The equilibrium constant, K, for the following reaction is 1.29x102 at 600 K. COC,(g) CO(g) + Cl(g) Calculate the equilibrium concentrations of reactant and products when 0.279 moles of COCI,(g) are introduced into a 1.00 L vessel at 600 K. [COCI,] = M [CO] M [Cl] M %3D
The equilibrium constant, K, for the following reaction is 1.29x102 at 600 K. COC,(g) CO(g) + Cl(g) Calculate the equilibrium concentrations of reactant and products when 0.279 moles of COCI,(g) are introduced into a 1.00 L vessel at 600 K. [COCI,] = M [CO] M [Cl] M %3D
Chemistry
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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
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![The equilibrium constant, K, for the following reaction is 1.29x10 at 600 K.
COCI,(g)
CO(g) + Cl2(g)
Calculate the equilibrium concentrations of reactant and products when 0.279 moles of COCI,(g) are introduced into a 1.00 L vessel at 600 K.
[COCH] =
M
[CO]
[Cl,]
M
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe011ab3d-63f0-4f4d-8f65-282cd40a67d1%2F759ee671-df25-4cba-8568-4d731e05e52a%2F058hjh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The equilibrium constant, K, for the following reaction is 1.29x10 at 600 K.
COCI,(g)
CO(g) + Cl2(g)
Calculate the equilibrium concentrations of reactant and products when 0.279 moles of COCI,(g) are introduced into a 1.00 L vessel at 600 K.
[COCH] =
M
[CO]
[Cl,]
M
M
Expert Solution
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Step 1: Given and using ICE table Kc equation values
Given:
Kc = 1.29 × 10-2
Temperature= T = 600 K
Balanced equilibrium equation:
CoCl2(g) <=> Co(g) + Cl2(g)
Initial | 0.279 moles | 0.0 | 0.0 |
Change | -x | x | x |
Equilibrium | 0.279 - x | x | x |
KC = [Co][Cl2] / [ CoCl2 ]
= 1.29 × 10^-2 = (X)^2 / ( 0.279 - x )
....(using above ICE table
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