Question 1
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.
Question 2
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.
Question 3
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.
Question 4
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.
Question 5
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.
Question 6
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]
Question 7
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]
Question 8
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]
Question 9
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]
Question 10
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]