1.95 g of H_{2} is allowed to react with 9.94 g of N _{2}, producing 1.56 g of NH _{3}. What is the theoretical yield in grams for this reaction under the given conditions? What is the percent yield for this reaction under the given conditions?

Determine the theoretical yield by identifying the limiting reagent between H_{2 }and N_{2}. Then calculate the percent yield using the provided mass of NH_{3}.

Step 1. Write the balanced equation.

- Reactant appears to be H
_{2}and N_{2}producing NH_{3 }

H_{2} + N_{2} → NH_{3}

- Balance N (2 on both sides):

H_{2} + N_{2} → 2NH_{3}