Final answer:
To obtain the equation for a reverse reaction, swap the reactants and products of the original reaction. The equilibrium constant for the reverse reaction is the inverse of that for the forward reaction. Rate equations depend on the balanced chemical equation's stoichiometry.
Step-by-step explanation:
To write the equation for the reverse reaction, you essentially need to switch the reactants and the products of the original reaction. For the rates of consumption and formation, the equation will depend on the stoichiometry of the balanced chemical equation. For example, if the reaction is αA + βB → γC + δD, where α, β, γ, and δ represent the stoichiometric coefficients, and A and B are the reactants while C and D are the products, the rate of consumption of A is related to the rate of formation of C by the ratio of their coefficients (α:γ).
For the reverse reaction, the balanced chemical equation would be γC + δD → αA + βB, and the equilibrium constant (K') for the reverse reaction is the inverse of the original equilibrium constant (K). This means that if the original reaction had an equilibrium constant of K, the reverse reaction's equilibrium constant K' would be equal to 1/K.