Page 1 of 1
Posted: Thu Jan 23, 2020 5:41 pm
Why does temperature affect the K? Does increasing heat for an exothermic reaction shift it to the reactants or products?
Posted: Thu Jan 23, 2020 5:43 pm
For exothermic reaction, increasing the temperature will decrease the K, while for endothermic, increasing the temperature will increase the k
Posted: Thu Jan 23, 2020 6:03 pm
For an exothermic reaction (ΔH is negative), K decreases with an increase in temperature. Increasing the temperature causes the equilibrium to shift to the left.
For an endothermic reaction (ΔH is positive), K increases with an increase temperature.
Posted: Thu Jan 23, 2020 6:25 pm
Temperature can be thought of as a reactant. If adding heat to a reaction, it will favor whichever direction has the positive change in H. This is because forming more of the "energy rich" molecule will harness more of the heat to minimize the net change of temperature of the environment. This is Le Chatelier's principle that reactions will try to minimize change when induced under some sort of stress.
Posted: Fri Jan 24, 2020 12:00 am
Increasing temperature decreases k for an exothermic reaction (which releases energy), and increasing temperature increases k for an endothermic reaction (which requires energy).
Posted: Fri Jan 24, 2020 1:39 pm
heat can be considered a product (in an exothermic reax) or a reactant (in an endothermic reax), and thus adding or removing heat can cause the reaction to shift
Posted: Fri Jan 24, 2020 9:44 pm
Increasing and decreasing temperature changes the value of K because it acts as either a product or reactant (exothermic or endothermic respectively)