Title: Chapter 17: Electrochemistry
Course: Test

Q: Write a balanced redox reaction for the formation of rust on iron metal and identify the correct oxidizing agent and/or reducing agent.
- Iron is the oxidizing agent and O_2 is neither a reducing agent nor an oxidizing agent
- Iron is the oxidizing agent and O_2 is the reducing agent
- Iron is the reducing agent and O_2 is the oxidizing agent
A: Iron is the reducing agent and O_2 is the oxidizing agent

Q: Which is the reducing agent in the combustion of methanol?
- CH_3OH
- O_2
- CO_2
A: CH_3OH

Q: Which is the oxidizing agent in the combustion of methanol?
- CH_3OH
- O_2
- CO_2
A: O_2

Q: Propane is used as a fuel source on many barbeque grills. What is undergoing oxidation during the burning of propane while grilling?
- CH_3CH_2CH_3
- O_2
- CO_2
A: CH_3CH_2CH_3

Q: Propane is used as a fuel source on many barbeque grills. What is undergoing reduction during the burning of propane while grilling?
- CH_3CH_2CH_3
- O_2
- CO_2
A: O_2

Q: Automobiles from northern states tend to show more signs of rust formation than southern states. The reason for this is that the rate of corrosion is affected by _____, which is more common during winter months especially in northern states.
- the cold air and clouds
- rain clouds
- snow, ice, and salt mixtures
A: snow, ice, and salt mixtures

Q: Certain anaerobic organisms such as methanogens have the ability to metabolize carbon dioxide into methane in the presence of hydrogen. Methane is produced by the oxidation of _____?
- H_2
- CO_2
- CH_4
A: H_2

Q: A voltaic cell must be split into two separate cells, an oxidation and reduction half-cells. The two half-cells must be connected by a _____ so ions can freely flow between the two half-cells to balance the charges or the voltaic cell cannot function.
- metallic wire
- salt bridge
- membrane
A: salt bridge

Q: In a voltaic cell, oxidation occurs at the _____.
- anode terminal
- cathode terminal
- positive terminal
A: anode terminal

Q: In a voltaic cell, reduction occurs at the _____.
- anode terminal
- cathode terminal
- negative terminal
A: cathode terminal

Q: Electron flow in a voltaic cell is always from _____ to _____.
- anode to cathode
- cathode to anode
- anode to negative terminal
A: anode to cathode

Q: The following can be used as an electrolyte for a salt bridge in a voltaic cell?
- KNO_3(aq)
- H_2O(l)
- CH_3OH(l)
A: KNO_3(aq)

Q: The following can be used as an electrolyte for a salt bridge in a voltaic cell?
- CCl_4(l)
- CH_3CH_2OH(l)
- Na_2SO_4(aq)
A: Na_2SO_4(aq)

Q: In a voltaic cell, electrons are produced at the _____.
- positive terminal
- anode terminal
- cathode terminal
A: anode terminal

Q: The anode terminal in a voltaic cell is the _____ terminal.
- (-)
- (+)
- Neutral
A: (-)

Q: The cathode terminal in a voltaic cell is the _____ terminal.
- (-)
- (+)
- neutral
A: (+)

Q: In a voltaic cell, electrons are received at the _____.
- cathode terminal
- negative terminal
- anode terminal
A: cathode terminal

Q: Based on the reduction potential data, what is the standard cell potential for the following electrochemical cell reaction: Zn(s) + Cu^2+(aq) → Zn^2+(aq) + Cu(s)?

E°_red = -0.763 V for Zn^2+(aq) + 2e^- → Zn(s)

E°_red = +0.340 V for Cu^2+(aq) + 2e^- → Cu(s)
- +1.103 V
- -0.423 V
- +0.423 V
A: +1.103 V

Q: Based on the reduction potential data, what is the standard cell potential for the following electrochemical cell reaction: Cu(s) + 2Ag^+ → Cu^2+(aq) + 2Ag(s)?

E°_red = +0.800 V for Ag^+(aq) + e^- → Ag(s)

E°_red = +0.340 V for Cu^2+(aq) + 2e^- → Cu(s)
- +1.14 V
- +0.460 V
- +1.26 V
A: +0.460 V

Q: Based on the following reduction potential data, which is the strongest reducing agent?

E°_red = +1.78 V for H_2O_2(aq) + 2H^+(aq) + 2e- → 2H_2O(l)

E°_red = +0.800 V for Ag^+(aq) + e^- → Ag(s)

E°_red = -0.130 V for Pb^2+(aq) + 2e^- → Pb(s)
- Pb(s)
- Ag(s)
- H_2O(l)
A: Pb(s)

Q: Based on the following reduction potential data, which is the strongest oxidizing agent?

E°_red = +1.78 V for H_2O_2(aq) + 2H^+(aq) + 2e^- → 2H_2O(l)

E°_red = +0.800 V for Ag^+(aq) + e^- → Ag(s)

E°_red = -0.130 V for Pb^2+(aq) + 2e^- → Pb(s)
- Pb^2+(aq)
- H_2O_2(aq)
- Ag^+(aq)
A: H_2O_2(aq)

Q: The standard cell potential is +0.460 V for the following electrochemical cell reaction: Cu(s) + 2Ag^+(aq) à Cu^2+(aq) + 2Ag(s). What is the ∆G°_rxn?
- -88.8 kJ/mol
- -44.4 kJ/mol
- +44.4 kJ/mol
A: -88.8 kJ/mol

Q: What is the ∆G°_rxn for a 2 electron transfer electrochemical cell with a standard cell potential of +0.770 V.
- -74.3 kJ/mol
- -149 kJ/mol
- +74.3 kJ/mol
A: -149 kJ/mol

Q: Based on the following reduction potential data, what is the ∆G°_rxn for the following electrochemical cell reaction: Zn(s) + Cu^2+(aq) → Zn^2+(aq) + Cu(s)?

E°_red = -0.763 V for Zn^2+(aq) + 2e^- → Zn(s)

E°_red = +0.340 V for Cu^2+(aq) + 2e^- → Cu(s)
- +106 kJ/mol
- -106 kJ/mol
- -213 kJ/mol
A: -213 kJ/mol

Q: Which of the following acids is a strong oxidant?
- HCl
- HNO_3
- HI
A: HNO_3

Q: Which strong acid is commonly used in automobile batteries?
- HCl
- H_2SO_4
- HNO_3
A: H_2SO_4

Q: Cell phones batteries are typically rechargeable. How do they differ from non-rechargeable batteries?
- A rechargeable battery has the ability to undergo a double replacement reaction while non-rechargeable batteries do not. Therefore, the forward direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.
- A rechargeable battery has the ability to undergo a reversible redox reaction while non-rechargeable batteries do not. Therefore, the forward direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.
- A rechargeable battery has the ability to undergo a redox reaction while non-rechargeable batteries do not. Therefore, the reverse direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.
A: A rechargeable battery has the ability to undergo a reversible redox reaction while non-rechargeable batteries do not. Therefore, the forward direction provides electrical energy and connecting the battery to a charger reverses the reaction to reform the starting the materials.

Q: The process of corrosion involves what type of reaction?
- double displacement reaction
- acid-base reaction
- redox reaction
A: redox reaction

Q: What is the oxidation state of oxygen in K_2O_2?
- 0
- -1
- -2
A: -1

Q: Which of the following is a strong oxidizing agent?
- N_2
- O_2
- H_2
A: O_2