19.1 Electrochemical Cells

Which of the following best describes the function of the salt bridge in a voltaic cell?

A. To provide a pathway for electron flow.

B. To prevent the mixing of the two half-cell solutions.

C. To complete the circuit by allowing ion flow.

D. To increase the voltage of the cell.

In cell notation, which electrode is written on the left-hand side?

A. The electrode with the higher reduction potential.

B. The anode.

C. The cathode.

D. The electrode with the lower reduction potential.

Which of the following is true regarding the standard hydrogen electrode?

A. It always acts as the anode in a cell.

B. It has a standard electrode potential of 1.00 V.

C. It is used as a reference electrode to measure other electrode potentials.

D. It involves the reduction of oxygen gas.

If the standard cell potential, E°cell, is positive, what can be inferred about the redox reaction?

A. The reaction is non-spontaneous.

B. The reaction is at equilibrium.

C. The reaction is spontaneous in the reverse direction.

D. The reaction is spontaneous in the forward direction.

Which of the following is NOT a factor that affects the electrode potential of a half-cell?

A. Concentration of the ions in the solution.

B. Temperature of the solution.

C. Presence of a catalyst.

D. Nature of the electrode metal.

a) Describe the primary components and functioning of a voltaic cell. [3]

b) Explain the significance of the salt bridge in an electrochemical cell. [2]

a) Define standard cell potential and explain its significance in predicting the spontaneity of redox reactions. [3]

b) Given the half-cell potentials: Zn^2+ + 2e^- -> Zn is -0.76 V and Cu^2+ + 2e^- -> Cu is +0.34 V, determine the standard cell potential for the voltaic cell constructed using these half-cells. [2]

a) Describe the construction and use of the standard hydrogen electrode (SHE). [3]

b) Why is the SHE important in establishing the electrochemical series? [2]

a) Explain the difference between a voltaic cell and an electrolytic cell in terms of energy conversion. [2]

b) Given the cell notation: Zn | Zn^2+(1M) || Cu^2+(1M) | Cu, identify the anode, cathode, and the direction of electron flow. [2]

c) How does the concentration of the electrolyte solutions affect the cell potential? [3]

a) Describe the significance of the standard hydrogen electrode in measuring electrode potentials. [3]

b) Why is it essential to maintain a constant temperature when measuring electrode potentials? [2]

c) How can the spontaneity of a redox reaction be predicted using standard cell potentials? [2]