4.4 g of CO2(g) are introduced into a 1 dm³ flask containing excess carbon at 1000°C, so that the equilibrium CO2(g) + C(s) CO(g) is reached. The gas density at equilibrium corresponds to an average molecular weight of 36. Calculate the equilibrium total pressure and the value of Kp.[1408 kPa; 7.04]
4.4 g of CO2(g) are introduced into a 1 dm³ flask containing excess carbon at 1000°C, so that the equilibrium CO2(g) + C(s) CO(g) is reached. The gas density at equilibrium corresponds to an average molecular weight of 36. Calculate the equilibrium total pressure and the value of Kp.[1408 kPa; 7.04]
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 61QRT
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![4.4 g of CO2(g) are introduced into a 1 dm flask containing excess carbon at 1000°C, so that the
equilibrium
CO2(g) + C(s) 2 CO(g)
is reached. The gas density at equilibrium corresponds to an average molecular
weight of 36. Calculate the equilibrium total pressure and the value of Kp.[1408 kPa; 7.04]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb115676e-ee4e-40ec-bf5c-fc874dff6cdf%2F3875b717-b80a-4960-9b04-f0d9d24cd957%2Fwvm8ubf_processed.png&w=3840&q=75)
Transcribed Image Text:4.4 g of CO2(g) are introduced into a 1 dm flask containing excess carbon at 1000°C, so that the
equilibrium
CO2(g) + C(s) 2 CO(g)
is reached. The gas density at equilibrium corresponds to an average molecular
weight of 36. Calculate the equilibrium total pressure and the value of Kp.[1408 kPa; 7.04]
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