Chemistry

QUESTION 1

Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of water.

NO3-(aq) + I(aq)- → NO(g) + I2(s)

a. 3

b. 1

c. 2

d. 4

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QUESTION 2

Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of water.

P4(aq) → HPO32-(aq) + PH3(g)

a. 3

b. 6

c. 2

d. 4

e. 5

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QUESTION 3

Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of water.

H2CO(aq) + S(s) → H2S(g) + CO2(g)

a. 5

b. 2

c. 1

d. 4

e. 3

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QUESTION 4

Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of water.

Cr2O72- + Fe2+(aq) → Cr3+(aq) + Fe3+(aq)

a. 4

b. 3

c. 2

d. 7

e. 6

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QUESTION 5

Which letter represents the electrode with a negative charge in the figure shown:

a. S

b. Z

c. T

d. X

e. Y

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QUESTION 6

Consider the Figure shown in which X represent Zn(s), T represents Co(s), and S is a solution that is 1.0 M in Co2+.

At which electrode are electrons generated? The reduction potentials of Co2+ and Zn2+ are -0.27 V and -0.76 V, respectively.

a. Y

b. S

c. X

d. T

e. Z

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QUESTION 7

Determine Eo for the following reaction, using the given standard reduction potentials:

Cu(s) + Fe2+(aq) → Cu2+(aq) + Fe(s)

Eo for Fe2+(aq) = -0.44 V

Eo for Cu2+(aq) = 0.34 V

Do not put in units.

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QUESTION 8

Determine Eo for the following reaction, using the given standard reduction potentials:

Sn(s) + Fe2+(aq) → Sn2+(aq) + Fe(s)

Eo for Fe2+(aq) = -0.44 V

Eo for Sn2+(aq) = -0.14 V

Do not put in units.

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QUESTION 9

Determine Eo for the following reaction, using the given standard reduction potentials:

Cr2+(aq) + Mn2+(aq) → Cr3+(aq) + Mn(s)

Eo for Mn2+(aq) = -1.18 V

Eo for Cr3+(aq) = -0.41 V

Do not put in units.

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QUESTION 10

Consider the following half-reactions. Which of these is the strongest oxidizing agent listed here?

I2(s) + 2 e- → 2 I-(aq) Eo = 0.53 V

S2O82-(aq) + 2 e- → 2 SO42-(aq) Eo = 2.01 V

Cr2O72-(aq) + 14 H+ + 6 e- → Cr3+(aq) + 7 H2O(l) Eo = 1.33 V

1. I2(s)

2. I-(aq)

3. S2O82-(aq)

4. SO42-

5. Cr2O72-

6. Cr3+(aq)

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QUESTION 11

Identify the oxidizing agent and the reducing agent in the reaction.

5H2C2O4(aq) + 2MnO4–(aq) + 6H+(aq) → 2Mn2+(aq) + 10CO2(g) + 8H2O(l)

1. oxidizing agent: MnO4– ; reducing agent: H2C2O4

2. oxidizing agent: 6H+ ; reducing agent: MnO4–

3. oxidizing agent: H2C2O4; reducing agent: 6H+

4. oxidizing agent: H2C2O4 ; reducing agent: MnO4–

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QUESTION 12

Consider the reaction between sulfite and a metal anion, X2-, to form the metal, X, and thiosulfate:

2 X2-(aq) + 2 SO32- + 3 H2O(l) → 2 X(s) + S2O32- (aq) + 6 OH-

for which Eocell = 1.07.

Given that the Eored for sulfite is -0.57 V, calculate Eored for X. Enter your answer to 2 decimal places.

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