The chemical equation for this equilibrium reaction is CH4 + H2O ⇌ CO + 3H2, where the reactants (CH4 and H2O) are in equilibrium with the products (CO and 3H2).
The equilibrium constant (K) for this reaction can be determined by taking the ratio of the concentrations of the products to the concentrations of the reactants, with each concentration raised to the power of its coefficient in the balanced chemical equation. In this case, the equilibrium constant expression would be K = [CO][H2]^3 / [CH4][H2O].
The equilibrium of this reaction is affected by temperature according to Le Chatelier's principle. An increase in temperature will shift the equilibrium towards the products, while a decrease in temperature will shift it towards the reactants. This is because the forward reaction is exothermic, meaning it releases heat, so an increase in temperature will favor the endothermic reverse reaction to absorb the excess heat.
A catalyst is a substance that speeds up the rate of a chemical reaction without being consumed in the process. In this equilibrium reaction, a catalyst can increase the rate of both the forward and reverse reactions, helping the reaction reach equilibrium faster. However, it does not affect the position of equilibrium or the equilibrium constant.
To manipulate the equilibrium of this reaction to favor the products, you can either increase the concentration of the products or decrease the concentration of the reactants. This can be achieved by adding more CO or 3H2 to the reaction mixture, or by removing CH4 or H2O from the mixture. Alternatively, you can decrease the volume of the reaction container or increase the temperature, both of which will shift the equilibrium towards the products according to Le Chatelier's principle.