If the theoretical yield of the reaction below corresponds to 25.3 g and the percent yield of the reaction is known to be reproducibly 81.1%, calculate the actual yield. given: li2o + h2o → 2 lioh 81.1 g 48.9 g 20.5 g 45.8 g none of the above

Question

Chemistry

Leslie

11 March, 15:58

If the theoretical yield of the reaction below corresponds to 25.3 g and the percent yield of the reaction is known to be reproducibly 81.1%, calculate the actual yield. given: li2o + h2o → 2 lioh 81.1 g 48.9 g 20.5 g 45.8 g none of the above

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Answers (1)

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Lowe · Answer 1

The actual yield is computed by multiplying the theoretical yield by the decimal equivalent of the given yield of reaction.

That is,

Actual yield = (Theoretical Yield) x (Percent Yield of reaction)

Actual yield = (25.3 g) x (0.811)

Actual yield = 20.51 g

Hence, the actual yield is approximately 20.5g and the answer is the third choice.