Question

For a certain reaction, k c = 2.64×105 and k f = 8.96×104 m −2 ⋅ s −1 . calculate the value of the reverse rate constant, k r , 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 = 1.24×107, kf=8.40×102s−1, and kr= 6.75×10−5 s−1 . adding a catalyst increases the forward rate constant to 3.53×105 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=4.32×105 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?

a.increase

b.decrease

c.not change

Answer 1

b decrease becoz I think it's the best option