For the reaction\ $\mathrm{CO}_{(\mathrm{g})}+\mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})} ightleftha

Question

For the reaction\ $\mathrm{CO}_{(\mathrm{g})}+\mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})} ightleftharpoons \mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})}$\ at a given temperature the equilibrium amount of $\mathrm{CO}_{2(\mathrm{~g})}$ can be increased by\

Professor PC Thomas Classes · Answer

(d): $\mathrm{CO}_{(\mathrm{g})}+\mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})} ightleftharpoons$ $$ K_{c}=\frac{\left[\mathrm{CO}_{2}ight]\left[\mathrm{H}_{2}ight]}{[\mathrm{CO}]\left[\mathrm{H}_{2} \mathrm{O}ight]} $$ Catalyst has no effect on point of equilibrium.\ Addition of inert gas has no effect on equilibrium because $\Delta n=0(2-2=0)$.\ Since, $\Delta n=0$ so the equilibrium is not affected by change in volume.\ If the amount of $\mathrm{CO}_{(g)}$ is increased, $K_{c}$ will decrease, but since temperature is constant and so the value of $K_{c}$ remains unchanged. To maintain constancy of $K_{c}$ the amount of $\mathrm{CO}_{2}$ will increase if we increase the amount of CO.\