Question

If 100.0g of nitrogen is reacted with 100.0g of hydrogen, what is the theoretical yield of the reaction in grams? What is the excess reactant? What is the limiting reactant?

66.7 g of NH3, hydrogen is the limiting, nitrogen is in excess.
121.6 g of NH3, nitrogen is the limiting, hydrogen is in excess.
33.0 mol of NH3, nitrogen is the limiting, hydrogen is in excess.
121.6 g of NH3, hydrogen is the limiting, nitrogen is in excess.

Answer 1

Answer:

121.6 of $NH_{3}$ ,Nitrogen is limiting and Hydrogen is in excess.

Step-by-step explanation:

The reaction involved in this question is known as Haeber's Process and the reaction is as follows

$N_{2} + 3H_{2} -->2 NH_{3}$

We need to find the moles of each to determine the total product, the excess reagent and limiting reagent.

No. of moles of$N_{2}$=$\frac{100}{28}$=3.57 mol

No. of moles of $H_{2}$=$\frac{100}{2}$=50 moles

We need moles of $H_{2}$ and $N_{2}$ in the ratio of 3:1.

Therefore, we can clearly see that $H_{2}$  is excess. And $N_{2}$ is the limitng reagent.

As, $N_{2}$ is the limiting reagent a total of 2 * 3.57 moles of $NH_{3}$ will be formed.

Therefore, total mass of $NH_{3}$ =7.14*17=121.6 g