Question

Ammonia (NH3) can be produced by the reaction of hydrogen gas with nitrogen gas:

3H2 + N2→2NH3

A chemist reacts 2.00 mol H2 with excess N2 . The reaction yields 0.80 mol NH3 .

What is the percent yield of the reaction? A. 25% B.40% C.60% D.80%

Answer 1

40%

Step-by-step explanation:

took the test

Answer 2

Percent yield = 61.5%

Step-by-step explanation:

Given data:

Moles of hydrogen = 2.00 mol

Actual yield of ammonia= 0.80 mol

Percent yield = ?

Solution:

Chemical equation:

3H₂ + N₂ → 2NH₃

Now we will compare the moles of ammonia with hydrogen from balance chemical equation:

H₂ : NH₃

3 : 2

2 : 2/3×2 = 1.3 mol

Percent yield:

Percent yield = Actual yield / theoretical yield × 100

Percent yield = 0.80 mol /1.3 mol × 100

Percent yield = 0.615 × 100

Percent yield = 61.5%