The question is incomplete, here is the complete question:
The Haber process can be used to produce ammonia, and it is based on the following reaction.
If the reaction occurs in the laboratory and 5 moles of each hydrogen and nitrogen gas reacts and produces 2.8 moles of ammonia, calculate the percent yield for the experiment. Use the quantity of the product that is produced by the limiting reagent as the theoretical yield.
<u>Answer:</u> The percent yield of the reaction is 84.08 %.
<u>Explanation:</u>
We are given:
Moles of nitrogen gas = 5 mole
Moles of hydrogen gas = 5 mole
For the given chemical equation:
By Stoichiometry of the reaction:
3 moles of hydrogen gas reacts with 1 mole of nitrogen gas
So, 5 mole of hydrogen gas will react with = of nitrogen gas
As, given amount of nitrogen gas is more than the required amount. So, it is considered as an excess reagent.
Thus, hydrogen gas is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
3 moles of hydrogen gas produces 2 moles of ammonia
So, 5 moles of hydrogen gas will produce = of ammonia
To calculate the percentage yield of ammonia, we use the equation:
Experimental yield of ammonia = 2.8 moles
Theoretical yield of ammonia = 3.33 moles
Putting values in above equation, we get:
Hence, the percent yield of the reaction is 84.08 %.