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IB DP Chemistry Questions

19.1 Electrochemical Cells

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]

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