Homework 2

[906023369]

Why on questions 7 and 8 it states that if the temperature increases Q will be greater than and less than K?

[Sabrina_Huang_1K]

If I'm not mistaken, you're talking about the week 1 Achieve problem set. So for endothermic reactions, K decreases when temperature increases and for exothermic reactions, K decreases when temperature increases. So from what we learned in class regarding enthalpies and equilibrium's response to changes in temperatures, we know that a positive delta H indicates an endothermic reaction. Endothermic reactions will favor product formations when temperature increases therefore, when the temperature is increased for endothermic reactions, Q<K because K increases because K = [P]/[R] and when P increases, K increases.

The opposite can be said about exothermic reactions. For exothermic reactions, the formation of reactants is favored when temperature increases. So for exothermic reactions (when delta H is negative) Q>K because K has decreased because K = [P]/[R] and when R increase K decreases.