Most reactions are reversible Given the reaction A B C and

Most reactions are reversible. Given the reaction: A + B => C and K_eq = 1.5 Which direction does the reaction go? What can you tell about Delta G^0? What is Delta G when the reaction reaches equilibrium?

Solution

4. If Keq = 1.5 which means Keq > 1 then it favours the formation of products since, for the reaction A+B=> C, the

Keq= [C]/[A]x[B], so the product formation is promoted and the reaction will move in the forwars direction.

5. delta G naught means Free energy under standard conditions of products and reactants to be at a concentration of 1M and the atmospheric pressure being 1 atmospheres. Its relationship with delta G is as follows:-

delta G = delta G naught + RTlnKeq

6. delta G becomes 0 at equilibrium since there is no tendency of the reaction to go either forward or backward, the rate of forward reaction is same as the rate of backward reaction.