Solution Found!
Producing Ammonium Sulfate: Calculating the Required Ammonia
Chapter 3, Problem 3.77(choose chapter or problem)
The fertilizer ammonium sulfate \(\left[\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\right]\) is prepared by the reaction between ammonia \(\left(\mathrm{NH}_{3}\right)\) and sulfuric acid:
\(2 \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q)\)
How many kilograms of \(\mathrm{NH}_{3}\) are needed to produce \(1.00\times10^5\mathrm{\ kg}\text{ of }\left(\mathrm{NH}_4\right)_2\mathrm{SO}_4\)?
Questions & Answers
QUESTION:
The fertilizer ammonium sulfate \(\left[\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\right]\) is prepared by the reaction between ammonia \(\left(\mathrm{NH}_{3}\right)\) and sulfuric acid:
\(2 \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q)\)
How many kilograms of \(\mathrm{NH}_{3}\) are needed to produce \(1.00\times10^5\mathrm{\ kg}\text{ of }\left(\mathrm{NH}_4\right)_2\mathrm{SO}_4\)?
ANSWER:Step 1 of 3
Molar mass of \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}:(14.01 \times 2+1.008 \times 8)+32.06+(16.00 \times 4)=132.14 \mathrm{~g} / \mathrm{mol}\)
Molar mass of \(\mathrm{NH}_{3}: 14.01+1.008 \times 3=17.03 \mathrm{~g} / \mathrm{mol}\).
Watch The Answer!
Producing Ammonium Sulfate: Calculating the Required Ammonia
Want To Learn More? To watch the entire video and ALL of the videos in the series:
Discover the process to determine the quantity of ammonia (NH?) required to produce a specific amount of ammonium sulfate ((NH?)?SO?). Through a step-by-step explanation, learn the application of the balanced chemical equation and molar mass conversions. Transform theoretical chemistry into practical knowledge with this insightful guide.