1 QUANTITATIVE CHEMISTRY 1CHEMISTRY FOR THE IB DIPLOMA © CAMBRIDGE UNIVERSITY PRESS 2011

1 Quantitative chemistry

Revision checklistI am able to:

state the value of Avogadro’s constant

work out the mass of one molecule of propanol

work out how many moles of chloride ions there are in 0.2 mol CaCl2

de� ne Mr and Ar

work out the molar mass of each of the following: CaCO3, C8H18, Mg(NO3)2

work out the number of moles in each of the following:a 2 g of calcium c 224 cm3 of O2 at STPb 0.8 g of ammonium nitrate d 10 cm3 of 2 mol dm−3 NaCl(aq)

work out the mass of 0.01 mol calcium sulfate

distinguish between empirical formula and molecular formula

work out which of the following are empirical formulas and which are molecular formulasC2H2 CH2 N2H3 C3H5 C6H6 NHO Cl2O C2H6O

work out the empirical formula of the following: compound X, which contains 24.7% K, 34.8% Mn and 40.5% O by mass

work out the molecular formula of a compound with empirical formula CH2O if the molar mass is 90 g mol−1

calculate the empirical formula of a compound, containing just carbon and hydrogen, given that it burns in excess oxygen to produce 8.08 g of carbon dioxide and 2.64 g of water

calculate the empirical formula of a compound containing carbon, hydrogen and oxygen given that, when 1.52 g of the compound burns in excess oxygen, 3.04 g of CO2 and 1.24 g of H2O are produced.

balance the following equations using whole numbers and � nd the sum of the coe� cients of the species involved:

C4H9OH + O2 → CO2 + H2O

Fe2O3 + CO → Fe + CO2

PCl3 + H2O → H3PO3 + HCl

NH3 + O2 → NO + H2O

calculate the percentage yield of ethyl ethanoate, given that 10 g of ethanol reacts with excess ethanoic acid to produce 15 g of ethyl ethanoate:

C2H5OH + CH3COOH → CH3COOC2H5 + H2O

work out the limiting reactant when 0.1 mol Sb4O6 reacts with 0.5 mol H2SO4:

Sb4O6 + 6H2SO4 → 2Sb2(SO4)3 + 6H2O

work out the volume of hydrogen gas (measured at STP) produced when 0.23 g of sodium is reacted with excess water:

2Na + 2H2O → 2NaOH + H2

work out the volume of oxygen required to react exactly with 10 cm3 of methane in the following reaction:

CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)

draw graphs showing the relationship between P and V, P and T, and V and T for a � xed mass of an ideal gas

work out the � nal volume when 200 cm3 of hydrogen gas is heated from 27 °C to 327 °C at constant pressure

state the ideal gas equation

state the units that are required for the ideal gas equation

calculate the volume occupied by 0.1 mol of an ideal gas at 25 °C and 1.2 × 105 Pa

calculate the molar mass of an ideal gas if 0.586 g of the gas occupies a volume of 282 cm3 at a pressure of 1.02 × 105 Pa and a temperature of −18 °C

2 CHEMISTRY FOR THE IB DIPLOMA © CAMBRIDGE UNIVERSITY PRESS 20111 QUANTITATIVE CHEMISTRY

distinguish between the terms ‘solute’, ‘solvent’, ‘solution’ and ‘concentration’

calculate the concentration (in g dm−3 and mol dm−3) of a sodium hydroxide solution, given that 10 cm3 of the solution contains 4 g of NaOH

work out the number of moles in 25 cm3 0.1 mol dm−3 H2SO4

calculate the concentration of a sodium hydroxide solution, given that 28.0 cm3 of the solution reacts with 25.0 cm3 of 0.100 mol dm−3 sulfuric acid according to the equation:

2NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l)