At a certain temperature, the equilibrium constant, K, for this reaction is 53.3.
H2(g)+I2(g)->2HI(g)
At this temperature, the reactants were placed in a container to react. If the partial pressures of H2 and I2 were each 0.300 bar initially, what is the partial pressure of HI at equilibrium?
To find the partial pressure of HI at equilibrium, we need to use the equilibrium constant expression and the given partial pressures of H2 and I2.
The equilibrium constant expression for the given reaction is as follows:
K = ([HI]^2) / ([H2] * [I2])
We can rearrange this expression to solve for [HI]:
[HI]^2 = K * ([H2] * [I2])
Substituting the given values:
K = 53.3
[H2] = 0.300 bar
[I2] = 0.300 bar
Plugging in these values, we get:
[HI]^2 = 53.3 * (0.300 * 0.300)
Solving this equation gives us:
[HI]^2 = 4.797
[HI] = √4.797
Taking the square root of 4.797 gives us:
[HI] ≈ 2.190
Therefore, the partial pressure of HI at equilibrium is approximately 2.190 bar.
To find the partial pressure of HI at equilibrium, we can use the principle known as the equilibrium expression. The equilibrium expression for this reaction is:
K = [HI]^2 / ([H2] * [I2])
Given that K is 53.3, and the initial partial pressures of H2 and I2 are both 0.300 bar, we need to find the partial pressure of HI at equilibrium.
Let's denote the partial pressure of HI at equilibrium as "x". Since 2 moles of HI are produced for every mole of H2 and I2 that react, the equilibrium partial pressure of HI can be expressed as 2x.
Substituting the known values into the equilibrium expression, we have:
53.3 = (2x)^2 / (0.300 * 0.300)
Now, let's solve for "x":
53.3 = 4x^2 / 0.090
Rearranging the equation:
4x^2 = 53.3 * 0.090
4x^2 = 4.797
Dividing by 4:
x^2 = 1.19925
Taking the square root of both sides:
x = √1.19925
x ≈ 1.095
Therefore, the partial pressure of HI at equilibrium is approximately 1.095 bar.
..........H2 + I2 --> 2HI
I........0.3...0.3.....0
C.......-x....-x.......x
E.....0.3-x..0.3-x.....x
Substitute the E line into the Kp expression and solve for x = p and 0.3-x