Electrochemistry Multiple Choice Test
Click in the appropriate box for each question, then click "Done" at the bottom. 10 marks for each correct answer. Hints cost 5 marks each.
1. A Galvanic cell: Has a spontaneous chemical reaction Has a positive cell potential Has a negatively charge anode All of the above None of the above
2. An electrolytic cell: Has a non-spontaneous chemical reaction Requires application of a negative potential to make the reaction occur Has a positively charged anode All of the above None of the above
3. In a galvanic cell: Electrons flow from the cathode to the anode via the external circuit Electrons lose some of their energy in the external circuit Electrons travel through the salt bridge, or electrolyte The chemical reaction has a positive free energy change None of these
4. Fluorine is above chlorine in the table of standard reduction potentials. This implies: Chlorine is more easily reduced Chloride ions can reduce fluorine Fluoride ions can reduce chlorine Can't tell from this information
5. In the cell represented by the shorthand notation: Cd(s) | Cd+2(aq) || F-(aq), F2(g) | Pt(s), The platinum is being oxidized by the fluorine gas The Cd+2 ions are being reduced The F- is being oxidized to fluorine gas The oxidation compartment is on the left None of the above
6. In an electrolytic cell containing aqueous Na2SO4 and two platinum electrodes, what is produced at the cathode? Click here for a table of reduction potentials. Sodium metal SO2(g) Oxygen gas Hydrogen gas Nothing
7. Which of the metals Zn, Cu, Al, and Ni can cathodically protect a sample of iron from corrosion? Click here for a table of reduction potentials. All of them None of them Only Zn and Al Only Cu and Ni Only Zn
8. If we pass a current of 10.0 Amperes through a solution for 1 hour, how many moles of electrons are used?
10 x 1 10 x 1 x 3600 10 x 1 x 3600 x 96487 10 x 1 x 3600 / 96487 none of the above
9. The REDOX reaction Zn(s) + Cu+2(aq) = Zn+2(aq) + Cu(s) has Eo = +1.10 V. The standard free energy for this reaction can be calculated as:
DGo = 96487 (1.10) J/mol DGo = 2 (96487) (1.10) J/mol DGo = - 96487 (1.10) J/mol DGo = - 2 (96487) (1.10) J/mol DGo = - 3 (96487) (1.10) J/mol
10. Secondary batteries can be recharged because:
The anode is not destroyed during use The products are in physical contact with the electrodes Both of the above Neither of the above