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Suppose you build a galvanic cell using silver and chromium electrodes. a) Determine which electrode is the cathode and which is the anode under standard conditions (explain how you know). b) Write the half-reactions and the balanced complete reaction under standard conditions. c) Calculate the standard cell potential for your galvanic cell (walk through your work). d) Now suppose you have 0.100 M silver ions in the silver half-cell and 0.250 M chromium ions in the chromium half- cell. Calculate the cell potential under these conditions. Compare the answers for (c) and (d), and explain how the difference you see makes sense in terms of equilibrium.

Suppose you build a galvanic cell using silver and chromium electrodes. a) Determine which electrode is the cathode and which is the anode under standard conditions (explain how you know). b) Write the half-reactions and the balanced complete reaction under standard conditions. c) Calculate the standard cell potential for your galvanic cell (walk through your work). d) Now suppose you have 0.100 M silver ions in the silver half-cell and 0.250 M chromium ions in the chromium half- cell. Calculate the cell potential under these conditions. Compare the answers for (c) and (d), and explain how the difference you see makes sense in terms of equilibrium.

Principles of Modern Chemistry
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 60P
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Part a,b,c,d properly solution

Suppose you build a galvanic cell using silver and chromium electrodes. a) Determine which electrode is the cathode and which is the anode under standard conditions (explain how you know). b) Write the half-reactions and the balanced complete reaction under standard conditions. c) Calculate the standard cell potential for your galvanic cell (walk through your work). d) Now suppose you have 0.100M silver ions in the silver half-cell and 0.250 M chromium ions in the chromium half- cell. Calculate the cell potential under these conditions. Compare the answers for (c) and (d), and explain how the difference you see makes sense in terms of equilibrium.
Transcribed Image Text:Suppose you build a galvanic cell using silver and chromium electrodes. a) Determine which electrode is the cathode and which is the anode under standard conditions (explain how you know). b) Write the half-reactions and the balanced complete reaction under standard conditions. c) Calculate the standard cell potential for your galvanic cell (walk through your work). d) Now suppose you have 0.100M silver ions in the silver half-cell and 0.250 M chromium ions in the chromium half- cell. Calculate the cell potential under these conditions. Compare the answers for (c) and (d), and explain how the difference you see makes sense in terms of equilibrium.
5. Which of the following is an example of a Lewis acid-base reaction, but not a Brønsted- Lowry acid-base reaction? А. 2C1O,²¯(aq) + 2H* (aq) →Cr,O, (aq) + H,O (1) В. Со(Н,0), * (аq) + 4HC1(aq) —> СОС1,;" (аq) + 4н" (аq) + бH,о() C. NH;(aq)+H*(aq) → NH,*(aq) D. CHCоо "(аq) + H,о(1) —СH,соон (аq) + Он (аq)
Transcribed Image Text:5. Which of the following is an example of a Lewis acid-base reaction, but not a Brønsted- Lowry acid-base reaction? А. 2C1O,²¯(aq) + 2H* (aq) →Cr,O, (aq) + H,O (1) В. Со(Н,0), * (аq) + 4HC1(aq) —> СОС1,;" (аq) + 4н" (аq) + бH,о() C. NH;(aq)+H*(aq) → NH,*(aq) D. CHCоо "(аq) + H,о(1) —СH,соон (аq) + Он (аq)
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