Final answer:
0.21 mol of Cl2 can form 0.42 mol of HCl. For the reaction of 0.18 mol of Cl2, 0.225 mol of H2O is required. If 0.50 mol of HCl is formed, 0.3125 mol of H2O will react based on the stoichiometry of the balanced equation.
Step-by-step explanation:
The reaction of sodium thiosulfate with chlorine and water is used to neutralize excess chlorine in the textile industry. The balanced chemical equation provided is as follows:
Na2S2O3(aq) + 4Cl2(g) + 5H2O(l) → 2NaHSO4(aq) + 8HCl(aq)
1) To find how many moles of HCl can form from 0.21 mol of Cl2, we look at the stoichiometry of the balanced equation. For every 4 moles of Cl2, 8 moles of HCl are produced. Thus, from 0.21 mol of Cl2, we can form:
(0.21 mol Cl2) × (8 mol HCl / 4 mol Cl2) = 0.42 mol HCl
2) To determine the number of moles of H2O required for the reaction of 0.18 mol of Cl2, we again refer to the stoichiometry of the equation which shows that 5 moles of H2O react with every 4 moles of Cl2:
(0.18 mol Cl2) × (5 mol H2O / 4 mol Cl2) = 0.225 mol H2O
3) To find out how many moles of H2O react if 0.50 mol HCl is formed, we need to consider the ratio of HCl to H2O from the balanced equation, which is 8:5. Therefore, for every 8 moles of HCl, 5 moles of H2O are used:
(0.50 mol HCl) × (5 mol H2O / 8 mol HCl) = 0.3125 mol H2O