Final answer:
The rate of formation of product C, based on the stoichiometry of the reaction 2A + B → 3C and given the reaction rate of A and B as 0.005 m/s, should be 0.0075 m/s. However, this does not match any of the provided answer options, indicating a possible error or misunderstanding in the question or options.
Step-by-step explanation:
To find the rate of formation of product C when the overall reaction rate is given, we must consider the stoichiometry of the reaction. The given reaction is 2A + B → 3C. If the rate of formation of A and B is 0.005 m/s, this rate refers to how quickly A and B are being consumed. Since for every 2 molecules of A, 3 molecules of C are produced, the rate of production of C can be found using a stoichiometric factor.
So, the rate of formation of C is (3/2) × rate of formation of A. Using the given reaction rate for A and B (0.005 m/s):
Rate of formation of C = (3/2) × 0.005 m/s = 0.0075 m/s
However, none of the options provided matches 0.0075 m/s. There seems to be a misunderstanding because based on the stoichiometry of the reaction, the rate of formation of product C should be higher than the rate of disappearance of reactants A and B.