Question

Part A

For a certain reaction, Kc = 9.48×10⁶ and kf= 2.19×10³M−2⋠s−1 . Calculate the value of the reverse rate constant, kr, given that the reverse reaction is of the same molecularity as the forward reaction.

Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M−2⋠s−1 include ⋠(multiplication dot) between each measurement.

Part B

For a different reaction, Kc = 1.09×10⁶, kf=6.68×103s−1, and kr= 6.14×10^−3 s−1 . Adding a catalyst increases the forward rate constant to 2.95×10⁶ s−1 . What is the new value of the reverse reaction constant, kr, after adding catalyst?

Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M−2⋠s−1 include ⋠(multiplication dot) between each measurement.

Part C

Yet another reaction has an equilibrium constant Kc=4.32×10^5 at 25 ∘C. It is an exothermic reaction, giving off quite a bit of heat while the reaction proceeds. If the temperature is raised to 200 ∘C , what will happen to the equilibrium constant?