Which of the following are redox reactions? Se 2 O 3 2- + I 2 ? I - + Se 4 O 6 2

Question

Which of the following are redox reactions?

Se2O32- + I2 ? I- + Se4O62-

TeO2 + H+ ? Te + H2O

HCl + BaCO3 ? BaCl2 + HCO3-

Question 2 options:

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Question 3 (0.26 points)

Balance the following equation in acid and report the number of H+.

CrO42- (aq) + SO32- (aq) ? Cr(OH)3 (s) + SO42- (aq)

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Question 4 (0.26 points)

Balance the following in base and report the number ofH2O in the balanced equation.

MnO4- + N2H4     ? MnO2 + N2   

Question 4 options:

0

2

4

12

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Question 5 (0.26 points)

The following half-cells are constructed to form a voltaic cell. Identify the oxidizing and reducing agent respectively.

MnO4-| Mn2+ and Br2| Br-

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Question 6 (0.26 points)

Calculate the standard cell potential, E, (V) for the following reaction:

3 Pb2+ (aq) + 2 MnO2 (s) + 8 OH- (aq) ? 3 Pb (s) + 2 MnO4- (aq) + 4 H2O (l)

Question 6 options:

-0.73

+0.73

01.47

+1.19

-1.77

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Question 7 (0.26 points)

Which of these is the best oxidizing agent?

Question 7 options:

Ag

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Question 8 (0.26 points)

Which of these is the best reducing agent?

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Question 9 (0.26 points)

Identify the cathode and anode, respectively, for the following reaction:

Mg (s)| Mg2+ (aq) || Au+ (aq) | Au (s)

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Question 10 (0.26 points)

Calculate the standard change in free energy, ?G, (kJ) for the unbalanced reaction below;
NO3- (aq) + Fe2+ (aq)   ? NO (g) + Fe3+ (aq)

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Question 11 (0.26 points)

An voltaic cell is assembled with Mn|Mn2+ and the [Mn2+] is 0.250 M. A separate half-cell contains a platinum electrode with a solution that contains 0.100 M Fe2+ and 0.400 M Fe3+. What is the potential of the cell?

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Question 12 (0.26 points)

A concentration cell consists of two Zn/Zn2+ electrodes. The electrolyte in compartment A is 0.10 M Zn(NO3)2 and in compartment B is 0.60 M Zn(NO3)2. What is the voltage (V ) of the cell at 25C?

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Question 13 (0.26 points)

Calculate the equilibrium constant for the following reaction at 25C:

3 Cd2+ (aq) + 2 Cr (s) ? 3 Cd (s) + 2 Cr3+ (aq)

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Question 14 (0.26 points)

Predict the products of electrolysis in a molten solution of FeCl2.

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Question 15 (0.26 points)

Predict the products of electrolysis in an aqueous solution of FeCl2.

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Question 16 (0.26 points)

Calculate the mass (g) of Ba produced when with a solution of BaCl2 is electrolyzed with a current of 0.750 amps for 25 min.

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Question 17 (0.26 points)

How long (hrs) must a current of 2.5 amps flow to produce 10 g of Cu from a 0.1500 M solution of CuCl2?

Question 17 options:

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Question 18 (0.26 points)

Identify the correct relationships.

i) When K > 1, the reaction is spontaneous
ii) When ?G < 0, the reaction is spontaneous
iii) When E > 0, the reaction is spontaneous

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Question 19 (0.32 points)

Which one of the following statements about electrochemical cells is correct?

Question 19 options:

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A) i B) i and ii C) ii and iii D) i and iii E) All of the Above Which of the following are redox reactions? Se2O32- + I2 ? I- + Se4O62- TeO2 + H+ ? Te + H2O HCl + BaCO3 ? BaCl2 + HCO3- Question 2 options: A) i B) i and ii C) ii and iii D) i and iii E) All of the Above Save Question 3 (0.26 points) Which one of the following statements about electrochemical cells is correct? Question 19 options: A) In a salt bridge, current is carried by cations moving toward the anode, and anions toward the cathode. B) In the external wire, electrons travel from cathode to anode. C) The anode of a voltaic cell is labeled minus (-). D) Oxidation occurs at the cathode in an electrolytic cell. E) The change in free energy, ?G°, is negative for an electrolytic cell. Save Identify the correct relationships. i) When K > 1, the reaction is spontaneous ii) When ?G 0, the reaction is spontaneous Question 18 options: A) i and ii B) iii only C) i and iii D) ii only E) i, ii, and iii Save Question 19 (0.32 points) How long (hrs) must a current of 2.5 amps flow to produce 10 g of Cu from a 0.1500 M solution of CuCl2? Question 17 options: A) 8.4 B) 214 C) 3.4 D) 203 E) 340 Save Question 18 (0.26 points) Calculate the mass (g) of Ba produced when with a solution of BaCl2 is electrolyzed with a current of 0.750 amps for 25 min. Question 16 options: A) 53.4 B) 0.80 C) 3.20 D) 1.6 E) 1.3 ?? 10-2 Save Question 17 (0.26 points) Predict the products of electrolysis in an aqueous solution of FeCl2. Question 15 options: A) Fe, Cl2 B) Cl2, H2, OH- C) OH-, O2, H+, H2 D) H2, O2 E) Fe2+, Cl- Save Question 16 (0.26 points) Predict the products of electrolysis in a molten solution of FeCl2. Question 14 options: A) Fe, Cl2 B) Cl2, H2, OH- C) Fe, O2, H+ D) H2, O2 E) Fe2+, Cl- Save Question 15 (0.26 points) Calculate the equilibrium constant for the following reaction at 25°C: 3 Cd2+ (aq) + 2 Cr (s) ? 3 Cd (s) + 2 Cr3+ (aq) Question 13 options: A) 2.4 ?? 10-39 B) 4.2 ?? 1038 C) 6.8 ?? 10-35 D) 1.7 ?? 1017 E) 2.9 ?? 1034 Save Question 14 (0.26 points) A concentration cell consists of two Zn/Zn2+ electrodes. The electrolyte in compartment A is 0.10 M Zn(NO3)2 and in compartment B is 0.60 M Zn(NO3)2. What is the voltage (V ) of the cell at 25°C? Question 12 options: A) 0.010 B) 0.020 C) 0.023 D) 0.046 E) None of these choices is correct. Save Question 13 (0.26 points) An voltaic cell is assembled with Mn|Mn2+ and the [Mn2+] is 0.250 M. A separate half-cell contains a platinum electrode with a solution that contains 0.100 M Fe2+ and 0.400 M Fe3+. What is the potential of the cell? Question 11 options: A) 2.00 B) 1.99 C) 1.90 D) 1.91 E) 1.95 Save Question 12 (0.26 points) Calculate the standard change in free energy, ?G°, (kJ) for the unbalanced reaction below; NO3- (aq) + Fe2+ (aq) ? NO (g) + Fe3+ (aq) Question 10 options: A) -167 B) +167 C) -55 D) -18 E) +500 Save Question 11 (0.26 points) Identify the cathode and anode, respectively, for the following reaction: Mg (s)| Mg2+ (aq) || Au+ (aq) | Au (s) Question 9 options: A) Au, Mg2+ B) Mg2+, Au+ C) Au, Mg D) Au+, Mg2+ E) Mg, Au Save Question 10 (0.26 points) Which of these is the best reducing agent? Question 8 options: A) SO42- B) Ni C) Ag D) Ca E) I- Save Question 9 (0.26 points) Which of these is the best oxidizing agent? Question 7 options: A) Br- B) Ag C) Ce4+ D) I2 E) Ni2+ Save Question 8 (0.26 points) Calculate the standard cell potential, E°, (V) for the following reaction: 3 Pb2+ (aq) + 2 MnO2 (s) + 8 OH- (aq) ? 3 Pb (s) + 2 MnO4- (aq) + 4 H2O (l) Question 6 options: A) -0.73 B) +0.73 C) 01.47 D) +1.19 E) -1.77 Save Question 7 (0.26 points) The following half-cells are constructed to form a voltaic cell. Identify the oxidizing and reducing agent respectively. MnO4-| Mn2+ and Br2| Br- Question 5 options: A) Mn2+, Br- B) MnO4-, Br- C) MnO4-, Br2 D) Br2, Mn2+ E) Br2, MnO4- Save Question 6 (0.26 points) Balance the following in base and report the number of H2O in the balanced equation. MnO4- + N2H4 ? MnO2 + N2 Question 4 options: A) 0 B) 2 C) 3 D) 4 E) 12 Save Question 5 (0.26 points) Balance the following equation in acid and report the number of H+. CrO42- (aq) + SO32- (aq) ? Cr(OH)3 (s) + SO42- (aq) Question 3 options: A) 1 B) 2 C) 3 D) 4 E) 6 Save Question 4 (0.26 points)

Explanation / Answer

Question 1.

Which of the following are redox reactions?

a)

Se2O32- + I2 --> I- + Se4O62-

I goes from 0 to -1, it gains 1 electron

Se goes from +2 to +3, it loses 1 electron

this is REDUCTION+OXIDATION, i.e. it is REDOX

B)

TeO2 + H+ --> Te + H2O

balance

TeO2 + 4H+ --> Te + 2H2O

Te goes from +4 to 0, it gains 4 electrons

but no other species is present so it must hav e acharge balance, i.e. it is a half reaciton

4e- + TeO2 + 4H+ --> Te + 2H2O

NOT REDOX

C)

HCl + BaCO3 --> BaCl2 + HCO3-

H remains with +1,

Ba remains with +1

CO3 remains with -2, this is simply double replacement

NO REDOX

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