Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
100%

At a certain temperature, the ?pKp for the decomposition of H2SH2S is 0.761.0.761.

 

H2S(g)↽−−⇀H2(g)+S(g)

Initially, only H2SH2S is present at a pressure of 0.151 atm0.151 atm in a closed container. What is the total pressure in the container at equilibrium?

Expert Solution
Check Mark
Step 1

consider the reaction:

s + H oss

Initial partial pressure of H2S is 0.104 and equilibrium constant,  is 0.842

ICE table for the reaction is:

H2 ICE Initial pressure Change in pressure At equilibrium 0 HS 0.104 -X 0.104-x

Use the expression:

K - (P.„)x(px) (PH)

Substitute 0.842 for , x for H2 and x for

XXX 0.842= 0.104

On solving, the equation is:

r? +0.842x -0.0876 = 0

The value of x is solved by using the quadratic equation:

- b b2-4ac 2a

Substitute 0.842 for b, 1 for a and 0.0876 for c and solve the equation:

-0.842 x= (0.842) -4(1)(-0.0876) 2x1

= 0.0936 or -0.936

The values for x is 0.0936

Explanation | Hint for next step

If x atm be the decrease in pressure of A at time t and one mole each of B and C is being formed, the increase in pressure of B and C will also be x atm.

As per the ICE table:

Equilibrium partial pressure of H2S , PH2S  is 0.104 – x

Substitute x as 0.0936

PH2  = 0.104 - 0.0936

PH2  is 0.0104 atm.

Equilibrium partial pressure of , PH2 is x

Substitute x as 0.0936

PH2 is 0.0936 atm

Equilibrium partial pressure of , Ps is x

Substitute x as 0.0936

Ps is 0.0936 atm

Explanation | Hint for next step

The value of x is 0.0936 which is used to calculate the equilibrium partial pressure of the gases.

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