# Problem: Consider the reaction shown below:   3 H2(g) + N2 (g) → 2 NH3 (g)When a certain amount of hydrogen reacts in excess nitrogen, it produces 2.153 g of ammonia with a percent yield of 38.25%, what is the theoretical yield?A) 5.629 gB) 0.1778 gC) 0.8235 gD) 0.05701 gE) 7.768 g

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###### FREE Expert Solution

We’re being asked to calculate the theoretical yield of NH­3 in a reaction that formed 2.153 g NH3 with a percent yield of 38.25%

The balanced chemical equation is:

3 H2(g) + N2(g)  2 NH3(g)

Recall that percent yield is given by:

###### Problem Details

Consider the reaction shown below:

3 H2(g) + N2 (g) → 2 NH3 (g)

When a certain amount of hydrogen reacts in excess nitrogen, it produces 2.153 g of ammonia with a percent yield of 38.25%, what is the theoretical yield?

A) 5.629 g

B) 0.1778 g

C) 0.8235 g

D) 0.05701 g

E) 7.768 g

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Percent Yield concept. If you need more Percent Yield practice, you can also practice Percent Yield practice problems.

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Our tutors rated the difficulty ofConsider the reaction shown below:   3 H2(g) + N2 (g) → 2 NH...as medium difficulty.

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What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Gillespie's class at FIU.