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When no + Cl2 → NOClrnrn8.2 liters of Cl2 are reacted with 1.3 liters of NO, 2.9 grams of NOCl are produced at STP. What is the percent yield of this reaction?

Accepted Answer

Assuming the reaction:

NO + Cl2 → 2NOCl

1.3 liters of NO at STP = 1.3 L * (273.15 K / 298.15 K) = 1.10 L

Using the mole ratio from the balanced equation, with Cl2 as the limiting reactant, we can calculate the theoretical yield of NOCl:

8.2 L Cl2 * (1 mol Cl2 / 22.4 L) * (2 mol NOCl / 1 mol Cl2) = 0.732 mol NOCl

Converting moles to grams:

0.732 mol NOCl * (65.45 g / mol) = 47.96 g NOCl

Percent yield = (Actual yield / Theoretical yield) * 100

Percent yield = (2.9 g / 47.96 g) * 100 = 6.05 %

Therefore, the percent yield of this reaction is 6.05%.

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