$$ \ce{2XY <--> X2(g) + Y2(g)} \hskip{2em} K_p=230 $$

A certain gas, \(\ce{XY(g)}\), decomposes as represented by the equation above. A sample of each of the three gases is put in a previously evacuated container. The initial partial pressures of the gases are shown in the table below.

$$ \begin{array}{|c|c|} \hline \text{Gas} & \text{Initial Partial } \\ & \text{Pressure (atm)} \\ \hline \hline \ce{XY} & 0.010 \\ \hline \ce{X_2} & 0.20 \\ \hline \ce{Y_2} & 2.0 \\ \hline \end{array} $$

The temperature of the reaction mixture is held constant. In which direction will the reaction proceed?

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Find the reaction quotient and compare it to \(K_p\).

$$ Q = \frac{[\ce{X_2}][\ce{Y_2}]}{[\ce{XY}]^2} $$ $$ Q = \frac{(0.20)(2.0)}{0.010} $$ $$ Q = \frac{.40}{0.0001} $$ $$ Q = 4000 $$

Since \(Q \gt K_p\), the system must shift to the reactant side.