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Standard XII

Chemistry

Electron Gain Enthalpy

Using the sta...

Question

Using the standard electrode potentials given in the table, predict if the reaction between the following is possible.
$A g_{(a q)}^{+}$ and $C u_{(s)}$

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Solution

Oxidation half reaction is $C u (s) \to C u^{2 +} (a q) + 2 e^{-}; E^{0} = - 0.34 V$ .
Reduction half reaction is $[A g^{+} (a q) + e^{-} \to A g (s)] \times 2; E^{0} = + 0.80 V$ .
The net cell reaction is $2 A g^{+} (a q) + C u (s) \to 2 A g (s) + C u^{2 +}; E^{0} = + 0.46 V$ .

Since the cell potential is positive, the reaction is feasible.

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$E_{\frac{1}{2} \frac{t_{2}}{1^{-}}}^{\circ} = + 0.541 V E_{(\frac{C u^{2 +}}{C u})}^{\circ} = + 0.34 V E_{(\frac{1}{2} \frac{B r_{2}}{B r^{-}})}^{\circ} = + 1.09 V E_{(\frac{A g^{+}}{A g})}^{\circ} = + 0.80 V E_{(\frac{F e^{3 +}}{F e^{2 +}})}^{\circ} = + 0.77 V$

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Using the standard electrode potentials given in the table, predict if the reaction between the following is possible.Ag+(aq) and Cu(s)

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