We’re being asked to sketch a galvanic cell for the following reaction:
Cr3+ (aq) + Cl2 (g) ⇌ Cr2O72- (aq) + Cl - (aq)
Recall that a voltaic or galvanic cell is an electrochemical cell that is spontaneous and produces electricity.
From the reaction, we can see that the oxidation state of Cr went from +3 (Cr3+) to +6 (Cr2O72-) which means it was oxidized or lost electrons.
The anode (–) half-reaction is:
2 Cr3+(aq) + 7 H2O(l) → Cr2O72-(aq) + 14 H+(aq) + 6e-
6 e– to the product side
The other half-reaction is then reduced or gained electrons.
The cathode (+) half-reaction is:
Cl2(g) + 2 e– → 2 Cl-(aq)
2(–1) + 8(+1) + x = 0
2 e– to the reactant side
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.
a. Cr3+ (aq) + Cl2 (g) ⇌ Cr2O72- (aq) + Cl - (aq)
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.