Final answer:
The rate of formation for products D, E, and F can be expressed in terms of the rate of disappearance of reactant A, adjusted by their stoichiometric coefficients: Rate of formation of D = (1/3) * Rate of A, Rate of formation of E = Rate of A, and Rate of formation of F = (4/3) * Rate of A. These relationships reflect the stoichiometry of the balanced chemical equation.
Step-by-step explanation:
The question requires the expression of the rate of product formation for the reaction:
A + 2 B + 3 C → D + 3 E + 4 F
Since the reaction is homogeneous and involves multiple reactants and products, the rate of formation of each product can be expressed relative to the rate of disappearance of the reactants, taking the stoichiometry of the reaction into consideration. For a balanced reaction, the rate of formation of products is directly proportional to the rate of consumption of reactants. Therefore, we can write the following expressions:
- Rate of formation of D = (1/3) * Rate of disappearance of A
- Rate of formation of E = Rate of disappearance of A
- Rate of formation of F = (4/3) * Rate of disappearance of A
This is because for every 1 mole of A consumed, 1 mole of D, 3 moles of E, and 4 moles of F are produced. Therefore, the rate of formation is adjusted according to the stoichiometric coefficients. The actual rates can then be found using the rate law for the reaction, which typically takes the form of a rate constant multiplied by the concentrations of the reactants raised to their respective powers (which are determined experimentally).
Note: The coefficients in the stoichiometric equation dictate the ratios of the rate of consumption and formation. Due to the different coefficients, we need to divide the rates of formation of D, E, and F by the respective stoichiometric coefficients of A (in their simplest whole number ratios) to maintain the balance as dictated by the law of conservation of mass.