Final answer:
To calculate the total pressure in the container at equilibrium, we need to find the equilibrium pressure of H₂S, H₂, and S.
Step-by-step explanation:
To determine the total pressure in the container at equilibrium, we need to calculate the equilibrium pressure of each species in the reaction. Given that the Kp for the decomposition of H₂S is 0.739, we can use the equation: H₂S(g) ⇌ H₂(g) + S(g). Initially, only H₂S is present at a pressure of 0.155 atm in a closed container.
Let's assume that the equilibrium pressure of H₂S is x atm and the equilibrium pressures of H₂H2 and S are y atm and z atm, respectively. According to the stoichiometry of the reaction, the change in pressure for H₂S is equal to the sum of the changes in pressure for H₂ and S. Therefore, we can write the equation: 0.155 - x = y + z.
Since the value of Kp is equal to (y * z)/(x), we can rearrange the equation to solve for y and z in terms of x: y = (Kp * x)/z and z = (Kp * x)/y. Substituting these values into the equation from step 2 and simplifying, we get: 0.155 - x = (Kp * x)/y + (Kp * x)/z. By solving this equation simultaneously with the two equations from step 3, we can determine the equilibrium pressure of each species and find the total pressure in the container at equilibrium.