As the temperature of a reaction is increased, the rate of the reaction increases because the: a) reactant molecules collide less frequently. b) reactant molecules collide with greater energy. c) reactant molecules collide less frequently and with greater energy. d) activation energy is lowered. e) activation energy is increased because of more collisions.

Generally, increasing the temperature increases the rate of a reaction. This is because: O increasing the temperature increases the frequency of collisions O increasing the temperature increases the average energy of the collisions and increases the frequency of collisions O increasing the temperature lowers the activation energy of the reaction increasing the temperature increases the average energy of the collisions.

Collision theory assumes the rate of a reaction depends on a) the energy of collisions. b) the orientation of colliding molecules. Oc) the change in energy between the products and the reactants. d) the change in free energy between the reactants and the products. e) the energy of collisions and the orientation of colliding molecules.

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Which factor, if increased in magnitude, will slow the rate of a reaction. O frequency factor O temperature O activation energy O concentration of a reactant

Which of the following is true?   Decreasing the activation energy decreases the reaction rate. Decreasing the activation energy increases the reaction rate. The activation energy of an exothermic reaction is negative. There is no relationship between activation energy and reaction rate.

When the concentrations of reactant molecules are increased, the rate of reaction increases. The best explanation for this is that as the reactant concentration increases, the activation energy increases. the frequency of molecular collisions increases. the average kinetic energy of molecules increases. the rate constant increases.