Exam 2 True/False Practice

Question 1

The temperature dependence of the reaction rate is contained in the rate constant, k

Answer 1

true

Question 2

An increase in temperature generally decreases k, which increases rate of reaction

Answer 2

false

Question 3

The frequency factor, A, can be thought of as the number of times that the reactants approach the activation barrier per unit time

Answer 3

true

Question 4

The exponential factor in the Arrhenius equation represents the fraction of molecules that have enough energy to make it over the activation barrier on a given approach.

Answer 4

true

Question 5

The transition state is found at the bottom after an activation energy “hill”

Answer 5

false

Question 6

As temperature decreases, the exponential factor of the Arrhenius equation increases

Answer 6

false

Question 7

Catalytic hydrogenation of an alkene by platinum is an example of heterogeneous catalysis.

Answer 7

true

Question 8

Sucrase is an enzyme that catalyzes the breaking up of table sugar into glucose and fructose by weakening the connecting bond

Answer 8

true

Question 9

catalyst provides a pathway that reduces the activation energy compared to the rate-limiting step for a reaction

Answer 9

true

Question 10

The catalytic destruction of ozone by Cl is an example of homogenous catalysis.

Answer 10

true

Question 11

When K&raquo_space; 1, the forward reaction is favored and there will be a relatively high concentration of products

Answer 11

true

Question 12

At a given temperature, all combinations of starting concentrations will produce the same set of equilibrium concentrations because the value of K is constant for a given temperature

Answer 12

false

Question 13

reaction is reversible if it can proceed in both the forward and reverse directions

Answer 13

true

Question 14

When a reaction reaches equilibrium, the concentration of products and reactants are equal

Answer 14

false

Question 15

When a reaction reaches equilibrium, the forward and reverse reactions stop

Answer 15

false

Question 16

Kp = Kc
for CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g)

Answer 16

true

Question 17

Kp = Kc
for PCl5(g) –> PCl3(l) + Cl2(g)

Answer 17

true

Question 18

Kp = PI2 / PI2
for I2(g) 2 I(g)

Answer 18

true

Question 19

Kc = [I]2 / [I2]
for I2(g) -> 2 I(g)

Answer 19

true

Question 20

If Kc = 6.26 x 10–22 at 25˚C
for I2(g) -> 2 I(g),
then Kp = 1.53 x 10–20 at 25 ˚C.

Answer 20

true

Question 21

HBrO4 is perbromic acid

Answer 21

true

Question 22

HBr is hydrobromic acid

Answer 22

true

Question 23

HIO is hypoiodic acid

Answer 23

false

Question 24

Adding together HClO4 and NaOH produces water and a salt.

Answer 24

true

Question 25

If it requires 60.0 mL of 0.040 M sodium hydroxide solution to completely neutralize 40.0 mL of an unknown triprotic acid, the concentration of the acid is 0.020 M.

Answer 25

true

Question 26

If you accidentally spill a strong acid on your face, you should splash your face with a strong base to neutralize the acid

Answer 26

false

Question 27

According to the Arrhenius definition, a base produces hydroxide in aqueous solution; according to the Brønsted-Lowry definition, an acid is a proton acceptor

Answer 27

false

Question 28

The conjugate base of water is hydroxide

Answer 28

true

Question 29

The conjugate acid of HSO4– is H2SO4

Answer 29

true

Question 30

HNO2(aq) + H2O(l) -> NO2–(aq) + H3O+(aq), nitrous acid and H2O are a conjugate acid-base pair

Answer 30

false

Question 31

Acidity increases as electronegativity increases to the right across a row for binary acids.

Answer 31

true

Question 32

Acidity decreases as bond strength decreases down a column for binary acids.

Answer 32

false

Question 33

Hydroiodic acid is stronger than hydrobromic acid.

Answer 33

true

Question 34

Periodic acid is weaker than perbromic acid

Answer 34

true

Question 35

Bromic acid is weaker than bromous acid

Answer 35

false

Question 36

Nitrite is a stronger base than nitrate

Answer 36

true