Transcript Question 1 - Alfred State College
Question 1
A) B) C) D) E) Identify the species that is oxidized and the species that is reduced in the reaction: 2 I – + Cl 2 2 Cl – + I 2 I – is oxidized and Cl 2 is reduced.
I Cl 2 is oxidized and I – 2 is oxidized and Cl – is reduced.
is reduced.
I Cl 2 2 is oxidized and Cl is oxidized and I – – is reduced.
is reduced.
Question 1
A) B) C) D) E) Identify the species that is oxidized and the species that is reduced in the reaction: 2 I – + Cl 2 2 Cl – + I 2 I – is oxidized and Cl 2 is reduced.
I Cl 2 is oxidized and I – 2 is oxidized and Cl – is reduced.
is reduced.
I Cl 2 2 is oxidized and Cl is oxidized and I – – is reduced.
is reduced.
Question 2
What is the expression for the equilibrium constant for the reaction 2 C 2 H 6 (
g
) + 7 O 2 (
g
) 4 CO 2 (
g
) + 6 H 2 O(
g
)?
A) K= [CO 2 ][H 2 O] [C 2 H 6 ][O 2 ] C) K= [C 2 H 6 ][O 2 ] [CO 2 ][H 2 O] B) K = [CO 2 ] 4 [H 2 O] 6 [C 2 H 6 ] 2 [O 2 ] 7 D) K = [C 2 H 6 ] 2 [O 2 ] 7 [CO 2 ] 4 [H 2 O] 6
K
K
2 [CO ][H O] 6 2 2 6
Question 2
What is the expression for the equilibrium constant for the reaction 2 C 2 H 6 (
g
) + 7 O 2 (
g
) 4 CO 2 (
g
) + 6 H 2 O(
g
)?
A) K= [CO 2 ][H 2 O] [C 2 H 6 ][O 2 ] C) K= [C 2 H 6 ][O 2 ] [CO 2 ][H 2 O] B) K = [CO 2 ] 4 [H 2 O] 6 [C 2 H 6 ] 2 [O 2 ] 7 D) K = [C 2 H 6 ] 2 [O 2 ] 7 [CO 2 ] 4 [H 2 O] 6
Question 3
The definition of a Brønsted-Lowry acid is: A) a compound that contains hydroxide and dissolves in water to form – OH.
B) C) D) a compound that is a proton donor.
a compound that is a proton acceptor.
a compound that contains a hydrogen atom and dissolves in water to form a hydrogen ion, H + .
Question 3
The definition of a Brønsted-Lowry acid is: A) a compound that contains hydroxide and dissolves in water to form – OH.
B) C) D) a compound that is a proton donor.
a compound that is a proton acceptor.
a compound that contains a hydrogen atom and dissolves in water to form a hydrogen ion, H + .
Question 4
An alpha particle is a high-energy particle that contains: A) one proton and one neutron.
B) C) D) two protons and two neutrons.
one electron. one proton.
Question 4
An alpha particle is a high-energy particle that contains: A) one proton and one neutron.
B) C) D) two protons and two neutrons.
one electron. one proton.
Question 5
In the balanced redox reaction: 2 Cu(
s
) + S(
s
) Cu 2 S(
s
) how many electrons are gained or lost by each sulfur atom?
A) B) C) D) each sulfur atom gains two (2) electrons each sulfur atom gains one (1) electron each sulfur atom loses one (1) electron each sulfur atom loses two (2) electrons
Question 5
In the balanced redox reaction: 2 Cu(
s
) + S(
s
) Cu 2 S(
s
) how many electrons are gained or lost by each sulfur atom?
A) B) C) D) each sulfur atom gains two (2) electrons each sulfur atom gains one (1) electron each sulfur atom loses one (1) electron each sulfur atom loses two (2) electrons
Question 6
An equilibrium constant with a value of 4.6 x 10 15 indicates that at equilibrium A) B) C) the reactants are favored.
the products are favored.
approximately equal concentrations of reactants and products are present.
Question 6
An equilibrium constant with a value of 4.6 x 10 15 indicates that at equilibrium A) B) C) the reactants are favored.
the products are favored.
approximately equal concentrations of reactants and products are present.
Question 7
Which species can be a Brønsted–Lowry acid?
A) CO 3 2 – B) HBr C) Br 2 D) LiOH
Question 7
Which species can be a Brønsted–Lowry acid?
A) CO 3 2 – B) HBr C) Br 2 D) LiOH
Question 8
Which species is the conjugate acid of HCO 3 – ?
A) CO 3 2 – B) H 2 CO 3 C) CO 2 D) H 2 O
Question 8
Which species is the conjugate acid of HCO 3 – ?
A) CO 3 2 – B) H 2 CO 3 C) CO 2 D) H 2 O
1 0 e
Question 9
Which is the symbol for the beta particle?
A) 0 1 e C) 0 e -1 B) 1 e -1 D) 1 0 e
1 0 e
Question 9
Which is the symbol for the beta particle?
A) 0 1 e C) 0 e -1 B) 1 e -1 D) 1 0 e
1 0 e
Question 10
In the balanced redox reaction: 2 C 2 H 6 (
g
) + 7 O 2 (
g
) which species is reduced?
4 CO 2 (
g
) + 6 H 2 O(
g
), A) C 2 H 6 (
g
) B) O 2 (
g
) C) CO 2 (
g
) D) H 2 O(
g
)
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Question 10
In the balanced redox reaction: 2 C 2 H 6 (
g
) + 7 O 2 (
g
) which species is reduced?
4 CO 2 (
g
) + 6 H 2 O(
g
), A) C 2 H 6 (
g
) B) O 2 (
g
) C) CO 2 (
g
) D) H 2 O(
g
)
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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 Reaction Zn 2+ (aq) + 2e Zn (s) Cu 2+ (aq) + 2e Cu (s) E 0 (v) -0.76
+0.34
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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 Reaction Zn 2+ (aq) + 2e Zn (s) Cu 2+ (aq) + 2e Cu (s) E 0 (v) -0.76
+0.34
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Question 12
What is the correct cell notation for the zinc/copper cell described in the previous question?
Reduction Reaction Zn 2+ (aq) + 2e Zn (s) A) Cu|Zn||Cu 2+ |Zn 2+ B) Cu|Cu 2+ ||Zn 2+ |Zn Cu 2+ (aq) + 2e Cu (s) C) Zn|Zn 2+ ||Cu 2+ |Cu D) Zn 2+ |Zn||Cu|Cu 2+ E 0 (v) -0.76
+0.34
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Question 12
What is the correct cell notation for the zinc/copper cell described in the previous question?
Reduction Reaction Zn 2+ (aq) + 2e Zn (s) A) Cu|Zn||Cu 2+ |Zn 2+ B) Cu|Cu 2+ ||Zn 2+ |Zn Cu 2+ (aq) + 2e Cu (s) C) Zn|Zn 2+ ||Cu 2+ |Cu D) Zn 2+ |Zn||Cu|Cu 2+ E 0 (v) -0.76
+0.34
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Question 13
For an endothermic reaction, increasing the temperature A) does not shift the equilibrium since
K
is a constant.
B) C) D) increases the rate of the reverse reaction to form more reactants.
increases the rate of the forward reaction to form more products.
increases the rate of the reverse reaction to form more products.
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Question 13
For an endothermic reaction, increasing the temperature A) does not shift the equilibrium since
K
is a constant.
B) C) D) increases the rate of the reverse reaction to form more reactants.
increases the rate of the forward reaction to form more products.
increases the rate of the reverse reaction to form more products.
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Question 14
Which acid is the strongest?
A) B) C) D) Hydrogen sulfate ion HSO 4 – Hydrocyanic acid HCN (
K
a (
K
a = 1.2 x10 = 4.9 x10 –10 ) –2 ) Hydrofluoric acid HF (
K
a = 7.2 x10 –4 ) Ammonium ion NH 4 + (
K
a = 5.6 x10 –10 )
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Question 14
Which acid is the strongest?
A) B) C) D) Hydrogen sulfate ion HSO 4 – Hydrocyanic acid HCN (
K
a (
K
a = 1.2 x10 = 4.9 x10 –10 ) –2 ) Hydrofluoric acid HF (
K
a = 7.2 x10 –4 ) Ammonium ion NH 4 + (
K
a = 5.6 x10 –10 )
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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
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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