Semester 2 AP Exam

The diagram shows a galvanic cell that has an electrode of Ni(s) immersed in 1.0 M solution of NiSO₄(aq) and a Zn(s) electrode that has been immersed in 1.0M solution of ZnSO₄(aq). As the cell begins to operate, electrons flow from the Zn(s), electrode to the Ni(s) electrode.

Which of the following particle views best represents what occurs in the salt bridge as current flows through the cell? (Solvent molecules are not shown.)

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A student sets up a galvanic cell that has a Sn(s) electrode and Cd(s) electrode. The half-reactions that occur at each electrode are represented in the table. Which of the following correctly describes what happens as the cell operates?

• The Sn(s) electrode increases in mass, and the Cd(s) electrode decreases in mass.

• The Sn(s) electrode decreases in mass, and the Cd(s) electrode increases in mass.

• Both Sn(s) electrode and the Cd(s) electrode increase in mass.

• TBoth Sn(s) electrode and the Cd(s) electrode decrease in mass.

When the switch is closed in the electrochemical cell represented above, the resulting cell voltage is 0.3 V. What would be the cell voltage if the salt bridge was removed from the cell?

• E^°cell​ =0 V

• 0 V< E^°cell <0.32 V

• E^°cell ​=0.32 V

• E^°cell ​>0.32 V

2NaBr_(l) --> 2Na _(l) + Br2_(g)

In an electrolytic cell based on the reaction represented above, which of the following occurs at the cathode?

• Sodium is oxidized.

• Sodium is reduced.

• Bromine is oxidized.

• Bromine is reduced.

A student sets up a galvanic cell that has a Mn(s) electrode and Ni(s) electrode. The half-reactions that occur at each electrode are represented in the table. Which of the following correctly describes what happens as the cell operates?

• The Mn(s) electrode increases in mass, and the Ni(s) electrode decreases in mass.

• The Mn(s) electrode decreases in mass, and the Ni(s) electrode increases in mass.

• Both Mn(s) electrode and the NI(s) electrode increase in mass.

• Both Mn(s) electrode and the Ni(s) electrode decrease in mass.

When the switch is closed in the electrochemical cell represented above, the resulting cell voltage is 0.53 V. What would be the cell voltage if the salt bridge was removed from the cell?

• It would be greater than 0.53V.

• It would be less than 0.53V but greater than 0 V.

• It would be V.

• It would not change.

In an electrolytic cell based on the reaction represented above, which of the following occurs at the anode?

• Lead is oxidized.

• Lead is reduced.

• Bromine is oxidized.

• Bromine is reduced.

The diagram shows a galvanic cell that has an electrode of Cu(s) immersed in 1.0 M solution of Cu(NO₃)₂(aq) and a Ag(s) electrode that has been immersed in 1.0M solution of AgNO₃(aq). As the cell begins to operate, electrons flow from the Cu(s), electrode to the Ag(s) electrode.

Which of the following particle views best represents what occurs in the salt bridge as current flows through the cell? (Solvent molecules are not shown.)

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Which of the following statements accurately describes the Nernst equation shown?

• At equilbrium, Ecell calculates a value will be 0, & the battery is considered dead because Q equals K_eq & K_eq has a value of 0.

• Increasing the concentration of the reactants will increase the value of Ecell.

• This equation is used to figure out the standard cell potential at any concentration, partial pressure, or temperature.

• At standard conditions, Ecell = E⁰cell because all the concentrations are 1M at an ambient temperature of 273 K.

Given the table of reduction potentials, which metals will displace hydrogen gas out of acid?

I. Aluminum

II. Palladium

III. Potassium

IV. Zinc

• II only

• I and III

• II and IV

• I, III, and IV