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Calculate the...

Question

Calculate the reduction potential for the following half cell at $25^{o} C$ .

$C u (s) | C u^{2 +} (a q, 0.2 M); E_{C u / C u^{2 +}}^{0} = - 0.34 V$

Take :
[ $l o g_{10} 5 = 0.7$ ]

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Solution

$C u (s) | C u^{2 +} (a q, 0.2 M); E_{C u^{2 +} / C u}^{0} = 0.34 V$

$E_{C u^{2 +} / C u} = E_{C u^{2 +} / C u}^{0} - \frac{2.303 R T}{n F} l o g \frac{[M (s)]}{[M^{n +} (a q)]}$

$n = 2$

$E_{C u^{2 +} / C u} = 0.34 - \frac{0.059}{2} l o g \frac{1}{[C u^{2 +}]}$

$E_{C u^{2 +} / C u} = 0.34 - \frac{0.059}{2} l o g \frac{1}{[0.2]}$

$E_{C u^{2 +} / C u} = 0.34 - \frac{0.059}{2} \times l o g 5$

$E_{C u^{2 +} / C u} = 0.34 - \frac{0.059}{2} \times 0.7 \approx 0.32 V$

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Similar questions

The cell potential for the electrochemical reaction shown below depends upon the

C l^{-}

C u^{2 +}

concentrations. Calculate the cell potential (in V) at

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] = 3.5 M and [

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C l^{-}

\Leftrightarrow

Cu(s) + 2AgCl(s) ; E = 0.12 V

Q. The standard reduction potentials for

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C u^{2 +} / C u^{+}

0.337 V

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respectively. The standard electrode potential of

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Consider the cell:

Z n | Z n^{2 +} (a q) (1.0 M) | | C u^{2 +} (a q) (1.0 M) | | C u

The standard reduction potential are

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- 0.763

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The cell reaction is:

Q. Calculate the reduction potential for the following half cell at

25^{o} C

C u (s) | C u^{2 +} (a q, 0.2 M); E_{C u^{2 +} / C u}^{0} = 0.34 V

l o g_{10} 5 = 0.7

]

Q. Solve

The e.m.f. of the cell

C u (s) |C u^{2 +} (a q) ∥ A g^{+} (a q)| A g (s) i s 0.46 V . T h e s \tan d a r d r e d u c t i o n p o t e n t i a l o f A g^{+} / A g i s 0.50 V . T h e s \tan d a r d r e d u c t i o n p o t e n t i a l o f C u^{2 +} Ι C u w i l l b e a) - 0.34 V b) 1.26 V c) - 1.26 V d) 0.34 V

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