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25 November, 07:36

Using the equation

N2+3H2-->2NH3

how many grams of hydrogen must react if the reaction needs to produce 31.75 grams of NH3?

Question options:

5.6

11.2

none of these

22.4

+5
Answers (1)
  1. 25 November, 08:12
    0
    (Answer) 5.6 g

    Mass of ammonia produced = 31.75 g

    Moles of ammonia produced = (Mass / molar mass of ammonia)

    = (31.75 g / 17.031 g / mol) = 1.86 moles.

    According to the balanced chemical equation, mole ratio of hydrogen and ammonia = 3: 2

    Moles of hydrogen needed to produce 1.86 moles of ammonia

    = (3/2 x 1.86) moles = 2.79 moles

    Mass of hydrogen needed = (Moles x molar mass of hydrogen)

    = (2.79 x 2) g = 5.58 g = 5.6 g

    Therefore, 5.6 g of hydrogen must react to produce 31.75 g of ammonia.
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