True or False: 1) The higher that the activation energy is for a reaction, the g

Question

True or False: 1) The higher that the activation energy is for a reaction, the greater the tendency of the reaction to proceed at a high rate. 2) A catalyst makes a reaction proceed more rapidly by increasing the amount of kinetic energy possessed by colliding reactant particles. 3) A catalyst makes a reaction proceed more rapidly by providing an alternative reaction mechanism which is characterized by a lower activation energy. 4) If a reaction takes place by a two-step mechanism, then the products will be different than if it took place by a single step mechanism. 5) The actual rate expression and reaction order for a given reaction depends upon the mechanism by which the reaction takes place. 6) The step in a reaction mechanism which is slowest is often referred to as the_______step ( rate-determining, catalyzed, highly activated, limiting reactant).

Explanation / Answer

Answer. 1) False.. k = A e-Ea/RT  from this Arrhenius equation we can infer that increase in rate is caused by decrease in energy of activation.

2) False.

3) True .In presence of a catalyst, a reaction proceeds in an alternative pathway with less activation energy.

4) False.

5) True.

6) The step in a reaction mechanism which is slowest is often referred to as the ( rate-determining)step.

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