Joseph T. answered • 12d

Experienced tutor for a variety of subjects

The first step to solve this problem is to write out a balanced chemical equation. With that, we get 3H_{2} + N_{2} --> 2NH_{3}. Now, we have to determine if the hydrogen or nitrogen is the limiting reactant in this example. In order to do that, we take the amount of H_{2} we have and determine the amount of NH_{3} we would expect if we had an abundance of N_{2}. This would look something like this: (1.87g H_{2})*(1 mol/2.02 g)*(2 mol NH_{3}/3 mol H_{2})(17.04 g NH_{3}/1 mol NH_{3}). The amount of NH_{3} we would expect from 1.87 g of H_{2} is 10.5 g. We do the same equation but with N_{2} and we would get 12.1 g of expected NH_{3}. During the chemical reaction, all of the H_{2} would be used up when we have 10.5 g of NH_{3} which makes H_{2} the limiting reactant and 10.5 g NH_{3} the theoretical yield. If the theoretical yield was 10.5 g and the experimental yield was 2.28 g, we divide the experimental yield by the theoretical yield to get the percent yield for part B. The percent yield is .217 = 21.7%.