Question

8. Given the following reaction, N₂ (g) + 3H₂(g) → 2NH3 (g), how many liters of H₂ are required toproduce 47 moles of NH3?

Answer 1

1579.2 liters of H₂

Step-by-step explanation

Given that:

N₂ (g) + 3H₂(g) → 2NH₃ (g)

What to find:

The liters of H₂ required to produce 47 moles of NH₃.

Step-by-step solution:

Step 1: Determine the moles of H₂ required to produce 47 moles of NH₃.

Using the mole ratio of H₂ to NH₃ in the given reaction; 3:2

If 3 moles of H₂ = 2 moles of NH₃

So x moles of H₂ = 47 moles of NH₃

To get x, cross multiply and divide both sides by 2 moles of NH₃

`\begin{gathered} x=\frac{47\text{ }moles\text{ }NH_3}{2\text{ }moles\text{ }NH_3}*3\text{ }moles\text{ }H_2 \\ \\ x=70.5\text{ }moles\text{ }H_2 \end{gathered}`

Step 2: Convert 70.5 moles of H₂ to liters.

Conversion factor: 1 mole of any gas at STP = 22.4 liters.

1 mole of H₂ = 22.4 liters

70.5 moles of H₂ = (70.5 mol/1 mol) x 22.4 liters = 1579.2 liters.

Therefore, 1579.2 liters of H₂ are required to produce 47 moles of NH₃.