Consider this system at equilibrium. A(aq)<--->B(aq)deltaH=+550 kJ/mol What can be said about Q and K immediately afteran increase in temperature? A) Q > K because Q increased B) Q > K because K decreased C) Q < K because Q decreased D) Q< K because K increased E) Q = K because neither charged How will the system respond to a temperature increase? A) shift left B) shift right C) no change

Q < K because K increased

The system will SHIFT TO THE RIGHT

Explanation:

First, the reaction is endothermic. That is, a reaction in which heat is absorbed from the surroundings. ΔH is positive for endothermic reactions.

At the addition of temperature, the system absorbed more heat causing more products to be formed, shifting the equilibrium to the right.

The equilibrium constant k will therefore increase as the concentration of product increases

K = [B] / [A].