For 2SO2(g) + O2(g) 2SO3(g), K_c = 100 L mol^-1 at some temperature. A mixture has [SO2] = 0.10, [O2] = 0.20 and [SO3] = 0.50 (all in mol L^-1). The reaction will

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For $2 SO X_{2} (g) + O X_{2} (g) 2 SO X_{3} (g)$ , $K_{c} = 100 L mo l^{- 1}$ at some temperature. A mixture has $[SO X_{2}] = 0.10$ , $[O X_{2}] = 0.20$ and $[SO X_{3}] = 0.50$ (all in $mol L^{- 1}$ ). The reaction will

Q_{c} = [SO X_{3}]^{2} / ([SO X_{2}]^{2} [O X_{2}]) = (0.50)^{2} / ((0.10)^{2} \times 0.20) = 125

. This exceeds

K_{c} = 100

, so

SO X_{3}

decomposes and the net reaction is backward.