The cell shown below has a measured cell potential of +0.06839 V at 25.0 °C. A graph of the cell potential as a function of temperature is linear in the temperature range 20 °C to 30 °C with a slope of +4.18x10 V-K. Ag (s) | AgBr (5) | KBr (aq) | Hg2Bra (S) | Hg () From this information, calculate the following. Enter each numerical value with its sign to the correct number of significant figures with the units indicated. kl-mole 450 JK1.mole

The cell shown below has a measured cell potential of +0.06839 V at 25.0 °C. A graph of the cell potential as a function of temperature is linear in the temperature range 20 °C to 30 °C with a slope of +4.18x10 V-K. Ag (s) | AgBr (5) | KBr (aq) | Hg2Bra (S) | Hg () From this information, calculate the following. Enter each numerical value with its sign to the correct number of significant figures with the units indicated. kl-mole 450 JK1.mole

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 59P

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From the standard potentials Ag2SeO4(s)+2e2Ag(s)+SeO42-E0=0.355V Ag++2eAg(s)E0=0.799V calculate the solubility product constant for Ag2SeO4.
Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.