Module #14: Kinetics

Question 1

What is a Controlled Experiment?

Answer 1

An experiment in which you change only one thing in comparison to the control.

Question 2

What is a Control?

Answer 2

A test done under standard conditions.

Question 3

In order to react, chemicals must ___ with one another so that their electrons can either be transferred or rearranged.

Answer 3

In order to react, chemicals must collide with one another so that their electrons can either be transferred or rearranged.

Question 4

What increases the reaction rate?

Answer 4

1. Higher Temperature - because the reactant molecules (or atoms) move faster, increasing the chance for a collision.
2. Increasing Concentration - because there are more reactant molecules (or atoms) to collide with one another.
3. Increase of Surface Area of Reactants - because the molecules (or atoms) of the reactant can more easily mingle with the molecules (or atoms) of the other reactants.

Question 5

What is the Rate Equation?

Answer 5

R = k [A]^x [B]^y

Question 6

What do the letters/symbols in the Rate Equation stand for?

Answer 6

R = Rate of chemical reaction
[A] = concentration of reactant A
[B] = Concentration of reactant B
K = rate constant for the chemical reaction
x & y = exponents for the concentrations of the reactants, order, x + y = overall order of the chemical reaction
The units for the rate constant vary. They depend on the exponents of the rate equation

Question 7

What is the Instantaneous Rate?

Answer 7

The rate calculated from the rate equation.

Question 8

The rate of many chemical reactions doubles for every ___ increase in temperature

Answer 8

The rate of many chemical reactions doubles for every 10 [degrees] C increase in temperature.

Question 9

The rate constant (k) ____ _____ as long as the temperature remains the same.

Answer 9

The rate constant (k) remains constant as long as the temperature also remains the same.

Question 10

What happens to Catalysts during a reaction?

Answer 10

Catalysts speed up the reaction rate without actually getting used up in the chemical reaction.

Question 11

What occurs when you decreasing the activation energy of a reaction?

Answer 11

Decreasing the activation energy of a reaction increases its rate.

Question 12

How to Catalysts work?

Answer 12

Catalysts speed up reaction rates by lowering the activation energy of the reaction.

Question 13

Define Reaction Rate.

Answer 13

The rate of change of a product in a chemical reaction

Question 14

Define Heterogeneous Catalysts.

Answer 14

Catalysts that are in a different phase than the reactants

Question 15

Define Homogeneous Catalysts.

Answer 15

Catalysts that have the same phase as at least one of the reactants.

Question 16

Define Reaction Mechanism.

Answer 16

A series of chemical equations that tells you the step-by-step process by which a chemical reaction occurs.