Final answer:
In chemical kinetics, the rate of consumption of Reactants is related to the formation of Products through rate laws, which are based on the concentrations of reactants and the stoichiometric coefficients of a balanced chemical equation.
Step-by-step explanation:
The equations that relate the rates of consumption of the reactants and the rates of formation of the products in a chemical reaction are determined by the stoichiometry of the balanced chemical equation. These rates can be expressed as rate laws, which often manifest in terms of the molar concentrations of the reactants and the coefficients from the balanced equation.
For example, consider a generic reaction aA + bB → cC + dD, where lowercase letters represent the stoichiometric coefficients, and uppercase letters represent the reactants and products. The rate of reaction is generally proportional to the concentration of the reactants raised to a power. The rate equation for the consumption of A would be rate = -k[A]^m and for the formation of C, it would be rate = k'[C]^n, where k and k' are the rate constants for the reaction, and m and n depend on the reaction mechanism. Often for elementary reactions, m and n are the same as the stoichiometric coefficients. Note that the negative sign indicates consumption.
If we consider a balanced chemical equation with state symbols, say 2H2(g) + O2(g) → 2H2O(l), the rate of consumption for hydrogen would be rate = -k[H2]^2, since the coefficient is 2, indicating that the rate of consumption is proportional to the square of the hydrogen's concentration. The rate of formation for water would be rate = k'[H2O], that implies the rate of formation is directly proportional to the concentration of water.