2. What is the percentyield if 121.5 g of silveris produced when 13.5 gof aluminum is reactedwith excess silver nitratesolution. The unbalancedreaction equation is:Al + AgNO3 →AI(NO3)3 +Ag

Предыдущий
вопрос Следующий
вопрос

To find the percent yield, we first need to determine the theoretical yield of silver that should be produced based on the balanced chemical equation.

Write and balance the chemical equation:
2Al + 3AgNO3 → 2Al(NO3)3 + 3Ag

Calculate the molar mass of Al:
Al = 26.98 g/mol

Calculate the molar mass of Ag (since we are interested in the yield of Ag):
Ag = 107.87 g/mol

Calculate the molar ratio between Al and Ag in the balanced equation:
2 mol Al : 3 mol Ag

Determine the number of moles of Al reacted:
13.5 g Al / 26.98 g/mol = 0.5 mol Al

Calculate the theoretical yield of Ag that should be produced:
(3 mol Ag / 2 mol Al) 0.5 mol Al 107.87 g/mol = 80.90 g Ag

Calculate the percent yield:
Percent Yield = (Actual Yield / Theoretical Yield) 100%
Percent Yield = (121.5 g / 80.90 g) 100%
Percent Yield ≈ 150.55%

Therefore, the percent yield of silver in this reaction is approximately 150.55%.