Chemistry Quiz - Term 1

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

• To provide electrons for the redox reaction

• To maintain electrical neutrality by allowing ion flow

• To prevent the mixing of solutions in the half-cells

• To catalyze the oxidation-reduction reactions

In a standard hydrogen electrode, what is the concentration of H+ ions?

• 1.0×10−7 M

• 1.0 M

• 0.5 M

• 2.0 M

The Nernst equation is used to calculate:

• The rate of electron transfer in a redox reaction

• The standard reduction potential of a half-cell

• The cell potential under non-standard conditions

• The concentration of ions in an electrolyte solution

Which of the following is NOT a factor affecting the rate of electrolysis?

• Temperature of the electrolyte

• Concentration of the electrolyte

• Color of the electrodes

• Surface area of the electrodes

In a galvanic cell, electrons flow:

• From the cathode to the anode through the external circuit

• From the anode to the cathode through the external circuit

• Through the salt bridge from anode to cathode

• Through the electrolyte solution in both half-cells

The standard reduction potential for Zn2+/Zn is -0.76 V, and for Cu2+/Cu is +0.34 V. What is the standard cell potential for a Zn-Cu galvanic cell?

• −0.42 V

• +0.42 V

• +1.10 V

• −1.10 V

Which of the following statements about corrosion is FALSE?

• It is an electrochemical process

• It always requires the presence of water

• It can be prevented by cathodic protection

• Rust is a common product of iron corrosion

In the electrolysis of molten NaCl, what is produced at the cathode?

• Sodium metal

• Chlorine gas

• Oxygen gas

• Hydrogen gas

The Faraday constant (F) is approximately equal to:

• 6.022×1023 C/mol

• 6.022×1023 C/mol

• 96,485 C/mol

• 1.602×10−19 C

Which of the following best describes the relationship between Gibbs free energy change (ΔG) and the cell potential (E°cell) in a spontaneous electrochemical reaction?

• ΔG=0 and E°cell>0

• ΔG<0 and E°cell<0

• ΔG=0 and E°cell=0