Label the reducing agent and the oxidizing agent and describe the direction of t
ID: 962107 • Letter: L
Question
Label the reducing agent and the oxidizing agent and describe the direction of the electron flow Determine the standard cell potential. Which electrode increases in mass as the reaction proceeds. and which electrode decreases in mass? Sketch the galvanic cells based on the following overall reactions. Show the direction of electron flow, and identify the cathode and anode. Give the overall balanced equation. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm. Sketch the galvanic cells based on the following overall reactions. Show the direction of electron flow, the direction migration through the salt bridge, and identify the anode. Give the overall balanced equation. Assume that all eventrations are 1.0 A/and that all partial pressures are 1.0 atmExplanation / Answer
37. (a): Oxidation - half cell: 2Cr3+ + 7H2O ------ > Cr2O72 + 14H+ + 6e ; E0(oxi) = - 1.33 V
Reduction - half reaction: 3Cl2(g) + 6 e- ------ > 6 Cl-(aq); E0(red) = + 1.36 V
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Overall reaction: 2Cr3+ + 7H2O + 3Cl2(g) -------- > Cr2O72 + 14H+ + 6 Cl-(aq)
E0(cell) = E0(oxi) + E0(red) = - 1.33 V + 1.36 V = + 0.03 V (answer)
(b): Oxidation - half cell: Mg(s) ------ > Mg2+(aq) + 2e ; E0(oxi) = +2.372 V
Reduction - half reaction: Cu2+(aq) + 2e ------ > Cu(s) ; E0(red) = + 0.337 V
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Overall reaction: Cu2+(aq) + Mg(s) -------- > Mg2+(aq) + Cu(s)
E0(cell) = E0(oxi) + E0(red) = 2.372 V + 0.337 V = + 2.709 V (answer)
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