another due to change in gravity. (iii) SI unit of mass is kilogram and while SI unit of weight is gram.;

(a) (i) and (iii);

(b) (ii) and (iii);

(c) (i) and (ii);

(d) All of these;

Q 10. Assertion : One atomic mass unit is defined as one twelfth of the mass of one carbon - 12 atom Reason : Carbon-12 isotope is the most abundunt isotope of carbon and has been chosen as standard.;

(a) Assertion is correct, reason is correct; reason is a correct explanation for assertion.;

(b) Assertion is correct, reason is correct; reason is not a correct explanation for assertion;

(c) Assertion is correct, reason is incorrect;

(d) Assertion is incorrect, reason is correct.;

Q 1. The prefix \(10^{18}\) is;

(a) giga;

(b) kilo;

(c) exa;

(d) nano;

Q 2. A mixture of sand and iodine can be separated by;

(a) crystallisation;

(b) distillation;

(c) sublimation;

(d) fractionation;

Q 3. Find out the normality of a solution, when \(9.8 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is dissolved in \(500 \mathrm{~mL}\) of solution.;

(A) 0.4;

(B) 0.2;

(C) 0.8;

(D) 4.0;

Q 4. Arrange the numbers in increasing no of significant figures \(0 002600,2 6000,2 6,0 260\);

(a) \(2.6<0.260<0.002600<2.6000\);

(b) \(2.6000<2.6<0.002600<0.260\);

(c) \(0.260<2.6<0.002600<2.6000\);

(d) \(0.002600<0.260<2.6<2.6000\);

Q 5. \(10 \mathrm{dm}^{3}\) of \(\mathrm{N}_{2}\) gas and \(10 \mathrm{dm}^{3}\) of gas \(\mathrm{X}\) at the same temperature contain the same number of molecules, the gas \(\mathrm{X}\) is;

(a) \(\mathrm{CO}_{2}\);

(b) \(\mathrm{CO}\);

(c) \(\mathrm{H}_{2}\);

(d) \(\mathrm{NO}\);

Q 6. The number of gram molecules of oxygen in \(6 02 \times 10^{24}\) CO molecules is;

(a) 10 gm molecules;

(b) \(5 \mathrm{gm}\) molecules;

(c) 1 gm molecules;

(d) 0.5 gm molelcules;

Q 7. One mole of \(\mathrm{CO}_{2}\) contains :;

(a) \(3 \mathrm{~g}\) atoms of \(\mathrm{CO}_{2}\);

(b) \(18.1 \times 10^{23}\) molecules of \(\mathrm{CO}_{2}\);

(c) \(6.02 \times 10^{23}\) atoms of \(\mathrm{O}\);

(d) \(6.02 \times 10^{23}\) atoms of \(\mathrm{C}\);

Q 8. In a hydrocarbon, mass ratio of hydrogen and carbon is \(1: 3\), the empirical formula of hydrocarbon is;

(a) \(\mathrm{CH}_{4}\);

(b) \(\mathrm{CH}_{2}\);

(c) \(\mathrm{C}_{2} \mathrm{H}\);

(d) \(\mathrm{CH}_{3}\);

Q 9. Moon takes 27 3 days to complete one orbit around the Earth Now read the following statements and choose the correct code Here \(\mathrm{T}\) is for true statement and \(\mathrm{F}\) is for 'False statement' (i) Moon takes 655.2 hours to complete one orbit around the Earth. (ii) Moon takes 39312 seconds to complete one orbit around the earth. (iii) Moon takes 1638 minutes to complete one orbit around the Earth.;

(a) F T F;

(b) \(\mathrm{T} \mathrm{T} \mathrm{T}\);

(c) T F F;

(d) TF T;

Q 10. Assertion : Volume of a gas is inversely proportional to the number of moles of gas Reason : The ratio by volume of gaseous reactants and products is in agreement with their mole ratio.;

(a) Assertion is correct, reason is correct; reason is a correct explanation for assertion.;

(b) Assertion is correct, reason is correct; reason is not a correct explanation for assertion;

(c) Assertion is correct, reason is incorrect;

(d) Assertion is incorrect, reason is correct.;

Q 1. The prefix zepto stands for (in \(\mathrm{m}\) );

(a) \(10^{9}\);

(b) \(10^{-12}\);

(c) \(10^{-15}\);

(d) \(10^{-21}\);

Q 2. A \(0.50 \mathrm{~g}\) mixture of \(\mathrm{Cu}_{2} \mathrm{O}\) and \(\mathrm{CuO}\) contains \(0.425 \mathrm{~g}\) of \(\mathrm{Cu}\). What is the mass of \(\mathrm{CuO}\) (in g) in the mixture?\n\[\n(\mathrm{Cu}=63.5 \mathrm{u}, \mathrm{O}=16 \mathrm{u})\n\];

(A) 0.21;

(B)0.22;

(C) 0.27;

(D) 0.23;

Q 3. Mixture of \(1 \mathrm{~g}\) each of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) and \(\mathrm{NaHCO}_{3}\) is reacted with \(0.1 \mathrm{NHCl}\). The quantity of \(0.1 \mathrm{MHCl}\) required to react completely with the above mixture is;

(A) \(15.78 \mathrm{~mL}\);

(B) \(157.8 \mathrm{~mL}\);

(C) \(198.4 \mathrm{~mL}\);

(D) \(308 \mathrm{~mL}\);

Q 4. Dimension of pressure are same as that of;

(a) Energy;

(b) Force;

(c) Force per unit volume;

(d) Energy per unit volume;

Q 5. One mole of a gas occupies a volume of \(22 4 \mathrm{~L}\) This is derived from;

(a) Berzelius' hypothesis;

(b) Gay-Lussac's law;

(c) Avogadro's law;

(d) Dalton's law;

Q 6. The number of oxygen atoms in \(4 4 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) is;

(a) \(1.2 \times 10^{23}\);

(b) \(6 \times 10^{22}\);

(c) \(6 \times 10^{23}\);

(d) \(12 \times 10^{23}\);

Q 7. Volume of a gas at NTP is \(1 12 \times 10^{-7} \mathrm{~cm}^{3}\) The number of molecules in it is :;

(a) \(3.01 \times 10^{12}\);

(b) \(3.01 \times 10^{24}\);

(c) \(3.01 \times 10^{23}\);

(d) \(3.01 \times 10^{20}\);

Q 8. An organic compound contains carbon, hydrogen and oxygen Its elemental analysis gave C, \(38 71 \%\) and \(\mathrm{H}, 9 67 \%\) The empirical formula of the compound would be :;

(a) \(\mathrm{CH}_{3} \mathrm{O}\);

(b) \(\mathrm{CH}_{2} \mathrm{O}\);

(c) \(\mathrm{CHO}\);

(d) \(\mathrm{CH}_{4} \mathrm{O}\);

Q 9. Give the correct order of initials \(\mathrm{T}\) or \(\mathrm{F}\) for following statements Use T if statement is true and F if it is false (i) Gay-Lussac's law of gaseous volumes is actually the law of definite proportion by volume. (ii) Law of conservation of mass is true for physical change, but not for chemical change. (iii) The percentage of oxygen in \(\mathrm{H}_{2} \mathrm{O}_{2}\) is different from that in \(\mathrm{H}_{2} \mathrm{O}\). Hence, it violates law of definite proportions. (iv) Fixed mass of A reacts with two different masses of \(\mathrm{B}\) (say \(x\) and \(y\) ), then the ratio of \(x / y\) can be any positive integer. (v) At STP, \(5 \mathrm{~mL}\) of \(\mathrm{N}_{2}\) and \(\mathrm{H}_{2}\) have different no. of molecules.;

(a) TTFTF;

(b) FTTFT;

(c) TFFTF;

(d) TFTTF;

Q 10. Assertion : Equal moles of different substances contain same number of constituent particles Reason : Equal weights of different substances contain the same number of constituent particles.;

(a) Assertion is correct, reason is correct; reason is a correct explanation for assertion.;

(b) Assertion is correct, reason is correct; reason is not a correct explanation for assertion;

(c) Assertion is correct, reason is incorrect;

(d) Assertion is incorrect, reason is correct.;

Q 1. The unit \(\mathrm{J} \mathrm{Pa}^{-1}\) is equivalent to;

(a) \(\mathrm{m}^{3}\);

(b) \(\mathrm{cm}^{3}\);

(c) \(\mathrm{dm}^{3}\);

(d) None of these;

Q 2. \(10 \mathrm{~mL}\) of gaseous hydrocarbon on combustion, gives \(40 \mathrm{~mL}\) of \(\mathrm{CO}_{2}(\mathrm{~g})\) and \(50 \mathrm{~mL}\) of \(\mathrm{H}_{2} \mathrm{O}\) (vapour). The hydrocarbon is:;

(A) \(\mathrm{C}_{4} \mathrm{H}_{5}\);

(B) \(\mathrm{C}_{8} \mathrm{H}_{10}\);

(C) \(\mathrm{C}_{4} \mathrm{H}_{8}\);

(D) \(\mathrm{C}_{4} \mathrm{H}_{10}\);

Q 3. When \(25 \mathrm{~g}\) of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) is dissolved in \(10^{3} \mathrm{Kg}\) of solution, its concentration will be;

(A) \(2.5 \mathrm{ppm}\);

(B) \(25 \mathrm{ppm}\);

(C) \(250 \mathrm{ppm}\);

(D) \(100 \mathrm{ppm}\);

Q 4. \(n g\) of substance \(X\) reacts with \(m g\) of substance \(Y\) to form \(\mathrm{p} g\) of substance \(\mathrm{R}\) and \(\mathrm{q} g\) of substance \(\mathrm{S}\) This reaction can be represented as, \(\mathrm{X}+\mathrm{Y}=\mathrm{R}+\mathrm{S}\) The relation which can be established in the amounts of the reactants and the products will be;

(a) \(\mathrm{n}-\mathrm{m}=\mathrm{p}-\mathrm{q}\);

(b) \(\mathrm{n}+\mathrm{m}=\mathrm{p}+\mathrm{q}\);

(c) \(\mathrm{n}=\mathrm{m}\);

(d) \(\mathrm{p}=\mathrm{q}\);

Q 5. One of the following combination which illustrates the law of reciprocal proportions?;

(a) \(\mathrm{N}_{2} \mathrm{O}_{3}, \mathrm{~N}_{2} \mathrm{O}_{4}, \mathrm{~N}_{2} \mathrm{O}_{5}\);

(b) \(\mathrm{NaCl}, \mathrm{NaBr}, \mathrm{NaI}\);

(c) \(\mathrm{CS}_{2}, \mathrm{CO}_{2}, \mathrm{SO}_{2}\);

(d) \(\mathrm{PH}_{3}, \mathrm{P}_{2} \mathrm{O}_{3}, \mathrm{P}_{2} \mathrm{O}_{5}\);

Q 6. Which has maximum number of molecules?;

(a) \(7 \mathrm{gm} \mathrm{N}_{2}\);

(b) \(2 \mathrm{gm} \mathrm{H}_{2}\);

(c) \(16 \mathrm{gm} \mathrm{NO}_{2}\);

(d) \(16 \mathrm{gmO}_{2}\);

Q 7. How many atoms are contained in one mole of sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) ?;

(a) \(20 \times 6.02 \times 10^{23}\) atoms \(/ \mathrm{mol}\);

(b) \(45 \times 6.02 \times 10^{23}\) atoms \(/ \mathrm{mol}\);

(c) \(5 \times 6.02 \times 10^{23}\) atoms \(/ \mathrm{mol}\);

(d) None of these;

Q 8. A hydrocarbon is composed of \(75 \%\) carbon The empirical formula of the compound is;

(a) \(\mathrm{CH}_{2}\);

(b) \(\mathrm{CH}_{3}\);

(c) \(\mathrm{C}_{2} \mathrm{H}_{5}\);

(d) \(\mathrm{CH}_{4}\);

Q 9. Consider the following statements (i) Atoms of \(\mathrm{H}, \mathrm{O}, \mathrm{N}\) and \(\mathrm{C}\) have identical properties but different mass. (ii) Matter is divisible into atoms which are further indivisible. (iii) The ratio of \(\mathrm{N}\) : \(\mathrm{H}\) in \(\mathrm{NH}_{3}\) is \(1: 3\) and \(\mathrm{N}\) : \(\mathrm{O}\) in nitric oxide is \(2: 1\). (iv) Dalton's atomic theory support law of conservation of mass. Which of the following pairs of statements is true according to Dalton's atomic theory?;

(a) (i) and (ii);

(b) (ii) and (iii);

(c) (ii) and (iv);

(d) (i) and (iv);

Q 10. Assertion : The empirical mass of ethene is half of its molecular mass Reason : The empirical formula represents the simplest whole number ratio of various atoms present in a compound.;

(a) Assertion is correct, reason is correct; reason is a correct explanation for assertion.;

(b) Assertion is correct, reason is correct; reason is not a correct explanation for assertion;

(c) Assertion is correct, reason is incorrect;

(d) Assertion is incorrect, reason is correct.;

Q 1. Which has highest weight?;

(a) \(1 \mathrm{~m}^{3}\) of water;

(b) A normal adult man;

(c) 10 litre of \(\mathrm{Hg}\);

(d) All have same weight;

Q 2. The empirical formula of a hydrocarbon containing \(80 \%\) carbon and \(20 \%\) hydrogen is:;

(A) \(\mathrm{CH}\);

(B) \(\mathrm{CH}_{2}\);

(C) \(\mathrm{CH}_{3}\);

(D) \(\mathrm{CH}_{4}\);

Q 3. 1 litre of a hydrocarbon weighs as much as one litre of \(\mathrm{CO}_{2}\) at same \(\mathrm{P}\) and \(\mathrm{T}\). Then the molecular formula of the hydrocarbon is:;

(A) \(\mathrm{C}_{3} \mathrm{H}_{8}\);

(B) \(\mathrm{C}_{2} \mathrm{H}_{6}\);

(C) \(\mathrm{C}_{2} \mathrm{H}_{4}\);

(D) \(\mathrm{C}_{3} \mathrm{H}_{6}\);

Q 4. \(20 \mathrm{~g}\) of \(\mathrm{CaCO}_{3}\) on heating gave \(8 8 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) and \(11 2 \mathrm{~g}\) of \(\mathrm{CaO}\) This is in accordance with;

(a) The law of conservation of mass.;

(b) The law of constant composition.;

(c) The law of reciprocal proportion.;

(d) None of these;

Q 5. Equal volumes of two gases \(\mathrm{A}\) and \(\mathrm{B}\) are kept in a container at the same temperature and pressure Avogadro's law is invalid if;

(a) the gases are reactive;

(b) the gases are non-reactive;

(c) gas A has more number of molecules than gas B.;

(d) None of these;

Q 6. Number of atoms in 558 5 gram \(\mathrm{Fe}\) (at wt of \(\mathrm{Fe}=55 85\) \(\mathrm{g} \mathrm{\textrm {mol } ^ { - 1 }}\) ) is;

(a) twice that in \(60 \mathrm{~g}\) carbon;

(b) \(6.023 \times 10^{22}\);

(c) half that in \(8 \mathrm{~g} \mathrm{He}\);

(d) \(558.5 \times 6.023 \times 10^{23}\);

Q 7. One litre oxygen gas at S T P will weigh :;

(a) \(1.43 \mathrm{~g}\);

(b) \(2.24 \mathrm{~g}\);

(c) \(11.2 \mathrm{~g}\);

(d) \(22.4 \mathrm{~g}\);

Q 8. \(12 \mathrm{gm}\) of \(\mathrm{Mg}\) (atomic mass 24 ) will react completely with hydrochloric acid to give;

(a) One mol of \(\mathrm{H}_{2}\);

(b) \(1 / 2 \mathrm{~mol}\) of \(\mathrm{H}_{2}\);

(c) \(2 / 3 \mathrm{~mol}\) of \(\mathrm{O}_{2}\);

(d) both \(1 / 2 \mathrm{~mol}\) of \(\mathrm{H}_{2}\) and \(1 / 2 \mathrm{~mol}\) of \(\mathrm{O}_{2}\);

Q 9. Choose the correct option based on following statements Here ' \(T\) ' stands for true and ' \(F\) ' stands for false statement (i) Molecular mass of cane sugar \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) is \(182 \mathrm{amu}\). (ii) 1 mole of cane sugar contains \(6.022 \times 10^{23}\) molecules of cane sugar. (iii) \(34.20 \mathrm{~g}\) of cane sugar contains \(6.022 \times 10^{21}\) molecules of cane sugar.;

(a) TTF;

(b) \(\mathrm{TFT}\);

(c) FTF;

(d) FTT;

Q 10. What are the significant figure(s) in a broken "ruler" show below? (A) 1 (B) 2 (C) 3 (D) 0;

(a) A, B and C;

(b) A, B, D;

(c) A only;

(d) A and B;

Q 1. Which one of the following set of units represents the smallest and largest amount of energy respectively?;

(a) J and erg;

(b) erg and cal;

(c) cal and \(\mathrm{eV}\);

(d) \(\mathrm{eV}\) and \(\mathrm{L}\)-atm;

Q 2. What percentage of oxygen is present in the compound \(\mathrm{CaCO}_{3} \cdot 3 \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) ?;

(A) \(40.54 \%\);

(B) \(35.56 \%\);

(C) \(15.40 \%\);

(D) \(41.95 \%\);

Q 3. A complex of iron contains \(45.6 \%\) iron by mass. Find out the number of iron atoms in \(5.00 \mathrm{~g}\) of this complex number of iron atoms \(=x^{*} 10^{\wedge} 22\) find the \(x\);

(A) 2.1;

(B) 2.2;

(C) 2.3;

(D) 2.4;

Q 4. Which of the following is the best example of law of conservation of mass?;

(a) \(12 \mathrm{~g}\) of carbon combines with \(32 \mathrm{~g}\) of oxygen to form \(44 \mathrm{~g}\) of \(\mathrm{CO}_{2}\);

(b) When \(12 \mathrm{~g}\) of carbon is heated in a vacuum there is no change in mass;

(c) A sample of air increases in volume when heated at constant pressure but its mass remains unaltered;

(d) The weight of a piece of platinum is the same before and after heating in air;

Q 5. Molecular mass is defined as the;

(a) mass of one atom compared with the mass of one molecule;

(b) mass of one atom compared with the mass of one atom of hydrogen;

(c) mass of one molecule of any substance compared with the mass of one atom of C-12;

(d) None of the above;

Q 6. The number of molecules in \(16 \mathrm{~g}\) of methane is;

(a) \(3.0 \times 10^{23}\);

(b) \(\frac{16}{6.02} \times 10^{23}\);

(c) \(6.023 \times 10^{23}\);

(d) \(\frac{16}{3.0} \times 10^{23}\);

Q 7. Number of moles of \(\mathrm{NaOH}\) present in 2 litre of \(0 5 \mathrm{M} \mathrm{NaOH}\) is :;

(a) 1.5;

(b) 2.0;

(c) 1.0;

(d) 2.5;

Q 8. \(20 0 \mathrm{~kg}\) of \(\mathrm{N}_{2(\mathrm{~g})}\) and \(3 0 \mathrm{~kg}\) of \(\mathrm{H}_{2(\mathrm{~g})}\) are mixed to produce \(\mathrm{NH}_{3(\mathrm{~g})}\) The amount of \(\mathrm{NH}_{3(\mathrm{~g})}\) formed is;

(a) \(17 \mathrm{~kg}\);

(b) \(34 \mathrm{~kg}\);

(c) \(20 \mathrm{~kg}\);

(d) \(3 \mathrm{~kg}\);

Q 9. How much time (in hours) would it take to distribute one Avogadro number of wheat grains if \(10^{20}\) grains are distributed each second ?;

(a) 0.1673;

(b) 1.673;

(c) 16.73;

(d) 167.3;

Q 10. Which one of the following sets of compounds correctly illustrate the law of reciprocal proportions?;

(a) \(\mathrm{P}_{2} \mathrm{O}_{3}, \mathrm{PH}_{3}, \mathrm{H}_{2} \mathrm{O}\);

(b) \(\mathrm{P}_{2} \mathrm{O}_{5}, \mathrm{PH}_{3}, \mathrm{H}_{2} \mathrm{O}\);

(c) \(\mathrm{N}_{2} \mathrm{O}_{5}, \mathrm{NH}_{3}, \mathrm{H}_{2} \mathrm{O}\);

(d) \(\mathrm{N}_{2} \mathrm{O}, \mathrm{NH}_{3}, \mathrm{H}_{2} \mathrm{O}\);

Q 1. A measured temperature on Fahrenheit scale is \(200^{\circ} \mathrm{F}\) What will this reading be on Celsius scale?;

(a) \(40^{\circ} \mathrm{C}\);

(b) \(94^{\circ} \mathrm{C}\);

(c) \(93.3^{\circ} \mathrm{C}\);

(d) \(30^{\circ} \mathrm{C}\);

Q 2. Find out the normality of a solution, when \(9.8 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is dissolved in \(500 \mathrm{~mL}\) of solution.;

(A) 0.4;

(B) 0.2;

(C) 0.8;

(D) 4.0;

Q 3. The sum of the masses of reactants and products is equal in any physical or chemical reaction. This is in accordance with law of:;

(A) Multiple proportion;

(B) Definite composition;

(C) Conservation of mass;

(D) Reciprocal proportion;

Q 4. Which of the following statements is correct about the reaction given below? \(4 \mathrm{Fe}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~g})\);

(a) Total mass of iron and oxygen in reactants = total mass of iron and oxygen in product therefore, it follows law of conservation of mass.;

(b) Total mass of reactants \(=\) total mass of product; therefore, law of multiple proportions is followed.;

(c) Amount of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) can be increased by reducing the amount of any one of the reactants (iron or oxygen).;

(d) Amount of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) produced will decrease if the amount of any one of the reactants (iron or oxygen) is taken in excess.;

Q 5. \(1 \mathrm{amu}\) is equal to;

(a) \(\frac{1}{14}\) ofO-16;

(b) \(\frac{1}{12}\) of C-12;

(c) \(1 \mathrm{~g}\) of \(\mathrm{H}_{2}\);

(d) \(1.66 \times 10^{-23} \mathrm{~kg}\);

Q 6. Among the following pairs of compounds, the one that illustrates the law of multiple proportions is;

(a) \(\mathrm{NH}_{3}\) and \(\mathrm{NCl}_{3}\);

(b) \(\mathrm{H}_{2} \mathrm{~S}\) and \(\mathrm{SO}_{2}\);

(c) \(\mathrm{CS}_{2}\) and \(\mathrm{FeSO}_{4}\);

(d) \(\mathrm{CuO}\) and \(\mathrm{Cu}_{2} \mathrm{O}\);

Q 7. \(\mathrm{O}_{2}, \mathrm{~N}_{2}\) are present in the ratio of \(1: 4\) by weight The ratio of number of molecules is :;

(a) \(7: 32\);

(b) \(1: 4\);

(c) \(2: 1\);

(d) \(4: 1\);

Q 8. 20.0 kg of \(H_{2}(g)\) and 32 kg of \(O_{2}(g)\) are reacted to produce \(H_{2}O(l)\). The amount of \(\mathrm{H}_{2} \mathrm{O}\) (1) formed after completion of reaction is;

(a) \(62 \mathrm{~kg}\);

(b) \(38 \mathrm{~kg}\);

(c) \(42 \mathrm{~kg}\);

(d) \(72 \mathrm{~kg}\);

Q 9. Arrange the following in the order of increasing mass (atomic mass: \(\mathrm{O}=16, \mathrm{Cu}=63, \mathrm{~N}=14\) ) I. one atom of oxygen II. one atom of nitrogen III. \(1 \times 10^{-10}\) mole of oxygen IV. \(1 \times 10^{-10}\) mole of copper;

(a) II \(<\) I \(<\) III \(<\) IV;

(b) I \(<\) II \(<\) III \(<\) IV;

(c) III \(<\) II \(<\) IV \(<\) I;

(d) IV \(<\) II \(<\) III \(<\) I;

Q 10. If we consider that \(1 / 6\), in place of \(1 / 12\), mass of carbon atom is taken to be the relative atomic mass unit, the mass of one mole of a substance will;

(a) decrease twice;

(b) increase two fold;

(c) remain unchanged;

(d) be a function of the molecular mass of the substance;

Q 1. Which of the following is not a SI unit?;

(a) metre;

(b) candela;

(c) mole;

(d) litre;

Q 2. Mixture of \(1 \mathrm{~g}\) each of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) and \(\mathrm{NaHCO}_{3}\) is reacted with \(0.1 \mathrm{NHCl}\). The quantity of \(0.1 \mathrm{MHCl}\) required to react completely with the above mixture is;

(A) \(15.78 \mathrm{~mL}\);

(B) \(157.8 \mathrm{~mL}\);

(C) \(198.4 \mathrm{~mL}\);

(D) \(308 \mathrm{~mL}\);

Q 3. If the true value for an experimental result is 6 23 and the results reported by three students \(\mathrm{X}, \mathrm{Y}\) and \(\mathrm{Z}\) are : \(\mathrm{X}: 6.18\) and 6.28 \(\mathrm{Y}: \quad 6.20\) and 6.023 \(\mathrm{Z}: \quad 6.22\) and 6.24 Which of the following option is correct :;

(a) \(\mathrm{X}\) precise, \(\mathrm{Y}\) accurate, \(\mathrm{Z}\) precise and accurate.;

(b) \(\mathrm{X}\) precise and accurate, \(\mathrm{Y}\) not precise, \(\mathrm{Z}\) precise;

(c) Both \(\mathrm{X} \& \mathrm{Z}\) precise \& accurate, \(\mathrm{Y}\) not precise.;

(d) Both \(\mathrm{X} \& \mathrm{Y}\) neither precise nor accurate, \(\mathrm{Z}\) both precise and accurate.;

Q 4. In an experiment \(4 2 \mathrm{~g}\) of \(\mathrm{NaHCO}_{3}\) is added to a solution of acetic acid weighing \(10 0 \mathrm{~g}\), it is observed that \(2 2 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) is released into the atmosphere The residue left behind is found to weigh \(12 0 \mathrm{~g}\) The above observations illustrate;

(a) law of definite proportions.;

(b) law of conservation of mass;

(c) law of multiple proportions;

(d) None of these;

Q 5. The modern atomic weight scale is based on;

(a) \(\mathrm{O}^{16}\);

(b) \(\mathrm{C}^{12}\);

(c) \(\mathrm{H}^{1}\);

(d) \(\mathrm{C}^{13}\);

Q 6. Two samples of lead oxide were separately reduced to metallic lead by heating in a current of hydrogen The weight of lead from one oxide was half the weight of lead obtained from the other oxide The data illustrates;

(a) law of reciprocal proportions;

(b) law of constant proportions;

(c) law of multiple proportions;

(d) law of equivalent proportions;

Q 7. How many moles of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) would be in \(50 \mathrm{~g}\) of the substance ?;

(a) 0.083 mole;

(b) 0.952 mole;

(c) 0.481 mole;

(d) 0.140 mole;

Q 8. What is the weight of oxygen required for the complete combustion of \(2 8 \mathrm{~kg}\) of ethylene?;

(a) \(2.8 \mathrm{~kg}\);

(b) \(6.4 \mathrm{~kg}\);

(c) \(9.6 \mathrm{~kg}\);

(d) \(96 \mathrm{~kg}\);

Q 9. If 1 5 moles of oxygen combines with \(\mathrm{Al}\) to form \(\mathrm{Al}_{2} \mathrm{O}_{3}\), the mass of \(\mathrm{Al}\) in \(\mathrm{g}\) [Atomic mass of \(\mathrm{Al}=27\) ] used in the reaction is;

(a) 2.7;

(b) 54;

(c) 40.5;

(d) 81;

Q 10. The maximum number of molecules are present in;

(a) \(15 \mathrm{~L}^{2} \mathrm{H}_{2}\) gas at STP;

(b) \(5 \mathrm{~L}\) of \(\mathrm{N}_{2}\) gas at STP;

(c) \(0.5 \mathrm{~g}\) of \(\mathrm{H}_{2}\) gas;

(d) \(10 \mathrm{~g}\) of \(\mathrm{O}_{2}\) gas;

Q 1. The prefix \(10^{-24}\) is;

(a) yotta;

(b) zeta;

(c) yocto;

(d) zepto;

Q 2. When \(25 \mathrm{~g}\) of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) is dissolved in \(10^{3} \mathrm{Kg}\) of solution, its concentration will be;

(A) \(2.5 \mathrm{ppm}\);

(B) \(25 \mathrm{ppm}\);

(C) \(250 \mathrm{ppm}\);

(D) \(100 \mathrm{ppm}\);

Q 3. In the final answer of the expression \[ \frac{(29.2-20.2)\left(1.79 \times 10^{5}\right)}{1.37} \] the number of significant figures is :;

(a) 1;

(b) 2;

(c) 3;

(d) 4;

Q 4. In one experiment, \(4 \mathrm{~g}\) of \(\mathrm{H}_{2}\) combine with \(32 \mathrm{~g}\) of \(\mathrm{O}_{2}\) to form \(36 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}\) In another experiment, when \(50 \mathrm{~g}_{\mathrm{of}} \mathrm{H}_{2}\) combine with \(400 \mathrm{~g}\) of \(\mathrm{O}_{2}\) then \(450 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}\) is formed Above two experiments follow;

(a) The law of conservation of mass;

(b) The law of constant composition;

(c) Both (a) and (b);

(d) Neither (a) nor (b);

Q 5. The percentage weight of \(\mathrm{Zn}\) in white vitriol \(\left[\mathrm{ZnSO}_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O}\right]\) is approximately equal to \((\mathrm{Zn}=65, \mathrm{~S}=32, \mathrm{O}=16\) and \(\mathrm{H}=1\) );

(a) \(33.65 \%\);

(b) \(32.56 \%\);

(c) \(23.65 \%\);

(d) \(22.65 \%\);

Q 6. In compound \(\mathrm{A}, 1 00 \mathrm{~g}\) of nitrogen unites with \(0 57 \mathrm{~g}\) of oxygen In compound B, \(2 00 \mathrm{~g}\) of nitrogen combines with \(2 24 \mathrm{~g}\) of oxygen In compound \(\mathrm{C}, 3 00 \mathrm{~g}\) of nitrogen combines with \(5 11 \mathrm{~g}\) of oxygen These results obey the following law;

(a) law of constant proportion;

(b) law of multiple proportion;

(c) law of reciprocal proportion;

(d) Dalton's law of partial pressure;

Q 7. The mass of 1 mole of electrons is;

(a) \(9.1 \times 10^{-28} \mathrm{~g}\);

(b) \(1.008 \mathrm{mg}\);

(c) \(0.55 \mathrm{mg}\);

(d) \(9.1 \times 10^{-27} \mathrm{~g}\);

Q 8. In the reaction \[ 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \rightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) \] When 1 mole of ammonia and \(1 \mathrm{~mole} \mathrm{of}_{2}\) are made to react to completion,;

(a) 1.0 mole of \(\mathrm{H}_{2} \mathrm{O}\) is produced;

(b) 1.0 mole of \(\mathrm{NO}\) will be produced;

(c) all the oxygen will be consumed;

(d) all the ammonia will be consumed;

Q 9. Which one of the following is the lightest?;

(a) 0.2 mole of hydrogen gas;

(b) \(6.023 \times 10^{22}\) molecules of nitrogen;

(c) \(0.1 \mathrm{~g}\) of silver;

(d) 0.1 mole of oxygen gas;

Q 10. How many moles of magnesium phosphate, \(\mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) will contain 0 25 mole of oxygen atoms?;

(a) \(1.25 \times 10^{-2}\);

(b) \(2.5 \times 10^{-2}\);

(c) 0.02;

(d) \(3.125 \times 10^{-2}\);