Electrochemistry, Voltaic Cells & Thermodynamics Chapter Exam

Exam Instructions:

Choose your answers to the questions and click 'Next' to see the next set of questions. You can skip questions if you would like and come back to them later with the yellow "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. Good luck!

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Question 1 1. What is the main difference between voltaic and electrolytic cells?

Question 2 2. What is the anode in an electrolytic or voltaic cell?

Question 3 3. Which type of cell is present in a rechargeable battery?

Question 4 4. Which of these is a TRUE statement about voltaic cells?

Question 5 5. What are electrolytic cells used for?

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Question 6 6. Which of the following atoms is used as a reference electrode when measuring standard reduction potentials in the lab?

Question 7 7. Which of the following describes how to calculate the standard cell potential for a battery?

Question 8 8. Which of the following is an application for calculating the standard cell potential?

Question 9 9. Which of the following species would be most likely to be reduced in a battery reaction?

Question 10 10. What is a standard reduction potential?

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Question 11 11.

Write the balanced equation for a voltaic cell from the half-cell reactions below

Fe+2 (aq) + 2 e- → Fe(s).

E0 (V) = - 0.44

Zn+2 (aq) + 2 e- → Zn(s).

E0 (V) = - 0.76

Question 12 12. For either an electrolytic or voltaic cell, oxidation occurs at the (anode/cathode), reduction occurs at the (anode/cathode), and electrons flow from the (anode/cathode to the (anode/cathode).

Question 13 13.

Calculate E0 (V) for the voltaic cell made from the half-cell reactions shown below.

Fe+2 (aq) + 2e- → Fe(s) E0 (V) = - 0.44

Zn+2 (aq) + 2e- → Zn(s) E0 (V) = - 0.76

Question 14 14.

Write the balanced equation for an electrolytic cell from the half-cell reactions below

Fe+2 (aq) + 2e- → Fe(s) E0 (V) = -0.44

Zn+2 (aq) + 2e- → Zn(s) E0 (V) = -0.76

Question 15 15.

Calculate E0 (V) for the electrolytic cell made from the half-cell reactions shown below.

Fe+2 (aq) + 2e- → Fe(s) E0 (V) = - 0.44

Zn+2 (aq) + 2e- → Zn(s) E0 (V) = - 0.76

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Question 16 16. Which of the following is true about the relationship between free energy and the cell potential?

Question 17 17. If you wanted to create a voltaic cell for your science fair project, which of the following properties should you look for in the chemical reaction between cells?

Question 18 18. A chemical reaction has an equilibrium constant of 3.45. Which of the following is also true about the reaction?

Question 19 19. A chemical reaction has a cell potential of -3.36V. Which of the following is also true about this reaction?

Question 20 20. Which of the following is true about electrochemical cells?

Electrochemistry, Voltaic Cells & Thermodynamics Chapter Exam Instructions

Choose your answers to the questions and click 'Next' to see the next set of questions. You can skip questions if you would like and come back to them later with the yellow "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. Good luck!

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