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Q1.1: Calculate the molecular mass of the following:

(i) H2O (ii) CO2 (iii) CH4

Q1.2: Calculate the mass percent of different elements present in sodium sulphate (Na2SO4).

Q1.3: Determine the empirical formula of an oxide of iron which has 69.9% iron and 30.1% dioxygen by mass.

Q1.4: Calculate the amount of carbon dioxide that could be produced when

(i) 1 mole of carbon is burnt in air.

(ii) 1 mole of carbon is burnt in 16 g of dioxygen.

(iii) 2 moles of carbon are burnt in 16 g of dioxygen.

Q1.5: Calculate the mass of sodium acetate (CH3COONa), required to make 500 mL of 0.375 molar aqueous solution. Molar mass of sodium acetate is 82.0245 g mol–1.

Q1.6: Calculate the concentration of nitric acid in moles per litre in a sample which has a density, 1.41 g mL–1 and the mass per cent of nitric acid in it being 69%.

Q1.7: How much copper can be obtained from 100 g of copper sulphate (CuSO4)?

Q1.8: Determine the molecular formula of an oxide of iron in which the mass per cent of iron and oxygen are 69.9 and 30.1 respectively. Given that the molar mass of the oxide is 159.69 g mol–1.

Q1.9: Calculate the atomic mass (average) of chlorine using the following data:


% Natural Abundance

Molar Mass







Q1.10: In three moles of ethane (C2H6), calculate the following:

(i) Number of moles of carbon atoms.

(ii) Number of moles of hydrogen atoms.

(iii) Number of molecules of ethane.

Q1.11: What is the concentration of sugar (C12H22O11) in mol L–1 if its 20 g are dissolved in enough water to make a final volume up to 2 L?

Q1.12: If the density of methanol is 0.793 kg L–1, what is its volume needed for making 2.5 L of its 0.25 M solution?

Q1.13: Pressure is determined as force per unit area of the surface. The SI unit of pressure, Pascal is as shown below:

1Pa = 1N m–2

If mass of air at sea level is 1034 g cm–2, calculate the pressure in Pascal.

Q1.14: What is the SI unit of mass? How is it defined?

Q1.15: Match the following prefixes with their multiples:


















Q1.16: What do you mean by significant figures?

Q1.17: A sample of drinking water was found to be severely contaminated with chloroform, CHCl3, supposed to be carcinogenic in nature. The level of contamination was 15 ppm (by mass).

(i) Express this in percent by mass.

(ii) Determine the molality of chloroform in the water sample.

Q1.18: Express the following in the scientific notation:

(i) 0.0048 (ii) 234,000 (iii) 8008 (iv) 500.0 (v) 6.0012

Q1.19: How many significant figures are present in the following?

(i) 0.0025 (ii) 208 (iii) 5005 (iv)126,000 (v) 500.0 (vi) 2.0034

Q1.20: Round off the following upto three significant figures:

(i) 34.216 (ii) 10.4107 (iii) 0.04597 (iv) 2808

Q1.21: The following data are obtained when dinitrogen and dioxygen react together to form different compounds:

Mass of dinitrogen

Mass of dioxygen


14 g

16 g


14 g

32 g


28 g

32 g


28 g

80 g

(a) Which law of chemical combination is obeyed by the above experimental data? Give its statement.

(b) Fill in the blanks in the following conversions:

(i) 1 km = __________ mm = _________pm

(ii) 1 mg = __________kg = __________ ng

(iii) 1 mL = __________L = __________dm3

Q1.22: If the speed of light is 3.0 × 108 m s–1, calculate the distance covered by light in 2.00 ns.

Q1.23: In a reaction

A + B2 → AB2

Identify the limiting reagent, if any, in the following reaction mixtures.

(i) 300 atoms of A + 200 molecules of B

(ii) 2 mol A + 3 mol B

(iii) 100 atoms of A + 100 molecules of B

(iv) 5 mol A + 2.5 mol B

(v) 2.5 mol A + 5 mol B

Q1.24: Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation:

N2 (g) + H2 (g) → 2NH3 (g)

(i) Calculate the mass of ammonia produced if 2.00 × 103 g dinitrogen reacts with 1.00 ×103 of dihydrogen.

(ii) Will any of the two reactants remain unreacted?

(iii) If yes, which one and what would be its mass?

Q1.25: How are 0.50 mol Na2CO3 and 0.50 M Na2CO3 different?

Q1.26: If ten volumes of dihydrogen gas react with five volumes of dioxygen gas, how many volumes of water vapour would be produced?

Q1.27: Convert the following into basic units:

(i) 28.7 pm (ii) 15.15 pm (iii) 25365 mg

Q1.28: Which one of the following will have largest number of atoms?

(i) 1 g Au (s) (ii) 1 g Na (s) (iii) 1 g Li (s) (iv) 1 g of Cl2 (g)

Q1.29: Calculate the molarity of a solution of ethanol in water in which the mole fraction of ethanol is 0.040.

Q1.30: What will be the mass of one 12C atom in g?

Q1.31: How many significant figures should be present in the answer of the following calculations?

i 0.02856 × 298.15 × 0.112 0.5785

ii 5 × 5.364

iii 0.0125 + 0.7864 + 0.0215

Q1.32: Use the data given in the following table to calculate the molar mass of naturally occuring argon isotopes:


Isotopic molar mass



35.96755 g mol–1



37.96272 g mol–1



39.9624 g mol–1


Q1.33: Calculate the number of atoms in each of the following

(i) 52 moles of Ar (ii) 52 u of He (iii) 52 g of He.

Q1.34: A welding fuel gas contains carbon and hydrogen only. Burning a small sample of it, in oxygen gives 3.38 g carbon dioxide, 0.690 g of water and no other products. A volume of 10.0 L (measured at STP) of this welding gas is found to weigh 11.6 g.

Calculate (i) empirical formula, (ii) molar mass of the gas, and (iii) molecular formula.

Q1.35: Calcium carbonate reacts with aqueous HCl to give CaCl2 and CO2 according to the reaction,

CaCO3 (s) + 2HCl (aq) → CaCl2(aq) + CO2(g) + H2O(l)

What mass of CaCO3 is required to react completely with 25 mL of 0.75 M HCl?

Q1.36: Chlorine is prepared in the laboratory by treating manganese dioxide (MnO2) with aqueous hydrochloric acid according to the reaction

4HCl(aq) + MnO2(s) → 2H2O (l) + MnCl2(aq) + Cl2(g)

How many grams of HCl react with 5.0 g of manganese dioxide?