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Question 1. Identify the species that is oxidized and the species that is reduced in the reaction: 2 I – + Cl 2  2 Cl – + I 2 A) I – is oxidized and Cl 2 is reduced . B ) Cl 2 is oxidized and I – is reduced . C) I 2 is oxidized and Cl – is reduced .

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question 1
Question 1

Identify the species that is oxidized and the species that is reduced in the reaction:

2 I– + Cl22 Cl– + I2

A) I– is oxidized and Cl2 is reduced.

B) Cl2 is oxidized and I– is reduced.

C) I2 is oxidized and Cl–is reduced.

D) Cl2 is oxidized and Cl–is reduced.

E) I2 is oxidized and I–is reduced.

question 11
Question 1

Identify the species that is oxidized and the species that is reduced in the reaction:

2 I– + Cl22 Cl– + I2

A) I– is oxidized and Cl2 is reduced.

B) Cl2 is oxidized and I– is reduced.

C) I2 is oxidized and Cl–is reduced.

D) Cl2 is oxidized and Cl–is reduced.

E) I2 is oxidized and I–is reduced.

question 2
Question 2

What is the expression for the equilibrium constant for the reaction

2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g)?

A)K= [CO2][H2O] B) K = [CO2]4[H2O]6

[C2H6][O2] [C2H6]2[O2]7

C) K= [C2H6][O2] D) K = [C2H6]2[O2]7

[CO2][H2O] [CO2]4[H2O]6

question 21
Question 2

What is the expression for the equilibrium constant for the reaction

2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g)?

A)K= [CO2][H2O] B) K = [CO2]4[H2O]6

[C2H6][O2] [C2H6]2[O2]7

C) K= [C2H6][O2] D) K = [C2H6]2[O2]7

[CO2][H2O] [CO2]4[H2O]6

question 3
Question 3

The definition of a Brønsted-Lowry acid is:

A) a compound that contains hydroxide and dissolves in water to form –OH.

B) a compound that is a proton donor.

C) a compound that is a proton acceptor.

D) a compound that contains a hydrogen atom and dissolves in water to form a hydrogen ion, H+.

question 31
Question 3

The definition of a Brønsted-Lowry acid is:

A) a compound that contains hydroxide and dissolves in water to form –OH.

B) a compound that is a proton donor.

C) a compound that is a proton acceptor.

D) a compound that contains a hydrogen atom and dissolves in water to form a hydrogen ion, H+.

question 4
Question 4

An alpha particle is a high-energy particle that contains:

A) one proton and one neutron.

B) two protons and two neutrons.

C) one electron.

D) one proton.

question 41
Question 4

An alpha particle is a high-energy particle that contains:

A) one proton and one neutron.

B) two protons and two neutrons.

C) one electron.

D) one proton.

question 5
Question 5

In the balanced redox reaction:

2 Cu(s) + S(s)  Cu2S(s)

how many electrons are gained or lost by each sulfur atom?

A) each sulfur atom gains two (2) electrons

B) each sulfur atom gains one (1) electron

C) each sulfur atom loses one (1) electron

D) each sulfur atom loses two (2) electrons

question 51
Question 5

In the balanced redox reaction:

2 Cu(s) + S(s)  Cu2S(s)

how many electrons are gained or lost by each sulfur atom?

A) each sulfur atom gains two (2) electrons

B) each sulfur atom gains one (1) electron

C) each sulfur atom loses one (1) electron

D) each sulfur atom loses two (2) electrons

question 6
Question 6

An equilibrium constant with a value of 4.6 x 1015 indicates that at equilibrium

A) the reactants are favored.

B) the products are favored.

C) approximately equal concentrations of reactants and products are present.

question 61
Question 6

An equilibrium constant with a value of 4.6 x 1015 indicates that at equilibrium

A) the reactants are favored.

B) the products are favored.

C) approximately equal concentrations of reactants and products are present.

question 7
Question 7

Which species can be a Brønsted–Lowry acid?

A) CO32–

B) HBr

C) Br2

D) LiOH

question 71
Question 7

Which species can be a Brønsted–Lowry acid?

A) CO32–

B) HBr

C) Br2

D) LiOH

question 8
Question 8

Which species is the conjugate acid of HCO3–?

A) CO32–

B) H2CO3

C) CO2

D) H2O

question 81
Question 8

Which species is the conjugate acid of HCO3–?

A) CO32–

B) H2CO3

C) CO2

D) H2O

question 9
Question 9

Which is the symbol for the beta particle?

A) 1e

0

B) 1e

-1

C) 0e

-1

D) 0e

1

question 91
Question 9

Which is the symbol for the beta particle?

A) 1e

0

B) 1e

-1

C) 0e

-1

D) 0e

1

question 10
Question 10

In the balanced redox reaction:

2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g), which species is reduced?

A) C2H6(g)

B) O2(g)

C) CO2(g)

D) H2O(g)

question 101
Question 10

In the balanced redox reaction:

2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g), which species is reduced?

A) C2H6(g)

B) O2(g)

C) CO2(g)

D) H2O(g)

question 111
Question 11

In the galvanic cell created using zinc and copper placed in zinc sulfate and copper (II) sulfate solutions respectively, which species forms the anode of the cell?

A) Zinc

B) Zinc sulfate

C) Copper

D) Copper sulfate

Reduction ReactionE0 (v)

Zn2+ (aq) + 2e- Zn (s) -0.76

Cu2+ (aq) + 2e-  Cu (s) +0.34

question 112
Question 11

In the galvanic cell created using zinc and copper placed in zinc sulfate and copper (II) sulfate solutions respectively, which species forms the anode of the cell?

A) Zinc

B) Zinc sulfate

C) Copper

D) Copper sulfate

Reduction ReactionE0 (v)

Zn2+ (aq) + 2e- Zn (s) -0.76

Cu2+ (aq) + 2e-  Cu (s) +0.34

question 12
Question 12

What is the correct cell notation for the zinc/copper cell described in the previous question?

A) Cu|Zn||Cu2+|Zn2+

B) Cu|Cu2+||Zn2+|Zn

C) Zn|Zn2+||Cu2+|Cu

D) Zn2+|Zn||Cu|Cu2+

Reduction ReactionE0 (v)

Zn2+ (aq) + 2e- Zn (s) -0.76

Cu2+ (aq) + 2e-  Cu (s) +0.34

question 121
Question 12

What is the correct cell notation for the zinc/copper cell described in the previous question?

A) Cu|Zn||Cu2+|Zn2+

B) Cu|Cu2+||Zn2+|Zn

C) Zn|Zn2+||Cu2+|Cu

D) Zn2+|Zn||Cu|Cu2+

Reduction ReactionE0 (v)

Zn2+ (aq) + 2e- Zn (s) -0.76

Cu2+ (aq) + 2e-  Cu (s) +0.34

question 13
Question 13

For an endothermic reaction, increasing the temperature

A) does not shift the equilibrium since K is a constant.

B) increases the rate of the reverse reaction to form more reactants.

C) increases the rate of the forward reaction to form more products.

D) increases the rate of the reverse reaction to form more products.

question 131
Question 13

For an endothermic reaction, increasing the temperature

A) does not shift the equilibrium since K is a constant.

B) increases the rate of the reverse reaction to form more reactants.

C) increases the rate of the forward reaction to form more products.

D) increases the rate of the reverse reaction to form more products.

question 14
Question 14

Which acid is the strongest?

A) Hydrogen sulfate ion HSO4– (Ka = 1.2 x10–2)

B) Hydrocyanic acid HCN (Ka = 4.9 x10–10)

C) Hydrofluoric acid HF (Ka = 7.2 x10–4)

D) Ammonium ion NH4+ (Ka = 5.6 x10–10)

question 141
Question 14

Which acid is the strongest?

A) Hydrogen sulfate ion HSO4– (Ka = 1.2 x10–2)

B) Hydrocyanic acid HCN (Ka = 4.9 x10–10)

C) Hydrofluoric acid HF (Ka = 7.2 x10–4)

D) Ammonium ion NH4+ (Ka = 5.6 x10–10)

question 15
Question 15

If the half-life of phosphorus-32 is 14 days, how much of a 300. mg sample of phosphorus-32 remains after 56 days?

A) 150. mg

B) 37.5 mg

C) 18.8 mg

D) 9.38 mg

question 151
Question 15

If the half-life of phosphorus-32 is 14 days, how much of a 300. mg sample of phosphorus-32 remains after 56 days?

A) 150. mg

B) 37.5 mg

C) 18.8 mg

D) 9.38 mg