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Write the cell notation for an electrochemical cell consisting of an anode where Mn (s) is oxidized to Mn \( { }^{2+} \) (aq) and a cathode where \( \mathrm{Co}^{2+}(\mathrm{aq}) \) is reduced to Co (s). Assume all aqueous solutions have a concentration of \( 1 \mathrm{~mol} / \mathrm{L} \). 9 more group attempts remaining
Write the cell notation for an electrochemical cell consisting of an anode where \( \mathbf{A l}(\mathbf{s}) \) is oxidized to \( \mathbf{A l}^{3+} \) \( \mathbf{( a q )} \) and a cathode where \( \mathbf{F e}^{3+}(\mathbf{a q}) \) is reduced to \( \mathbf{F e}^{2+}(\mathbf{a q}) \) at a platinum electrode. Assume all aqueous solutions have a concentration of \( 1 \mathrm{~mol} / \mathrm{L} \).
Expert Answer
Q-1 Answer of the question is = Mn|Mn2+(1M) || Co2+(1M)|Co Solution :- In the question given, Concentration of [Mn2+] = 1 M Concentration of [Co2+] = 1 M The cathode reaction of the cell is(reduction) -> Co2+(aq) +2e- ? Co(s) ---------(i) The anode r