?At \(100^{\circ} \mathrm{C}\), the equilibrium constant for the reaction

Chapter 15, Problem 15.43

(choose chapter or problem)

At \(100^{\circ} \mathrm{C}\), the equilibrium constant for the reaction \(\mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g)\) has the value \(K_{c}=\) \(2.19 \times 10^{-10}\). Are the following mixtures of \(\mathrm{COCl}_{2}, \mathrm{CO}\), and \(\mathrm{Cl}_{2}\) at \(100^{\circ} \mathrm{C}\) at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium.

(a) \(\left[\mathrm{COCl}_{2}\right]=2.00 \times 10^{-3} \mathrm{M},[\mathrm{CO}]=3.3 \times 10^{-6} \mathrm{M}\), \(\left[\mathrm{Cl}_{2}\right]=6.62 \times 10^{-6} \mathrm{M}\)

(b) \(\left[\mathrm{COCl}_{2}\right]=4.50 \times 10^{-2} \mathrm{M},[\mathrm{CO}]=1.1 \times 10^{-7} \mathrm{M}\), \(\left[\mathrm{Cl}_{2}\right]=2.25 \times 10^{-6} \mathrm{M}\)

(c) \(\left[\mathrm{COCl}_{2}\right]=0.0100 \mathrm{M},[\mathrm{CO}]=\left[\mathrm{Cl}_{2}\right]=1.48 \times 10^{-6} \mathrm{M}\)

Text Transcription:

100^circ C

COCl_2(g) \rightleftharpoons CO(g)+Cl_2(g)

K_c=

2.19 \times 10^-10

COCl_2, CO

Cl_2

100^circ C

[COCl_2]=2.00 \times 10^-3 M,[CO]=3.3 \times 10^-6 M

[Cl_2]=6.62 \times 10^-6 M

[COCl_2]=4.50 \times 10^-2 M,[CO]=1.1 \times 10^-7 M

[Cl_2]=2.25 \times 10^-6 M

[COCl_2]=0.0100 M,[CO]=[Cl_2]=1.48 \times 10^-6 M