The equilibrium constant, Kc, for the following reaction is 1.54E-2 at 643 K.
2HI(g) H2(g) + I2(g)
When a sufficiently large sample of HI(g) is introduced into an evacuated vessel at 643 K, the equilibrium concentration of I2(g) is found to be 0.351 M.
Calculate the concentration of HI in the equilibrium mixture. ___M
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To calculate the concentration of HI in the equilibrium mixture, we can use the equilibrium constant expression and the given information. The equilibrium constant expression for the given reaction is as follows:
Kc = [H2][I2] / [HI]^2
We are given the equilibrium constant (Kc = 1.54E-2) and the concentration of I2 in the equilibrium mixture ([I2] = 0.351 M). We need to calculate the concentration of HI ([HI]).
First, let's substitute the known values into the equilibrium constant expression:
1.54E-2 = [H2][0.351] / [HI]^2
Now, let's rearrange the equation to solve for [HI]:
[HI]^2 = ([H2] * 0.351) / 1.54E-2
To find the concentration of HI in the equilibrium mixture, we need to take the square root of both sides:
[HI] = √(([H2] * 0.351) / 1.54E-2)
Unfortunately, we don't have the concentration of H2 ([H2]) in the given information. Therefore, we can't calculate the concentration of HI without additional data.
To find the concentration of HI, we need either the value of [H2] or alternate information about the reaction, such as the initial or equilibrium concentrations of the reactants.