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Standard XII

Chemistry

Representation of Cell

The values fo...

Question

The values for cell is
$Z n | Z n^{2 +} (a q) | | C u^{2 +} (a q) | C u$
$E^{o}$ for Cu and Zn are $0.35$ and $- 0.76$ respectively: then what will be the cell reaction?

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Solution

The cell reaction is : $Z n + C u^{2 +} \to$ $C u + Z n^{2 +}$

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

E^{o}

for

C u

and

Z n

are

0.35

and

- 0.76

respectively:

Find EMF of cell (nearest integer) if

Z n^{2 +}

and

C u^{2 +}

are 1 M each.

E^{\circ}

for the electrochemical cell,

Z n (s) | Z n^{2 +} 1 M (a q .) ∥ C u^{2 +} 1 M (a q .) | C u (s)

1.10 V

25^{\circ} C

. The equilibrium constant for the cell reaction,

Z n (s) + C u^{2 +} (a q .) ⇌ Z n^{2 +} (a q .) + C u (s)

will be:

$E^{0}$ for the cell, $Z n | Z n {^{2 +}}_{(a q)} | | C u {^{2 +}}_{(a q)} | C u$ is $1.10 V$ at $25^{0} C$ . The equilibrium constant for $Z n + C u {^{2 +}}_{(a q)} \to Z n {^{2 +}}_{(a q)} + C u$ the cell reaction is of the order of :

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

0.350

V for

C u^{2 +} (a q) + 2 e^{-} \to C u

and

- 0.763

V for

Z n^{2 +} (a q) + 2 e^{-} \to Z n

The cell reaction is:

E^{\circ}

for the cell is

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

25^{\circ} C

, the equilibrium constant for the reaction

Z n + C u^{2 +} (a q) ⇌ C u + Z n^{2 +} (a q)

is of the order of

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The values for cell isZn|Zn2+(aq)||Cu2+(aq)|CuEo for Cu and Zn are 0.35 and −0.76 respectively: then what will be the cell reaction?

The cell reaction is : Zn+Cu2+→ Cu+Zn2+

The values for cell is
$Z n | Z n^{2 +} (a q) | | C u^{2 +} (a q) | C u$
$E^{o}$ for Cu and Zn are $0.35$ and $- 0.76$ respectively: then what will be the cell reaction?

The cell reaction is : $Z n + C u^{2 +} \to$ $C u + Z n^{2 +}$