Solution Found!
Consider the reaction. An equilibrium mixture of this reaction at a certain temperature
Chapter 15, Problem 51P(choose chapter or problem)
Consider the reaction.
\(\mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g)\)
An equilibrium mixture of this reaction at a certain temperature has \(\left[\mathrm{COCl}_{2}\right]=0.225 \mathrm{M},[\mathrm{CO}]=0.105 \mathrm{M}\), and \(\left[\mathrm{Cl}_{2}\right]=0.0844 \mathrm{M}\). What is the value of the equilibrium constant at this temperature?
Equation Transcription:
Text Transcription:
\mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g)
\left[\mathrm{COCl}_{2}\right]=0.225 \mathrm{M},[\mathrm{CO}]=0.105 \mathrm{M}
\left[\mathrm{Cl}_{2}\right]=0.0844 \mathrm{M}
Questions & Answers
QUESTION:
Consider the reaction.
\(\mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g)\)
An equilibrium mixture of this reaction at a certain temperature has \(\left[\mathrm{COCl}_{2}\right]=0.225 \mathrm{M},[\mathrm{CO}]=0.105 \mathrm{M}\), and \(\left[\mathrm{Cl}_{2}\right]=0.0844 \mathrm{M}\). What is the value of the equilibrium constant at this temperature?
Equation Transcription:
Text Transcription:
\mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g)
\left[\mathrm{COCl}_{2}\right]=0.225 \mathrm{M},[\mathrm{CO}]=0.105 \mathrm{M}
\left[\mathrm{Cl}_{2}\right]=0.0844 \mathrm{M}
ANSWER:Solution 51P:
Here, we are going to find out the value of equilibrium constant at this temperature.
Step 1:
COCl2(g) ⇆ CO(g) + Cl2(g)
The equilibrium constant for this reaction is