9. Urea is produced from the reaction of ammonia with carbon dioxide according to the following equation: CO2(g) + 2NH3(g) → CO(NH2)2(s) + H20(1) In an experiment, a 25.0-L reaction vessel was charged with 12.0 atm of CO2 and 23.0 atm of NH3, and the above reaction occurred at 123°C until the limiting reactant was completely reacted. (a) Which is the limiting reactant? (b) How many grams of urea was produced if the yield was 100%? (c) What is the percent yield if 493 g of urea were obtained? (R = 0.0821 L.atm/K.mol)

9. Urea is produced from the reaction of ammonia with carbon dioxide according to the following equation: CO2(g) + 2NH3(g) → CO(NH2)2(s) + H20(1) In an experiment, a 25.0-L reaction vessel was charged with 12.0 atm of CO2 and 23.0 atm of NH3, and the above reaction occurred at 123°C until the limiting reactant was completely reacted. (a) Which is the limiting reactant? (b) How many grams of urea was produced if the yield was 100%? (c) What is the percent yield if 493 g of urea were obtained? (R = 0.0821 L.atm/K.mol)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

9.
Urea is produced from the reaction of ammonia with carbon dioxide according to the following equation:
CO2(g) + 2NH3(g) → CO(NH2)2(s) + H2O(1)
In an experiment, a 25.0-L reaction vessel was charged with 12.0 atm of CO2 and 23.0 atm of NH3, and the
above reaction occurred at 123°C until the limiting reactant was completely reacted. (a) Which is the limiting
reactant? (b) How many grams of urea was produced if the yield was 100%? (c) What is the percent yield
if 493 g of urea were obtained? (R = 0.0821 L.atm/K.mol)

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