Adding heat to an exothermic reaction will have what effect? reactants ↔ products + heat view available hint(s) adding heat to an exothermic reaction will have what effect? reactants ↔ products + heat no effect and k doesn't change. causes the equilibrium to shift to the left, in favor of making more reactants, and k decreases causes the equilibrium to shift to the right, in the direction of making more reactants, and k increases. causes the equilibrium to shift to the right, in the direction of making more products, and k increases.

Causes the equilibrium to shift to the left, in favor of making more reactants, and K decreases.

Explanation:

Le Châtelier's principle states that if there is a stress in equilibrium, the reaction will shift to restore the equilibrium. An exothermic reaction loses heat for the surroundings, so the equilibrium must be represented as:

Reactants ⇔ Products + Heat

Then, when more heat is added, to restore the equilibrium, the reaction shift to the left ("consuming" heat), in favor of making more reactants.

The equilibrium constant (K) is:

K = [Products]/[Reactants]

So, [Reactants] will increase, and K must decrease.

"record the time to complete a chemical reaction" would most likely be part of a lab procedure.