🤓 Based on our data, we think this question is relevant for Professor Velazquez Mojica's class at UCD.
We are asked to calculate the mass of urea is produced per minute by this reaction assuming 100% yield
2NH3(g) + CO2(g) → H2NCONH2(s) + H2O(g)
Step 1. Calculate moles per minute of each
n = 1105.27 mol/min NH3
n = 663.16 mol/min CO2
Step 2. Simultaneously calculate the theoretical yield and identify the limiting reactant.
Use both to calculate for H2NCONH2
Molar mass H2NCONH2 = 60.07 g/mol
Urea (H2NCONH2) is used extensively as a nitrogen source in fertilizers. It is produced commercially from the reaction of ammonia and carbon dioxide:
2NH3(g) + CO2(g) H2NCONH2(s) + H2O(g)
Ammonia gas at 223°C and 90. atm flows into a reactor at a rate of 500. L/min. Carbon dioxide at 223°C and 45 atm flows into the reactor at a rate of 600. L/min. What mass of urea is produced per minute by this reaction assuming 100% yield?
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.
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Based on our data, we think this problem is relevant for Professor Velazquez Mojica's class at UCD.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.