Kinetics

Question 1

Describe 0 order reactions

Answer 1

Proceeds at a constant rate independent of concentration. rate = k, typically using a catalyzed reaction @ saturation.

Temperature and catalyst are the only things that can change the reaction.

Question 2

Describe first order reactions

Answer 2

Dependent on only one of the reactants. rate= k[R], changes linearly; decreasing. the rate constant k, is the slope of the line. Just add a (-) at the end.

Question 3

Describe second order reactions

Answer 3

Dependent on two reactants. rate = k[r]^2, changes exponentially.

Question 4

How do you define the rate of a reaction?

Answer 4

change in concentration / change in time.

Question 5

How do you calculate the rate constant k for a given experiment.

Answer 5

First, find the rate equation and then plug in the experimental data.

Question 6

What are the requirements of collision theory?

Answer 6

1. Proper Orientation. 2. Must collide. 3. Must have enough activation energy.

Question 7

How are exothermic and endothermic reactions represented on a graph.

Answer 7

Endothermic, the products are higher in energy. Exothermic, the products are lower in energy.

Question 8

What is the Arrhenius equation?

Answer 8

Question 9

How can you change the rate constant in the Arrhenius equation, and therefore increase the rate of the reaction?

Answer 9

Decrease Ea, or increase temperature.

Question 10

When is the only time you’re able to use the coefficient in the balanced equation for the exponent in the rate law?

Answer 10

When it’s a singular, elementary, reaction either unimolecular or bimolecular. This does not work with multi step reactions.

Question 11

What is the rate determining step of a reaction?

Answer 11

The slowest step. The rate determining step also determines what will go into the overrall rate law.