H+D2 → HD+D is the exchange of isotopes of hydrogen of atomic mass 1 (H) and 2 (D, deuterium). The following data were obtained for the rate constant k of this reaction: Temperature (K) k (L mol¬1 s-1) 299 1.56 x 104 327 3.77 x 104 346 7.6 x 104 440 106 549 1.07 x 106 745 8.7 x 107 (a) Calculate the activation energy of this reaction. (b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant.

Find the rate law equation and the value of k.

The reaction 2A--->P has a rate constant k= 3.50 x 10-4 dm6 mol-2s-1What is the order of this reaction? Why?

6

-1 For a certain reaction, the frequency factor A is 7.5 × 10⁹ s1 and the activation energy is 21.4 What is the rate constant for the reaction at 95. °C? Round your answer to 2 significant digits. Note: Reference the Fundamental constants table for additional information. k = -1 S X kJ mol S

The following data were obtained at constant temperature for the reaction: 4A(g) + 4B (g) → 3C(g) Initial [A] Initial [B] mol Experiment mol mol Initial Rate L-min L L 1 0.105 0.215 4.50 2 0.315 0.215 13.5 3 0.105 0.430 18.0 4 0.315 0.430 54.0 Part 1 of 2 Select the single best expression for the rate law for the reaction. Ok [A]³ [B]³ G Ok [A] [B] Ok [A] [B] Ok [A][B]²