The reaction N2 + 3 H2 → 2 NH3 is used to produce ammonia. When 450. g of hydrogen was reacted with nitrogen, 1575 g of ammonia were actually produced. What is the percent yield of this reaction?

a. 20,7%

b. 41,5%

c. 62,1%

d. 30,8%

e. More information is needed to solve this problem

61.76%

Explanation:

Percent yield = Actual yield/Theoeetical yield * 100%

We need to calculate the theoretical yield for this reaction.

Firstly, we need to know the number of moles of hydrogen reacted = mass of hydrogen : molar mass = 450 : 2 = 225 moles

From the reaction, we can see that 3 moles of hydrogen yielded 2 moles of ammonia. Hence 225 moles of hydrogen will yield:

(225 * 2) : 3 = 150 moles

The actual mass of ammonia yielded = number of moles * molar mass = 150 * 17 = 2550g

Actual yield = 1575g

Theoretical yield = 2550g

Percentage yield = 1575/2550 * 100% = 61.76%