Question
A reaction vessel for synthesizing ammonia by reacting nitrogen and hydrogen is charged with $6.04 \mathrm{kg}$ of $\mathrm{H}_{2}$ and excess $\mathrm{N}_{2} .$ A total of $28.0 \mathrm{kg}$ of $\mathrm{NH}_{3}$ is produced. What is the percent yield of the reaction?
Step 1
We know that the molar mass of hydrogen is 2.02 g/mol. So, we have: \[6.04 \, \text{kg} \, H_{2} = 6040 \, \text{g} \, H_{2}\] \[ \text{Moles of} \, H_{2} = \frac{6040 \, \text{g}}{2.02 \, \text{g/mol}} = 2990 \, \text{moles}\] Show more…
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