The equillibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121:
PCl5(g) --> PCl3(g) + Cl2(g)
A vessel is charged with PCl5, giving a initial pressure of 0.123 atm. At equillibrium, the partial pressure of PCl3 is _____ atm.
.........PCl5 ==> PCl3 + Cl2
initial...0.123.....0.......0
change...-2p........p.......p
equil...0.123-2p.....p......p
Substitute the equilibrium values into the expression for Kp and solve for p.
Post your work if you get stuck.
.0330
To find the partial pressure of PCl3 at equilibrium, we can use the equilibrium constant (Kp) expression. The equilibrium constant expression for the given reaction is:
Kp = [PCl3] * [Cl2] / [PCl5]
Since we are given the value of Kp as 0.0121, we can substitute the initial and equilibrium partial pressures of PCl5, PCl3, and Cl2 into the expression:
Kp = (PCl3(eq) * Cl2(eq)) / PCl5(0)
We know the initial pressure of PCl5 is 0.123 atm, so we can substitute that into the equation:
0.0121 = (PCl3(eq) * Cl2(eq)) / 0.123
Assuming the concentrations of PCl3 and Cl2 at equilibrium are x, we can rewrite the equation as:
0.0121 = (x * x) / 0.123
Simplifying the equation, we have:
0.0121 = x^2 / 0.123
To solve for x, we can rearrange the equation:
0.0121 * 0.123 = x^2
0.0014963 = x^2
Taking the square root of both sides, we get:
x = √0.0014963
x ≈ 0.0387
Therefore, the partial pressure of PCl3 at equilibrium is approximately 0.0387 atm.
To find the partial pressure of PCl3 at equilibrium, we need to use the equilibrium constant expression and the initial pressure of PCl5.
The equilibrium constant expression for the given reaction is:
Kp = (PCl3 * Cl2) / PCl5
We are given that the equilibrium constant (Kp) is 0.0121. Let's assume that the partial pressure of PCl3 at equilibrium is x atm. Since Cl2 is a product of the reaction, its partial pressure will also be x atm.
Substituting the given values in the equilibrium constant expression, we get:
0.0121 = (x * x) / 0.123
Cross-multiplying the equation, we can rewrite it as:
0.0121 * 0.123 = x^2
Next, solve for x:
x^2 = (0.0121 * 0.123)
x^2 = 0.0014883
Taking the square root of both sides gives:
x ≈ 0.0386 atm
Therefore, the partial pressure of PCl3 at equilibrium is approximately 0.0386 atm.