If the percent yield for the following reaction is 75.0%,and 25.0 g of NO₂ are consumed in the reaction,how many grams of nitric acid,HNO₃(aq) are produced?
3 NO₂(g) + H₂O(l) → 2 HNO₃(aq) + NO(g)

Question

Quizplus · Accepted Answer

First, calculate the theoretical yield of HNO3. The molar mass of NO2 is 46.01 g/mol, and the molar mass of HNO3 is 63.01 g/mol. From the balanced equation, 3 moles of NO2 produce 2 moles of HNO3. Convert 25.0 g of NO2 to moles: 25.0 g / 46.01 g/mol = 0.543 moles of NO2. Using the stoichiometry of the reaction, 0.543 moles NO2 * (2 moles HNO3 / 3 moles NO2) = 0.362 moles HNO3. Convert moles of HNO3 to grams: 0.362 moles * 63.01 g/mol = 22.8 g (theoretical yield). With a 75% yield, the actual yield is 22.8 g * 0.75 = 17.1 g.

If the Percent Yield for the Following Reaction Is 75