Answer to Question #170303 in General Chemistry for daisy

Question

You react 10.0 g of nitrogen gas with hydrogen

gas according to the following reaction.

N 2 (g) 3 H2 (g) n 2N H3 (g)

a. What mass of hydrogen is required to

completely react with 10.0 g sample of

nitrogen gas?

b. What mass of ammonia is produced from

10.0 g of nitrogen gas and sufficient

hydrogen gas?

Answer 1

(a) moles of N₂ $=\dfrac{mass}{MM}= \dfrac{10.0g}{28.02g/mol}=0.3569mol$

Moles of H₂ needed will then be;

Moles ratio of N₂:H₂ = 1:3

Moles of H₂ $=\dfrac{3}{1}x0.3569mol = 1.0707mol$

Mass of H₂ = moles x MM = 1.0707mol x 2.016g/mol

= 2.158g

(b) Moles of N₂ = 0.3569mol

Mole ratio of N₂ : NH₃ = 1:2

Moles of NH₃ $=\dfrac{2}{1}x0.3569mol = 0.7138mol$

Mass of NH₃= moles x MM

= 0.7138mol x 17.031g/mol

=12.134g