What volume of H₂ gas at 780 mm Hg and 23 °C is required to produce 10.6 L of NH₃ gas at the same temperature and pressure using the following chemical reaction?
N₂(g) + 3H₂(g) $\rightarrow$ 2NH₃(g)

Question

What volume of H₂ gas at 780 mm Hg and 23 °C is required to produce 10.6 L of NH₃ gas at the same temperature and pressure using the following chemical reaction?
N₂(g) + 3H₂(g)

\rightarrow

2NH₃(g)

Quizplus · Accepted Answer

According to the balanced chemical equation, 3 moles of $H_2$ gas react to produce 2 moles of $NH_3$ gas. Therefore, to produce 10.6 L of $NH_3$, the volume of $H_2$ required can be calculated using the stoichiometric relationship from the equation. Since the conditions of temperature and pressure are the same for both gases, we can use the direct ratio from the balanced equation: $3:2 = x:10.6$, solving for $x$ gives us 15.9 L of $H_2$ gas needed.

What Volume of H2 Gas at 780 Mm Hg and 23

What Volume of H₂ Gas at 780 Mm Hg and 23