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Standard XII

Chemistry

Redox Reactions and Couple

The standard ...

Question

The standard electrode potential of Cu and Ag are 0.34V and 0.80V respectively. Calculate the cell potential (E) for the cell containing 0.100M Ag⁺and 4.00 M Cu²⁺at 25°C

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Solution

$T h e r e a c t i o n o c c u r i n a n o d e a n d c a t h o d e A d : C u \to C u^{2 +} + 2 e^{-} E^{0} = - 0.34 V C d : 2 A g^{+} + 2 e^{-} \to 2 A g E^{0} = 0.80 - - - - - - - - - - - - - C u + 2 A g^{+} \to C u^{2 +} + 2 A g - - - - - - - - - - - - - - E^{0} = E_{o x}^{0} + E_{r e d}^{0} = - 0.34 + 0.80 = 0.46 V E_{c e l l} = E^{0} - \frac{0.0591}{n} \log \frac{[C u^{2 +}]}{[A g^{+}]^{2}} = 0.46 - \frac{0.0591}{2} \log \frac{[4]}{[0.1]^{2}} = 0.3831 V$

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Similar questions

Q. The standard electrode potential of

A g^{+} / A g

+ 0.80 V

and of

C u^{2 +} / C u

+ 0.34 V

. These electrodes are connected through a salt bridge and if:

Q. The standard reduction potentials for

C u^{2 +} / C u

and

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

are

0.337 V

and

0.153 V

respectively. The standard electrode potential of

C u^{+} / C u

half cell is:

Q. The standard reduction potentials of

C u^{2 +} | C u

and

A g^{+} | A g

electrodes are

0.337

and

0.799 v o l t s

respectively. Construct a galvanic cell using these electrodes so that its standard emf is positive. For what concentration of

A g^{+}

will the emf of the cell at

25^{\circ} C

be zero if concentration of

C u^{2 +}

0.01 M

Q. Standard emf of cell = 0.463 vCu/

{C u}^{+ 2}

(M) ll

{A g}_{+}

(1 M)

1 A g

If standard potential of Cu electrode is 0.337v then what is standard potential of Ag electrode?

The e.m.f. of the cell at $25^{\circ} C$
$\frac{C u}{C u^{2 +} (0.01 M)} | | \frac{A g^{+} (0.1 M)}{A g}$
is $[E^{0} (\frac{C u^{2 +}}{C u}) = 0.34 V a n d E^{0} (\frac{A g +}{A g}) = 0.80 V]$

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The standard electrode potential of Cu and Ag are 0.34V and 0.80V respectively. Calculate the cell potential (E) for the cell containing 0.100M Ag+ and 4.00 M Cu2+ at 25°C

The reaction occur in anode and cathode Ad: Cu →Cu2+ + 2e- E0 = - 0.34 VCd: 2 Ag+ + 2e- → 2 Ag E0 = 0.80-------------Cu + 2 Ag+ →Cu2+ + 2 Ag--------------E0 = Eox0 + Ered0 = - 0.34 + 0.80 = 0.46 VEcell = E0 - 0.0591 n log [Cu2+][Ag+]2 = 0.46 - 0.0591 2 log [4][0.1]2 = 0.3831 V

The standard electrode potential of Cu and Ag are 0.34V and 0.80V respectively. Calculate the cell potential (E) for the cell containing 0.100M Ag⁺and 4.00 M Cu²⁺at 25°C