Question

The number of moles of hydrogen molecules required to produced $20$ moles of ammonia through Haber's process is:

• A. $10$
• B. $20$
• C. $30$
• D. $40$

Answer 1

The correct option is C

$30$

Explanation for the correct option:

Option C: 30

Step 1: Given data

Moles of ammonia$=20$

Step 2: Calculating the number of moles of hydrogen

$\underset{\mathrm{nitrogen}}{{\mathrm{N}}_2\left(\mathrm{g}\right)}+\underset{\mathrm{hydrogen}}{3{\mathrm{H}}_2\left(\mathrm{g}\right)}\rightleftharpoons \underset{\mathrm{ammonia}}{2{\mathrm{NH}}_3\left(\mathrm{g}\right)}$

From the balanced equation of Haber's process, we can say that two moles of ammonia are produced by consuming three moles of hydrogen.

Applying stoichiometry, one mole of ammonia is produced by $\frac{3}{2}$moles of hydrogen.

Hence, to produce $20$ moles of ammonia, the number of hydrogen required$=\frac{3}{2}\times 20\Rightarrow 30\mathrm{moles}$

Therefore, the number of moles of hydrogen molecules required to produce $20$ moles of ammonia through Haber's process is $30\mathrm{moles}$