5.77 g of nitrogen react with excess hydrogen producing 6.83 g of ammonia what is the percent yield. Determine/Label the actual yield, theoretical yield, and the percent yield for the reaction. N2+3H2=2NH3

Question

Chemistry

Flores

4 January, 23:24

5.77 g of nitrogen react with excess hydrogen producing 6.83 g of ammonia what is the percent yield. Determine/Label the actual yield, theoretical yield, and the percent yield for the reaction. N2+3H2=2NH3

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Answers (1)

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Aden Burns · Answer 1

Percentage yield is 41.21%

Explanation:

Equation of reaction,

N₂ + 3H₂ → 2NH₃

Actual NH3 = 6.83g

Mass of N2 = 5.77g

Theoretical yield = ?

5.77g of N2 = 6.83g of NH3

14g of N2 = xg

X = (14 * 6.83) / 5.77

X = 95.62 / 5.77

X = 16.57g of NH3

Theoretical yield of NH3 is 16.57g

Percentage yield = (actual yield / theoretical yield) * 100

% yield = (6.83 / 16.57) * 100

% yield = 0.4121 * 100

% yield = 41.21%

The percentage yield of NH3 is 41.21%