Chemistry

Warren

6 July, 23:21

Use the rate constants for the forward and reverse reactions to determine whether reactants or products

are favored at equilibrium in this case:

kforward

Keq = kreverse

When Kea < 1, the equilibrium lies to the left (reactants are favored).

When Keq > 1, the equilibrium lies to the right (products are favored)

When Keo = 1, neither reactants nor products are favored.

kforward = 1.5 x 10-5

kreverse = 2.2 x 10-3

1) Reactants are favored.

2) Products are favored.

3) Both are equal.