For the following reaction, Kc = 255 at 1000 K.

CO (g) + Cl2 (g) ⇌ COCl2 (g)

A reaction mixture initially contains a CO concentration of 0.1490 M and a Cl2 concentration of 0.172 M at 1000 K.

Part A

What is the equilibrium concentration of CO at 1000 K?

Express your answer in molarity to three significant figures.

Part B

What is the equilibrium concentration of Cl2 at 1000 KK?

Express your answer in molarity to three significant figures.

Part C

What is the equilibrium concentration of COCl2 at 1000 KK?

Express your answer in molarity to three significant figures.

Question

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kobenhavn kobenhavn · Answer 1 · 2020-03-18T05:54:43+01:00

Answer: Equilibrium concentration of [tex]CO=0.014M[/tex]

Equilibrium concentration of [tex]Cl_2=0.037M[/tex]

Equilibrium concentration of [tex]COCl_2=0.135M[/tex]

Explanation:

Initial concentration of [tex]CO=0.1490M[/tex]

Initial concentration of [tex]Cl_2=0.172M[/tex]

The given balanced equilibrium reaction is,

[tex]CO(g)+Cl_2(g)\rightleftharpoons COCl_2(g)[/tex]

Initial conc. 0.1490 M 0.172 0

At eqm. conc. (0.1490-x) M (0.172-x) M (x) M

The expression for equilibrium constant for this reaction will be,

[tex]K_c=\frac{[COCl_2]}{[Cl_2]\times [CO]}[/tex]

[tex]255=\frac{x}{(0.1490-x)\times (0.172-x)}[/tex]

[tex]x=0.135[/tex]

Equilibrium concentration of [tex]CO=(0.1490-x)M= (0.1490-0.135)=0.014M[/tex]

Equilibrium concentration of [tex]Cl_2=(0.172-x)M= (0.172-0.135)=0.037M[/tex]

Equilibrium concentration of [tex]COCl_2=0.135M[/tex]