Variation of equilibrium constant K for the reaction; $2A\left(s\right)+B\left(g\right) \rightleftharpoons C\left(g\right)+2D\left(g\right)$ is plotted against absolute temperature T in figure as $lnKVs(1/T) :$

 

The relation between Equilibrium constant and Temperature is given by Van't Hoff  equation, $\ln K_{eq}=-\frac{\Delta H°}{RT}+\frac{\Delta S°}{R}.$

For the $\ln K_{eq}vs\frac{1}{T}plot,-\frac{\Delta H°}{R}$ is the slope.

The graph suggests positive slope, hence $-\frac{\Delta H°}{R}$ is positive or $\Delta H°$ is negative.Hence, the reaction is exothermic. Slope line is proportional to $\Delta H$ Also, by Le Chatelier's principle, removing C favours forward reaction.