1.12g H2 is allowed to react with 9.60 g N2, producing 1.23 g NH3. A. What is the theoretical yield in grams for this reaction under the given conditions?
B. What is the percent yield for this reaction under the given conditions?

A.

B.

Explanation:

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In this case, since the undergoing chemical reaction between nitrogen and hydrogen is:

Thus we proceed as follows:

A. Here, we first need to compute the moles of ammonia yielded by each reactant, in order to identify the limiting one:

Thus, since nitrogen yields the fewest moles of ammonia, we realize it is the limiting reactant, so the theoretical yield, in grams, of ammonia is:

B. Finally, since the actual yield of ammonia is 1.23, the percent yield turns out:

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