6.1 Stoichiometry and composition  (Page 2/5)

Moles and empirical formulae

1. Calcium chloride is produced as the product of a chemical reaction.
   1. What is the formula of calcium chloride?
   2. What percentage does each of the elements contribute to the mass of a molecule of calcium chloride?
   3. If the sample contains 5 g of calcium chloride, what is the mass of calcium in the sample?
   4. How many moles of calcium chloride are in the sample?
2. 13g of zinc combines with 6.4g of sulfur.What is the empirical formula of zinc sulfide?
   1. What mass of zinc sulfide will be produced?
   2. What percentage does each of the elements in zinc sulfide contribute to its mass?
   3. Determine the formula of zinc sulfide.
3. A calcium mineral consisted of 29.4% calcium, 23.5% sulphur and 47.1% oxygen by mass. Calculate the empirical formula of the mineral.
4. A chlorinated hydrocarbon compound was analysed and found to consist of 24.24% carbon, 4.04% hydrogen and 71.72% chlorine. From another experiment the molecular mass was found to be 99 g.mol ${}^{-1}$ . Deduce the empirical and molecular formula.

Molar volumes of gases

It is possible to calculate the volume of one mole of gas at STP using what we now know about gases.

1. Write down the ideal gas equation pV = nRT, therefore V = $\frac{nRT}{p}$
2. Record the values that you know, making sure that they are in SI units You know that the gas is under STP conditions. These are as follows: p = 101.3 kPa = 101300 Pan = 1 mole R = 8.31 J.K ${}^{-1}$ .mol ${}^{-1}$ T = 273 K
3. Substitute these values into the original equation.
   $$V=\frac{nRT}{p}$$
   $$V=\frac{1mol\times 8.31J.K^{-1}.mo{l}^{-1}\times 273K}{101300Pa}$$
4. Calculate the volume of 1 mole of gas under these conditions The volume of 1 mole of gas at STP is 22.4 $\times$ 10 ${}^{-3}$ m ${}^3$ = 22.4 dm ${}^3$ .