The following reaction is used in some self-contained breathing devices as a source of O2 (g). 4 KO2(s) + 2 CO2(g) ↔ 2 K2CO3(s) + 3 O2(g) Kp = 28.5 at 250C (for pressures in atm). Suppose that a sample of CO2(g) is added to an evacuated flask containing KO2(s) and equilibrium is established. If the equilibrium partial pressure of CO2(g) is found to be 0.0571 atm, what are the equilibrium partial pressures of O2(g) and the total gas pressure? a. 0.453 atm; 0.510 atm b. 0.529 atm; 0.601 atm c. 0.0929 atm; 0.150 atm d. 1.18 atm; 1.23 atm
The following reaction is used in some self-contained breathing devices as a source of O2 (g). 4 KO2(s) + 2 CO2(g) ↔ 2 K2CO3(s) + 3 O2(g) Kp = 28.5 at 250C (for pressures in atm). Suppose that a sample of CO2(g) is added to an evacuated flask containing KO2(s) and equilibrium is established. If the equilibrium partial pressure of CO2(g) is found to be 0.0571 atm, what are the equilibrium partial pressures of O2(g) and the total gas pressure? a. 0.453 atm; 0.510 atm b. 0.529 atm; 0.601 atm c. 0.0929 atm; 0.150 atm d. 1.18 atm; 1.23 atm
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 41QRT: Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures.
2 NOCl(g) ⇌ 2 NO(g) +...
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The following reaction is used in some self-contained breathing devices as a source of O2 (g).
4 KO2(s) + 2 CO2(g) ↔ 2 K2CO3(s) + 3 O2(g) Kp = 28.5 at 250C (for pressures in atm).
Suppose that a sample of CO2(g) is added to an evacuated flask containing KO2(s) and equilibrium is established. If the equilibrium partial pressure of CO2(g) is found to be 0.0571 atm, what are the equilibrium partial pressures of O2(g) and the total gas pressure?
a. 0.453 atm; 0.510 atm
b. 0.529 atm; 0.601 atm
c. 0.0929 atm; 0.150 atm
d. 1.18 atm; 1.23 atm
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