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%

idk what the question is about

it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2