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]

In the electrochemical series, which of the following metals is most likely to be reduced?

A. The metal with the highest reduction potential.

B. The metal with the lowest reduction potential.

C. The metal with the highest oxidation potential.

D. The metal in the middle of the series.

In a voltaic cell, where does oxidation occur?

A. At the cathode.

B. At the anode.

C. In the salt bridge.

D. In the external circuit.

What is the purpose of the standard hydrogen electrode?

A. To measure the pH of a solution.

B. To provide a reference against which other electrode potentials can be measured.

C. To generate electricity.

D. To oxidise hydrogen gas.

If the standard cell potential of a voltaic cell is negative, what does it indicate about the spontaneity of the cell reaction?

A. The cell reaction is spontaneous.

B. The cell reaction is non-spontaneous.

C. The cell reaction is at equilibrium.

D. The cell reaction will be spontaneous if the temperature is increased.

Which of the following is true regarding the electrochemical series?

A. It is a list of elements in order of increasing atomic number.

B. It is a list of metals in order of increasing reactivity.

C. It ranks half-cells based on their standard electrode potentials.

D. It determines the pH of a solution.

a) What is cell notation, and why is it used? [2]

b) Given the cell notation: Ag | Ag^+ || Cl^- | Cl2, deduce the overall cell reaction. [3]

c) Explain the importance of the double vertical lines (||) in cell notation. [2]

a) Define the term "equilibrium constant" in the context of a redox reaction. [2]

b) How is the equilibrium constant related to the standard cell potential of a redox reaction? [3]

c) Given a redox reaction with a large positive standard cell potential, what can be inferred about the position of equilibrium? [2]

a) Describe the role of the salt bridge in a voltaic cell. [2]

b) Given a voltaic cell with cell notation: Mg | Mg^2+ || Cu^2+ | Cu, determine which electrode acts as the anode and which acts as the cathode. [2]

c) Write the half-reactions occurring at each electrode for the above cell. [3]

d) If the concentration of Cu^2+ is increased, how would it affect the cell potential? [2]

a) Explain the significance of standard cell potentials in predicting the spontaneity of redox reactions. [3]

b) How can the standard cell potential be used to determine the Gibbs free energy change for a reaction? [3]

c) Given a reaction with a negative Gibbs free energy change, what can be inferred about its standard cell potential and spontaneity? [2]

d) Describe the importance of the standard hydrogen electrode in establishing the electrochemical series. [3]

a) What is meant by the term "equivalence point" in the context of a redox titration? [3]

b) How can a pH curve be used to identify the equivalence point in a titration involving a strong acid and a strong base? [3]

c) Describe the buffer region observed in a pH curve. [3]

d) Why is the choice of indicator crucial in a redox titration? [2]