Question

Consider the following equilibrium reaction:

2ICl(g) (reverse reaction symbol) I2(g) + Cl2(g)
Some ICl is added to an empty flask. How do the reaction rates change as the system approaches equilibrium?

a. forward rate increases, reverse rate increases.
b. forward rate increases, reverse rate decreases.
c. forward rate decreases, reverse rate increases.
d. forward rate decreases, reverse rate decreases.

Answer 1

I think the correct answer would be forward rate increases, reverse rate decreases. As more of the reactants are added to the flask, the formation of more products would be favored thus the forward rate increases which consequently decreases the reverse rate. Hope this helps.

Answer 2

The correct option is C. This is because as the chemical reaction moves toward equilibrium, the concentration and the reaction rate of ICI decrease while the concentration and the reaction rate of I2 and CI2 increase.