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Urea $\left(\mathrm{H}_{2} \mathrm{NCONH}_{2}\right)$ is used extensively as a nitrogen source in fertilizers. It is produced commercially from the reaction of ammonia and carbon dioxide:
$$2 \mathrm{NH}_{3}(g)+\mathrm{CO}_{2}(g) \underset{\text { Pressure }}{\stackrel{\text { Heat }}{\text { Pressur }} \mathrm{H}_{2} \mathrm{NCONH}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(g)}$$
Ammonia gas at $223^{\circ} \mathrm{C}$ and 90 . atm flows into a reactor at a rate of $500 . \mathrm{L} / \mathrm{min}$. Carbon dioxide at $223^{\circ} \mathrm{C}$ and $45 \mathrm{~atm}$ flows into the reactor at a rate of $600 . \mathrm{L} / \mathrm{min}$. What mass of urea is produced per minute by this reaction assuming $100 \%$ yield?
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5 comments
Kelly C.
March 20, 2023
Thanks for breaking down the production of urea from ammonia and carbon dioxide 🙌
Tyler M.
June 14, 2023
way to go for showing the step-by-step calculations and keeping it real with the moles of ammonia and carbon dioxide! 💯
Austin M.
June 23, 2023
good lookin out for explaining how to find the limiting reactant and calculating the mass of urea produced 🙏
Edwin G.
November 26, 2023
props for showing the conversion to grams and kilograms for the mass of urea per minute! you rock! 🌟
Robin R.
November 29, 2023
Mad respect for breaking it down and coming through with the final answer Keep shining ✨