For the non-stoichiometric reaction 2A + B → C + D, the following kinetic data were obtained in three separate experiments, all at 298 K. The rate law for the formation of C is:

To determine the rate law, we need to analyze the given kinetic data. The general rate law for this reaction is of the form: Rate = k[A]^x[B]^y where k is the rate constant, x is the order with respect to A, and y is the order with respect to B.

We need experimental data (concentrations of A and B and the corresponding reaction rates) to determine x and y. Unfortunately, this data is missing from the provided input. Without the experimental data, we cannot determine the rate law. The options provided are possible rate laws, but we need data to determine which one is correct. A method to solve this would involve comparing reaction rates at different concentrations to determine the order of each reactant. For instance, if doubling the concentration of A doubles the rate, then the reaction is first order with respect to A. If doubling the concentration of A quadruples the rate, then the reaction is second order with respect to A. The same process would be repeated for reactant B.