WORKHSEET ON ELECTROCHEMISTRY

 

Here are 20 challenging questions related to electrochemistry for a deeper understanding of the topic:

1. What is the standard electrode potential for the reduction of chlorine to chloride ions?
   +1.36 V

2. In the context of the Nernst equation, what does the term $E$ represent?
   Cell potential

3. Calculate the cell potential for the reaction: $Zn + Cu^{2+} \rightarrow Zn^{2+} + Cu$ using standard electrode potentials: Zn²⁺/Zn = -0.76 V and Cu²⁺/Cu = +0.34 V.
   1.10 V

4. What is the standard reduction potential of the silver/silver ion electrode?
   +0.80 V

5. For a concentration cell, what is the relationship between the concentration difference and the cell potential?
   Directly proportional

6. How does the electrode potential of a metal change when it is immersed in a solution of its ions?
   Depends on concentration

7. What type of reaction is described by the cell notation: $\text{Zn | Zn}^{2+}(0.01 M) \| \text{Cu}^{2+}(1 M) | \text{Cu}$?
   Concentration cell

8. What is the term for the process in which electrolysis is used to separate a metal from its ore?
   Electrometallurgy

9. In an electrolytic cell, what is the role of the anode?
   Oxidation site

10. Determine the cell potential at 298 K for a cell reaction with $E^\circ_{\text{cell}} = 0.45$ V and $Q = 10$, using the Nernst equation.
    0.45 V (assuming standard conditions for simplification)

11. What is the effect of increasing the temperature on the cell potential according to the Nernst equation?
    Varies with reaction enthalpy

12. What is the effect of increasing the concentration of the reactant on the cell potential of a galvanic cell?
    Increases potential

13. What is the term for the potential difference that drives a galvanic cell when the reactants are in their standard states?
    Standard cell potential

14. In the context of electrochemical cells, what is meant by the term "electrochemical equivalent"?
    Mass deposited per unit charge

15. Calculate the cell potential for the reaction: $2 \text{Ag}^+ + \text{Cu} \rightarrow 2 \text{Ag} + \text{Cu}^{2+}$ given the standard reduction potentials: Ag⁺/Ag = +0.80 V and Cu²⁺/Cu = +0.34 V.
    1.12 V

16. What is the relationship between Gibbs free energy change ($\Delta G$) and cell potential ($E$) in an electrochemical reaction?
    $\Delta G = -nFE$

17. For a concentration cell involving $\text{Cu}$ electrodes with different concentrations, what will be the cell potential if the concentrations are equal?
    Zero

18. Which electrode reaction is favored in a galvanic cell with a high concentration of the reactant?
    Reduction at the cathode

19. How does the presence of a common ion affect the cell potential of an electrochemical cell?
    Reduces the potential

20. What is the term for the change in cell potential with respect to temperature known as?
    Thermodynamic sensitivity