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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