If the reaction quotient, Q, for a reaction is less than the value of the equilibrium constant, K, for the reaction at a given temperature what must be converted to work for the system to reach equilibrium?

1 Answer
Feb 27, 2017

Answer:

The equilibrium must move in a forward direction..........

Explanation:

For the reaction,

#A+Brightleftharpoons C+D#,

we write #K_(eq)=([C][D])/([A][B])#

This describes an equilibrium condition, where the rate of forward reaction is equal to the reverse rate of reaction.

Under non-equilibrium conditions, (for instance at the start of the reaction), we write #Q_"rxn quotient"=([C][D])/([A][B])#.

At the start of the reaction, we can conceive that the reactant concentrations, #[A]# and #[B]#, are LARGER than they would be at equilibrium, so #Q_"rxn"# #<# #K_"eq"#, and so the reaction proceeds in a forward direction, until #Q_"rxn"# #=# #K_"eq"#.