At a certain temperature, the 𝐾p for the decomposition of H2S is 0.887.H2S(g)↽−−⇀H2(g)+S(g)Initially, only H2S is present at a pressure of 0.142 atm in a closed container. What is the total pressure in the container at equilibrium?

To solve this problem, we need to use the concept of equilibrium and the equilibrium constant (Kp in this case).

Step 1: Write the balanced chemical equation The balanced chemical equation is already given: H2S(g) ⇌ H2(g) + S(g)

Step 2: Write the expression for the equilibrium constant For the reaction, the equilibrium constant expression Kp is: Kp = [H2][S] / [H2S]

Step 3: Set up the ICE table ICE stands for Initial, Change, and Equilibrium. It's a method to keep track of the concentrations (or in this case, pressures) of the reactants and products.

Initial pressures: [H2S] = 0.142 atm, [H2] = 0, [S] = 0

Change in pressures: [H2S] decreases by x, [H2] increases by x, [S] increases by x

Equilibrium pressures: [H2S] = 0.142 - x, [H2] = x, [S] = x

Step 4: Substitute the equilibrium pressures into the Kp expression 0.887 = x*x / (0.142 - x)

Step 5: Solve for x This is a quadratic equation, and solving it gives x = 0.099 atm

Step 6: Calculate the total pressure at equilibrium The total pressure is the sum of the pressures of all gases present, so it's the sum of the equilibrium pressures of H2S, H2, and S.

Total pressure = [H2S] + [H2] + [S] = (0.142 - 0.099) + 0.099 + 0.099 = 0.241 atm

So, the total pressure in the container at equilibrium is 0.241 atm.