Question

Some of the acid in acid rain is produced from the following reaction: 3N*O_{2}(g) + H_{2}*O(l) -> NO(g) + 2HN*O_{3}(aq) A falling raindrop weighing 0.05 g comes into contact with 0.010 g of N*O_{2} a) What is the theoretical yield of HN*O_{3} ? b) What is the % yield of nitric acid if 0.006 g of HN*O_{3} are actually formed?

Answer 1

The theoretical yield of HNO3 is 0.000214 g, and the % yield of HNO3 is 2801%.

Step-by-step explanation:

To calculate the theoretical yield of HNO3, we need to determine the limiting reactant first. The molar mass of N2O2 is 4 × 14.01 g/mol = 56.04 g/mol. So, the moles of N2O2 are 0.010 g / 56.04 g/mol = 0.000178 moles. According to the balanced equation, the mole ratio between N2O2 and HNO3 is 3:2. Therefore, the theoretical yield of HNO3 is (0.000178 moles of N2O2) × (2 moles of HNO3 / 3 moles of N2O2) × (63.01 g/mol) = 0.000214 g.

To calculate the % yield of HNO3, we need to compare the actual yield given (0.006 g) with the theoretical yield (0.000214 g). The % yield is (0.006 g / 0.000214 g) × 100% = 2801%.