Question

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

CO (g) + Cl2 (g) ⇌ COCl2 (g)


Part A

If a reaction mixture initially contains a CO concentration of 0.1530 and a Cl2 concentration of 0.174 at 1000K. What is the equilibrium concentration of CO at 1000 K?

Part B

What is the equilibrium concentration of Cl2 at 1000 K?

Part C

What is the equilibrium concentration of COCl2 at 1000 K?


4)Consider the following reaction:

HC2H3O2(aq)+H2O(l)⇌H3O+(aq)+C2H3O−2(aq)

Kc=1.8×10−5 at 25∘C


If a solution initially contains 0.180 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25∘C?


5)Consider the following reaction:

Br2(g)+Cl2(g)⇌2BrCl(g)

Kp=1.11×10−4 at 150 K.

A reaction mixture initially contains a Br2 partial pressure of 755 torr and a Cl2 partial pressure of 740 torr at 150 K.


Calculate the equilibrium partial pressure of BrCl.

Answer 1

Phosgene dissociates almost completely at this temperature, so the applied equilibrium constant for the reverse reaction

COCl2=CO+Cl2

[CO][Cl ₂ ] / [COCl ₂ ]=255 mole/ l

[COCl2]=X moles

[CO]=0,153-x=0.1527958

[Cl ₂ ]=0,174-x=0.173895

=>(0.153-x) (0.174-x)/x=255

0.026622-0.327 x+x2=255x

x=0.0001042

[H₃O]⁺[C₂HO₂]^-/[(HCOOH)₂]

Let x = change in [HC2H3O2]

At equilibrium: [HC2H3O2] = (0.250 – x)

At equilibrium = [H3O+] = x and [C2H3O2-] = x

1.8 x 10^-5 = (x) (x) / (0.250 – x) ; I will neglect x in the (0.180 –x) since x is much smaller than 0.250

x^2 = 1.8 x 10^-5*(0.180)

x^2 = 1.8*1.8*10-6

x = [H3O+] = 1.8*10-3