Calculate the amount of hydrogen gas required | vedclass

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Question

(B) The balanced chemical equation for the formation of ammonia is:
$N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$
From the stoichiometry of the reac

Vedclass · Accepted Answer

$17.65$

Vedclass · Answer

(B) The balanced chemical equation for the formation of ammonia is:
$N_{2(g)} + 3H_{2(g)} ightarrow 2NH_{3(g)}$
From the stoichiometry of the reaction:
$2 	ext{ moles}$ of $NH_3$ are produced from $3 	ext{ moles}$ of $H_2$.
Molar mass of $NH_3 = 17 	ext{ g/mol}$.
Molar mass of $H_2 = 2 	ext{ g/mol}$.
Therefore,$2 	imes 17 	ext{ g} = 34 	ext{ g}$ of $NH_3$ is produced from $3 	imes 2 	ext{ g} = 6 	ext{ g}$ of $H_2$.
To produce $100 	ext{ g}$ of $NH_3$,the mass of $H_2$ required is:
$	ext{Mass of } H_2 = \frac{6 	ext{ g}}{34 	ext{ g}} 	imes 100 	ext{ g} = 17.647 	ext{ g} \approx 17.65 	ext{ g}$.

Calculate the amount of hydrogen gas required to produce $100 \text{ g}$ of ammonia by the reaction of $N_{2(g)}$ and $H_{2(g)}$ gases. (in $\text{ g}$)

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