The first step in the Ostwald process for producing nitric acid is
4NH₃(g) + 5O₂(g) $\rarr$ 4NO(g) + 6H₂O(g) .
If the reaction of 150.g of ammonia with 150.g of oxygen gas yields 87.g of nitric oxide (NO) , what is the percent yield of this reaction?

Question

The first step in the Ostwald process for producing nitric acid is
4NH₃(g) + 5O₂(g)

\rarr

4NO(g) + 6H₂O(g) .
If the reaction of 150.g of ammonia with 150.g of oxygen gas yields 87.g of nitric oxide (NO) , what is the percent yield of this reaction?

Quizplus · Accepted Answer

The percent yield is calculated as follows:Percent yield = (Actual yield / Theoretical yield) x 100%The theoretical yield is the amount of product that would be produced if the reaction went to completion. To calculate the theoretical yield, we need to determine the limiting reactant.To do this, we can compare the moles of each reactant to the stoichiometric coefficients in the balanced chemical equation:Moles of NH3 = 150 g / 17 g/mol = 8.82 molMoles of O2 = 150 g / 32 g/mol = 4.69 molThe stoichiometric coefficients in the balanced chemical equation are:4 moles of NH3 react with 5 moles of O2Therefore, the mole ratio of NH3 to O2 is 4:5.Comparing the moles of each reactant to the mole ratio, we find that O2 is the limiting reactant because it has the smallest mole ratio.The theoretical yield of NO is therefore:Theoretical yield of NO = 4.69 mol O2 x (4 mol NO / 5 mol O2) x (30 g NO / 1 mol NO) = 117.2 g NOThe actual yield of NO is given as 87 g.Therefore, the percent yield is:Percent yield = (87 g / 117.2 g) x 100% = 74.2%The closest answer choice to 74.2% is C) 77%.

The First Step in the Ostwald Process for Producing Nitric →\rarr→

The First Step in the Ostwald Process for Producing Nitric $\rarr$