1. A battery is constructed from these two half reactions: not balanced CCr not
ID: 1046632 • Letter: 1
Question
1. A battery is constructed from these two half reactions: not balanced CCr not balanced) CIO: (g) E 1.33 Vvs SHE B 0.954 V CO (a) (1 pts) Balance each halfreaction. Assume acid solution, pH = 2.00. (b) (0.5 pts) Derive the overall balanced equation for the battery reaction. (c) (0.4 pts) the oxidizing agent is (d) (0.5 pts) Eovell for the battery is The reducing agent is Show your calculation here) (e) (1 pt) Write the shorthand "line" notation of the battery. Put the anode compartment on the left.Explanation / Answer
1. For the given cell
(a) balanced equations,
Cr2O7^2- + 14H+ + 6e- --> 2Cr3+ + 7H2O
ClO2 + e- --> ClO2-
(b) overall equation,
6ClO2- + Cr2O7^2- + 14H+ ---> 6ClO2 + 2Cr3+ + 7H2O
(c) oxidizing agent : Cr2O7^2- Reducing agent : ClO2-
(d) Eo = Ecathode - Eanode
= 1.33 - 0.954 = 0.376 V
(e) Cell notation,
Cr2O7^2-,H+ | Cr3+ || ClO2- | ClO2
(f) Ecell = Eo - 0.0592/n logK
= 0.376 - 0.0592/6 log[(0.0125)^2 x (0.3)^6/(0.050) x (1 x 10^-2)^14 x (0.00527)^6]
= 0.0335 V
(g) When battery is at equilibrium,
Ecell = 0
(h) at standard conditions
Ecell = 0.376 - 0.0592/6 log(1)
= 0.376 V
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