Barium chloride can be made by reacting excess barium carbonate with dilute hydrochloric acid.
The equation for the reaction is:
BaCO3(s)+2HCl(aq)→BaCl2(aq)+H2O(l)+CO2(g) \text{BaCO}_3(\text{s}) + 2\text{HCl}(\text{aq}) \rightarrow \text{BaCl}_2(\text{aq}) + \text{H}_2\text{O}(\text{l}) + \text{CO}_2(\text{g}) BaCO3(s)+2HCl(aq)→BaCl2(aq)+H2O(l)+CO2(g)In one experiment, a sample of 0.080 mol0.080\text{ mol}0.080 mol of BaCO3\text{BaCO}_3BaCO3 is added to 0.130 mol0.130\text{ mol}0.130 mol of HCl\text{HCl}HCl. Show, by calculation, that the BaCO3\text{BaCO}_3BaCO3 is in excess.
Calculate the maximum volume, in cm3\text{cm}^3cm3, of carbon dioxide, measured at room temperature and pressure (RTP), that would be obtained when 0.130 mol0.130\text{ mol}0.130 mol of HCl\text{HCl}HCl reacts completely with BaCO3\text{BaCO}_3BaCO3.
One mole of any gas occupies 24,000 cm3 at room temperature and pressure. \text{One mole of any gas occupies } 24,000\text{ cm}^3\text{ at room temperature and pressure.} One mole of any gas occupies 24,000 cm3 at room temperature and pressure.In another experiment, 0.050 mol0.050\text{ mol}0.050 mol of BaCO3\text{BaCO}_3BaCO3 reacts with excess HCl\text{HCl}HCl. A yield of 9.5 g9.5\text{ g}9.5 g of hydrated barium chloride crystals, BaCl2⋅2H2O\text{BaCl}_2 \cdot 2\text{H}_2\text{O}BaCl2⋅2H2O, is obtained.
Calculate the percentage yield of BaCl2⋅2H2O\text{BaCl}_2 \cdot 2\text{H}_2\text{O}BaCl2⋅2H2O.
Relative atomic masses, Ar: Ba=137; Cl=35.5; H=1; O=16. \text{Relative atomic masses, } A_r\text{: Ba} = 137\text{; Cl} = 35.5\text{; H} = 1\text{; O} = 16\text{.} Relative atomic masses, Ar: Ba=137; Cl=35.5; H=1; O=16.Suggest one practical reason why the percentage yield of BaCl2⋅2H2O\text{BaCl}_2 \cdot 2\text{H}_2\text{O}BaCl2⋅2H2O crystals is less than 100%100\%100%.
