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- 1. Multiple ChoiceAn electrochemical cell was set up using iron and copper plates in molar solution of Fe2+ (aq) and Cu2+ respectively. Which one is the correct cell diagram represent?Fe (s) | Fe2+ (aq) || Cu2+ (aq) | Cu (s)Cu (s) | Cu2+ (aq) || Fe2+ (aq) | Fe (s)
- 2. Multiple ChoiceThe standard reduction potential, E°, at 298K for five half-cells are given below. W2+ (aq) + 2e- <=> W (s) -2.38V, X3+ (aq) + 3e- <=> X (s) -1.66V, Y2+ (aq) +2e- <=> Y (s) +0.34V, Z+ (aq) + e- <=> Z (s) +0.80V, Fe2+ (aq) + 2e- <=> Fe (s) -0.44V. Which species causes iron to rust faster?Z+W2+X3+Y2+
- 3. Multiple ChoiceThe standard reduction potential of several half-cell reactions are shown below. Sn2+ (aq) + 2e- -> Sn (s) -0.14V Fe2+ (aq) + 2e- -> Fe (s) -0.44V Cr3+ (aq) + 3e- -> Cr (s) -0.74V Mn2+ (aq) + 2e- -> Mn (s) -1.18V Al3+ (aq) + 3e- -> Al (s) -1.66V Which metal will produce the most rust when it comes in contact with iron in an electrolyte?SnAlCrMn
- 4. Multiple ChoiceThe standard reduction potential for several half-cells at 298K are given. Al3+ = -1.66v, Fe2+ = -0.44v, Sn2+ = -0.14v, Cu2+ = +0.34v, I2 = +0.54, Fe3+ = +0.77, Br2 = +1.07, Cl2 = +1.36, Mn3+ = +1.49. Which species is the most powerful oxidising agent?Mn3+Al3+Cu2+Sn2+
- 5. Multiple ChoiceZn (s) | Zn2+ (aq) || Fe3+ (aq) , Fe2+ (aq) Pt (s). Which acts as the positive terminal?PtZn
- 6. Multiple ChoiceZn (s) | Zn2+ (aq) || Fe3+ (aq) , Fe2+ (aq) Pt (s). Where the negative ions go?Zn / Zn2+Fe2+ / Pt
- 7. Multiple ChoiceZn (s) | Zn2+ (aq) || Fe3+ (aq) , Fe2+ (aq) Pt (s). What happens to the [Fe2+] / [Fe3+]?Increases.Decreases.
- 8. Multiple ChoiceAn electrochemical cell consist of Ag+ (aq) | Ag (s) = +0.80 V, and Zn2+ (aq) | Zn (s) = -0.76 V. Where the anions from the salt bridge go?Ag+ (aq) | Ag (s) half-cell.Zn2+ (aq) | Zn half-cell.
- 9. Multiple ChoiceAn electrochemical cell consist of Ag+ (aq) | Ag (s) = +0.80 V, and Zn2+ (aq) | Zn (s) = -0.76 V. Which has a greater tendency to form positively charged ions?ZnAg
- 10. Multiple ChoiceAn electrochemical cell consist of Ag+ (aq) | Ag (s) = +0.80 V, and Zn2+ (aq) | Zn (s) = -0.76 V. Which electrode acts as the anode?ZnAg
- 11. Multiple ChoiceAn electrochemical cell consist of Ag+ (aq) | Ag (s) = +0.80 V, and Zn2+ (aq) | Zn (s) = -0.76 V. Which electrode acts as the cathode?AgZn
- 12. Multiple ChoiceAn electrochemical cell consist of Ag+ (aq) | Ag (s) = +0.80 V, and Zn2+ (aq) | Zn (s) = -0.76 V. What happens when reaction continues?concentration of Zn2+ increasesconcentration of Ag+ increases
- 13. Multiple ChoiceAn electrochemical cell consist of Ag+ (aq) | Ag (s) = +0.80 V, and Zn2+ (aq) | Zn (s) = -0.76 V. What happens to the Ecell when reaction continues?Ecell decreasesEcell increases
- 14. Multiple ChoiceThe Nernst equation is written as Ecell = E°cell - 0.059/n log Q. For the reaction Mg (s) + 2H+ (aq) -> Mg2+ (aq) + H2 (g), Q may be expressed as[ Mg2+ ] PH2 ÷ [ H2 ]²[ Mg2+ ] ÷ {[Mg] [ H+ ]²}[ Mg2+ ] PH2 ÷ { [ Mg ] [ H+ ]² }[ H+ ]² ÷ [ Mg2+ ] PH2
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