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A cell is prepared by dipping copper rod...

A cell is prepared by dipping copper rod in 1 M copper sulphate solution and zinc rod in 1 M zinc sulphate solution. The standard reduction potential of copper and zin c are `0.34 V and - `0.76 V respectively.
(i) What will be the cell reaction ?
(ii) What will be the standard electromotive force of the cell ?
(iii) Which electrode will be positive ?

Text Solution

AI Generated Solution

To solve the problem step by step, we will address each part of the question systematically. ### Step 1: Determine the Cell Reaction 1. **Identify the half-reactions**: - For zinc (Zn), which has a lower reduction potential (-0.76 V), it will undergo oxidation: \[ \text{Zn (s)} \rightarrow \text{Zn}^{2+} (aq) + 2e^- ...
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A cell is prepared by dipping a copper rod in 1 MCuSO_(4) solution and a nickel rod in 1M NiSO_(4) . The standard reduction potentials of copper and nickel electrodes are +0.34 V and -0.25 V respectively. (i) Which electrode will work as anode and which as cathode? (ii) What will be the cell reaction? (iii) How is the cell represented ? (iv) Calculate the EMF of the cell.

Knowledge Check

  • Which cell will measure standard electrode potential of copper electrode?

    A
    `Pt_((s))|H_2(g,0.1 "bar") |H^(+) (aq, 1 M) || Cu^(2+) (aq, 1M) |Cu`
    B
    `Pt_((s))|H_2(g,1 "bar") |H^(+) (aq, 1 M) || Cu^(2+) (aq, 2M) |Cu`
    C
    `Pt_((s))|H_2(g,1 "bar") |H^(+) (aq, 1 M) || Cu^(2+) (aq, 1M) |Cu`
    D
    `Pt_((s))|H_2(g,1 "bar") |H^(+) (aq, 0.1 M) || Cu^(2+) (aq, 1M) |Cu`

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