Final

Question 1

What are the conditions listed in the kinetic theory of reactions?

Answer 1

-collisions must have enough energy
-molecules must collide to react
-collisions must have correct orientation

Question 2

These are not the function of a catalyst?

Answer 2

-It increases the activation energy
-It slows down the rate of a reaction
-It is used up during a reaction

Question 3

A reversible reaction is at equilibrium when

Answer 3

the forward reaction rate equals the reverse
reaction rate

Question 4

An equilibrium constant greater than 1 indicates that a reaction mixture at equilibrium most likely contains

Answer 4

Mostly products

Question 5

For the reaction CO (g) + H2O (g) ↔ CO2 (g) + H2 (g) + Heat, if the temperature is decreased, where does the equilibrium
shift?

Answer 5

Shifts right towards the products

Question 6

Using the same equation from question 10, if H2 (g) is added, where does the equilibrium shift?

Answer 6

Shifts left towards the reactants

Question 7

For the following reaction C2H4 (g) + Cl2 (g) ↔ C2H4Cl2 (g) + Heat, if a catalyst is added, where the does the equilibrium
shift?

Answer 7

No change

Question 8

Out of the choices listed, what is true about KOH?

Answer 8

It would increase the pH of a solution

Question 9

Name the following acid, H3PO4

Answer 9

Phosphoric acid

Question 10

For the following equation identify the Bronsted-Lowry acid and the Bronsted-Lowry base

Answer 10

H2O is the acid (proton donor), NH3 is the base
(proton acceptor)

Question 11

Identify if the equilibrium mixture from the previous question contains mostly reactants, products, or an equal amount of
both. Assume H2SO4 has a pKa <1 and H3PO4 has a pKa >1.

Answer 11

Contains mostly products

Question 12

Identify what is true about weak acids

Answer 12

-They have a small Ka value
-They have a large pKa
-They dissociate only slightly in aqueous
solutions

Question 13

Energy stored in an object due to its position (like a holding a ball 5 feet above the ground) is an example of

Answer 13

Potential energy

Question 14

H30 is higher and between (10-7 and 10-0)
OH is lower and between (10-14 and 10-7)

Answer 14

Acidic

Question 15

H30 and OH equals 10-7

Answer 15

Neutral

Question 16

H30 is lower and between (10-14 and 10-7)
OH is higher and between (10-7 and 10-0)

Answer 16

Basic

Question 17

pOH

Answer 17

pH+pOH=14
14-pOH=answer

Question 18

Reactions occur when

Answer 18

bonds break and bonds form

Question 19

Define Catalyst

Answer 19

know catalysts lower the energy of activation, but they do not change the energy difference between reactants and product.

Question 20

Acid

Answer 20

– increases concentration of H+
-Anything that release H+, like HCl, HNO3, H2SO4
-Proton donor

Question 21

Base

Answer 21

– increases concentration of OH-
-Anything that releases OH-, like NaOH, KOH, Ca(OH)2
-Proton acceptor

Question 22

pH scale

Answer 22

1 is more acidic
13 is more basic

Question 23

Acids and Metals

Answer 23

Acids react with metals to produce hydrogen gas and a salt

Question 24

Acids and Carbonates

Answer 24

Acids react with carbonates to produce a salt, carbon dioxide, and water

Question 25

Neutralization Reactions

Answer 25

-Acids react with bases and form a salt and water
-The acid or base is “neutralized”

Question 26

Buffers consist of:

Answer 26

-A weak acid
-A salt containing the conjugate base

Question 27

An equilibrium expression

Answer 27

for a reversible chemical reaction multiplies the concentrations of the products together and divides by the concentrations of the reactants

Question 28

Equilibrium Expression

Answer 28

aA+bB <===> cC+dD

Question 29

Kc=

Answer 29

Products/Reactants

Question 30

What items contribute to changing rate of reaction?

Answer 30

Heat, concentration of reactants, volume, catalysts