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9 April, 16:22

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

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Answers (1)
  1. 9 April, 16:25
    0
    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%
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