At a certain temperature, the Kp for the decomposition of H2S is 0.791.
H2S<--> H2 + S
Initially, only H2S is present at a pressure of 0.111 atm in a closed container. What is the total pressure in the container at equilibrium?
Please Help!
We need the phases.
Is that H2S(g) ==> H2(g) + S(g) or S(s)
I assume H2S(g) ==> H2(g) + S(g)
I........0.111.......0.......0
C.........-x.........x.......x
E.......0.111-x.....x........x
Kp = 0.791 = p(H2)*p(S)/p(H2S)
Solve for x = p(H2) = p(S)
p(H2S) = 0.111-x
Then Ptotal = p(H2) + p(S) + p(H2S)
To solve this problem, we can use the concept of equilibrium and the equilibrium constant (Kp) to find the total pressure at equilibrium. Here's how you can approach it:
Step 1: Write the balanced chemical equation for the decomposition of H2S:
H2S <--> H2 + S
Step 2: Set up the partial pressure expressions for each species involved in the equilibrium:
P(H2S) = 0.111 atm (given)
P(H2) = ?
P(S) = ?
Step 3: Use the equilibrium constant expression to relate the partial pressures of the species:
Kp = (P(H2) * P(S)) / P(H2S)
Step 4: Rearrange the equation and solve for P(H2) * P(S):
P(H2) * P(S) = Kp * P(H2S)
Step 5: Substitute the given values into the equation:
P(H2) * P(S) = 0.791 * 0.111
Step 6: Since we know that at equilibrium the total pressure is equal to the sum of the partial pressures, we can write:
Total pressure = P(H2) + P(S)
Step 7: Substitute the value of P(H2) * P(S) from Step 5 into the equation from Step 6:
Total pressure = P(H2) + P(S) = 0.791 * 0.111
Step 8: Solve the equation to find the total pressure at equilibrium.
By following these steps, you should be able to calculate the total pressure at equilibrium for the given reaction.