1.The equilibrium constant Kc for the reaction of hydrogen with iodine

1.	1.The equilibrium constant Kc for the reaction of hydrogen with iodine is 54.0 at 700 K.#H2(g) + 12(g) = 2 HI(g)#Kc= 54.0 at 700 Ka. If kf is the rate constant for the formation of HI and kr is the rate constant for the decomposition ofHI, deduce whether kf is larger or smaller than kr.
Answer» Answer: 1.The equilibrium constant Kc for the reaction of hydrogen with iodine is 54.0 at 700 K. #H2(G) + 12(g) = 2 HI(g) #Kc= 54.0 at 700 K a. If KF is the rate constant for the formation of HI and kr is the rate constant for the decomposition of HI, deduce whether kf is larger or smaller than kr.

1.The equilibrium constant Kc for the reaction of hydrogen with iodine is 54.0 at 700 K.#H2(g) + 12(g) = 2 HI(g)#Kc= 54.0 at 700 Ka. If kf is the rate constant for the formation of HI and kr is the rate constant for the decomposition ofHI, deduce whether kf is larger or smaller than kr.

Answer»

Answer:

1.The equilibrium constant Kc for the reaction of hydrogen with iodine is 54.0 at 700 K.

#H2(G) + 12(g) = 2 HI(g)

#Kc= 54.0 at 700 K

a. If KF is the rate constant for the formation of HI and kr is the rate constant for the decomposition of

HI, deduce whether kf is larger or smaller than kr.