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reduction-potential-worksheet - Based on these equations...

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Cell Potentials and Reduction Potentials: Worksheet Reference: 17.6 (pg. 711 – 716) 1. What is the difference between E cell and E ° cell ? Be specific. 2. If Galvanic cells have a maximum voltage of only a few volts, how is it possible that a 9-volt battery (or greater) can exist? 3. What is meant by reduction potential? 4. When two half-cells are connected, how is it possible to determine which will gain electrons? 5. Look at the diagram on pg. 710. Which half-cell has the greater reduction potential? How can you tell? 6. For PE 5 on pg. 711. Which half-cell has the greater reduction potential? 7. What equation is used to calculate E ° cell ? 8. For the silver-copper cell, E ° cell = E ° Ag+ - E ° Cu2+ . What would E ° cell equal if E ° Ag+ was 0.96 V and E ° Cu2+ was 0.34 V? 9. What problem is associated with assigning reduction potentials? How is this overcome? 10. On pg. 713, half-cell equations are shown for copper and hydrogen.
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Unformatted text preview: Based on these equations, which half-cell has the greatest reduction potential? 11. On pg. 714, explain where the 0.00 V in “0.34 V = E ° Cu2+- 0.00 V” comes from and why the value is zero. 12. What does a negative E ° value indicate about a half-cell? 13. The double arrows in table 17.1 are not meant to suggest that an equilibrium exists. What do they indicate? 14. Solve for PE 6 (pg. 716). Show your work. 15. What is the maximum voltage that can be produced by a single cell under standard conditions (25 ° C and 1 M solutions)? Explain. 16. What would the voltage be in the following cells:a) Ni - Au, b) Ag - Cu, c) Mg - Al, d) Cu - Fe? 17. Is it accurate to say that E ° cell = E ° larger reduction potential- E ° smaller reduction potential ? Explain with reference to equation 17.2 on pg. 712. 18. Will the voltage from a cell always be positive? Why or why not?...
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