Consider the following reaction: 2a + b -> 3c + d 3.0 mol a and 2.0 mol b react to form 4.0 mol c. what is the percent yield of this reaction?
a) 50%
b) 67%
c) 75%
d) 89%
e) 100%
what other formulas for % yield other than actual/theoretical yield?

Answer : The correct option is, (D) 89 %

Solution : Given,

Moles of A = 3.0 mol

Moles of B = 2.0 mol

First we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

From the balanced reaction we conclude that

As, 2 mole of A react with 1 mole of B

So, 3 moles of A react with moles of B

From this we conclude that, B is an excess reagent because the given moles are greater than the required moles and A is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of C.

From the reaction, we conclude that

As, 2 mole of A react to give 3 mole of C

So, 3 mole of A react to give mole of C

Theoretical yield of C = 4.5 mol

Actual yield of C = 4 mol

Now we have to calculate the percent yield of of the reaction.

Therefore, the percent yield of the reaction is 89 %

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step-by-step explanation:

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