The equilibrium constant, KC, for the following reaction is 280 at 1,000 K.2SO2(g) + O2(g) ⇌ 2SO3(g)If [SO2]eq = 0.80 M and [O2]eq = 0.35 M, then [SO3]eq =
Question
The equilibrium constant, KC, for the following reaction is 280 at 1,000 K.2SO2(g) + O2(g) ⇌ 2SO3(g)If [SO2]eq = 0.80 M and [O2]eq = 0.35 M, then [SO3]eq =
Solution
The equilibrium constant (Kc) for the reaction is given by the expression:
Kc = [SO3]^2 / ([SO2]^2 * [O2])
We know that Kc = 280, [SO2]eq = 0.80 M, and [O2]eq = 0.35 M. We need to find [SO3]eq.
Substituting the known values into the expression for Kc, we get:
280 = [SO3]^2 / ((0.80)^2 * 0.35)
To isolate [SO3]^2 on one side of the equation, we multiply both sides by ((0.80)^2 * 0.35):
[SO3]^2 = 280 * ((0.80)^2 * 0.35)
Calculate the right side of the equation:
[SO3]^2 = 280 * (0.64 * 0.35) = 280 * 0.224 = 62.72
Finally, to find [SO3]eq, we take the square root of both sides of the equation:
[SO3]eq = sqrt(62.72) = 7.92 M
So, the equilibrium concentration of SO3 is 7.92 M.
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