The tabulated data were collected for this reaction: 2 NO2(g) + F2(g) → 2 NO2F(g). Write an expression for the reaction rate law and calculate the value of the rate constant, k. What is the overall order of the reaction?

Verified step by step guidance

1. <insert step 1: Identify the general form of the rate law for the reaction. The rate law is typically expressed as: rate = k [NO_2]^m [F_2]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to NO_2 and F_2, respectively.>
2. <insert step 2: Use the experimental data to determine the reaction orders m and n. This is done by comparing the changes in concentration and the corresponding changes in the reaction rate.>
3. <insert step 3: Once the reaction orders m and n are determined, substitute them back into the rate law expression.>
4. <insert step 4: Use the experimental data to calculate the rate constant k. Choose one set of experimental data, substitute the concentrations and the rate into the rate law, and solve for k.>
5. <insert step 5: Determine the overall order of the reaction by adding the reaction orders m and n. The overall order is the sum of the exponents in the rate law expression.>