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Byju's Answer

Standard XII

Chemistry

Redox Reactions and Couple

The cell pote...

Question

The cell potential for the electrochemical reaction shown below depends upon the $C l^{-}$ and $C u^{2 +}$ concentrations. Calculate the cell potential (in V) at $25^{0} C$ if [ $C u^{2 +}$ ] = 3.5 M and [ $C l^{-}$ ] = 1.7 M.
$C u^{2 +}$ (aq) + 2 $C l^{-}$ (aq) + 2Ag(s) $\Leftrightarrow$ Cu(s) + 2AgCl(s) ; E = 0.12 V

0.15 V

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- 0.15 V

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0.30 V

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-0.30 V

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Solution

The correct option is B 0.15 V
Using Nearest Equation :-
$\begin{matrix} E_{c e l l} = E_{c e l l}^{\circ} - \frac{0.059}{n} log \frac{1}{{[C 1^{θ}]}^{2} [C u^{21}]} a t 25^{\circ} C E_{c e l l} = 0.12 - \frac{0.059}{2 \times 0} log \frac{1}{{(1.7)}^{2} (3.5)} \Rightarrow 0.12 - \frac{0.059}{2 \times 0} log (0.099) \Rightarrow 0.12 - (- 0.029) \Rightarrow 0.12 + 0.029 = 0.15 V = E_{c e l l}^{\circ} \end{matrix}$

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Similar questions

Q. 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 potentials are

+ 0.35 V

for

2 e^{-} + C u^{2 +} (a q) \to C u^{2 +} (a q) (1.0 M) | C u

The standard reduction potentials are

+ 0.35 V

for

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

and

- 0.763 V

for

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

Calculate the emf of the cell and tell whether the cell reaction spontaneous or not ?

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:

Q. The electrode potentials for

C u^{2 +} (a q) + e^{-} \to C u^{+} (a q) and C u^{2 +} (a q) + e^{-} \to C u (s) are + 0.15 V and + 0.50 V

respectively. The value of

E_{C u^{2 +} / C u}^{0}

will be:

Q. In a cell reaction;

C u_{(s)} + 2 A g_{(a q)}^{+} \to C u_{(a q)}^{2 +} + 2 A g_{(s)}

E_{c e l l}^{o} = + 0.46

V. If the concentration of

C u^{2 +}

ions is doubled then

E_{c e l l}^{o}

will be:

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

Assertion: The reaction is spontaneous.

Reason: The cell potential is positive.

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The cell potential for the electrochemical reaction shown below depends upon the Cl− and Cu2+ concentrations. Calculate the cell potential (in V) at 250C if [ Cu2+] = 3.5 M and [Cl−] = 1.7 M.Cu2+(aq) + 2Cl−(aq) + 2Ag(s) ⇔ Cu(s) + 2AgCl(s) ; E = 0.12 V

The correct option is B 0.15 VUsing Nearest Equation :-Ecell=E∘cell−0.059nlog1[C1θ]2[Cu21]at25∘CEcell=0.12−0.0592×0log1(1.7)2(3.5)⇒0.12−0.0592×0log(0.099)⇒0.12−(−0.029)⇒0.12+0.029=0.15V=E∘cell