Consider this system at equilibrium. A(aq)↽−−⇀B(aq)ΔH=+350 kJ/mol What can be said about Q and K immediately after an increase in temperature? Q < K because Q decreased. Q < K because K increased. Q > K because Q increased. Q > K because K decreased. Q = K because neither changed. How will the system respond to a temperature increase?

A.) Q < K because Q decreased

B. shift right

Explanation:

Reactant>Products

K = Product/Reactant

An endothermic reffers to any reaction which absorbs energy from its surroundings, usually in the form of heat.

ΔH. In endothermic reactions, K increases when Temperature increases.

The given reaction is an endothermic reaction, and in an endothermic reaction, when there is increase in temperature, the product side is more favored. The system will shifts to the right side of the reaction. Q < K then K is constant and Q is decreased.then Q < K because Q decreased

The system respond to a temperature increase by shifting to the right

c (diamond),

sio2 (quartz)

the answer is 0.42 is that is an option. this question provides no info