The E - for Cu 2- - Cu - - Cu - - Cu - Cu 2- - Cu are 0-15 V - 0-50 V and 0-325 V respectively- The redox cell showing redox reaction 2 Cu -Cu 2- Cu is made- The E - of this cell reaction and - G - may be-A- - G -33-775 kJB- All of these C- E -0-175 V or E -0-350 VD- n-1 or 2

The correct option is B All of these 2Cu^+ → Cu^2++Cu; Cell I : Cu^+ → Cu^2++e Cu^+ +e → Cu 2Cu^+ → Cu^2++Cu E^∘ = 0.15+0.50 =+0.35 V n=1 Cell II: Cu → Cu^2+ + ...

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Byju's Answer

Standard XII

Chemistry

Equilibrium Constant from Nernst Equation

The E ∘ for C...

Question

The $E^{\circ}$ for $C u^{2 +} / C u^{+}$ ; $C u^{+} / C u$ , $C u^{2 +} / C u$ are 0.15V, 0.50 V and 0.325 V respectively. The redox cell showing redox reaction $2 C u^{+} \to C u^{2 +} + C u$ is made. The $E^{\circ}$ of this cell reaction and $Δ G^{\circ}$ may be:

$E^{\circ} = 0.175 V$ or $E^{\circ} = 0.350 V$

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n = 1 or 2

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$Δ G^{\circ} = 33.775 k J$

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All of these

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Solution

The correct option is D
All of these

$2 C u^{+} \to C u^{2 +} + C u$ ;

Cell I :

$C u^{+} \to C u^{2 +} + e$

$C u^{+} + e \to C u$

$2 C u^{+} \to C u^{2 +} + C u$

$E^{\circ} = - 0.15 + 0.50$

$= + 0.35 V$

$n = 1$

Cell II:

$C u \to C u^{2 +} + 2 e$

$2 C u^{+} + 2 e \to 2 C u$

$2 C u^{+} \to C u^{2 +} + C u$

$E^{\circ} = - 0.325 + 0.50$

$= + 0.175 V$

$n = 2$

Suggest Corrections

Similar questions

Q. The

E^{⊖} f o r C u^{2 +} / C u^{\oplus}, C u^{\oplus} / C u, C u^{2 +} / C u,

are 0.15 V, 0.50 V, and 0.325 V, respectively. The redox cell showing redox reaction

2 C u^{+}, \to C u^{2 +} + C u

is made.

E^{⊖}

of this cell reaction and

Δ G^{⊖}

may be :

Q. Find the change in standard gibb's free energy

(Δ G^{\circ})

for the following reaction.

2 C u^{+} \to C u + C u^{2 +}

(Given :

E_{C u^{+} / C u}^{\circ} = 0.52 V, E_{C u^{2 +} / C u^{+}}^{\circ} = 0.16 V

)

Q. The electrode potentials for :

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

and

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

are +0.15V and +0.50V respectively. The value of

E_{C u^{2 +} / C u}^{\circ}

will be:

Q. If for the half cell reactions

C u^{2 +} + e^{-} \to C u^{+}

E^{o} = 0.15 V

C u^{2 +} + 2 e^{-} \to C u

E^{o} = 0.34 V

Calculate

E^{o}

of the half cell reaction

C u^{+} + e^{-} \to C u

also predict whether

C u^{+}

undergoes disproportionation or not.

Q. If for the following half-cell reactions :

C u^{2 +} + e^{-} \to C u^{\oplus}

;

E^{\oplus} = 1.77 V

C u^{2 +} + 2 e^{-} \to C u

;

E^{⊖} = - 0.34

The

E^{⊖}

of the half-cell reaction will be (in V)

C u^{\oplus} + e^{-} \to C u

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The E∘ for Cu2+/Cu+ ; Cu+/Cu,Cu2+/Cu are 0.15V, 0.50 V and 0.325 V respectively. The redox cell showing redox reaction 2Cu+→Cu2++Cu is made. The E∘ of this cell reaction and ΔG∘ may be:

The correct option is D All of these 2Cu+→Cu2++Cu; Cell I : Cu+→Cu2++e Cu++e→Cu 2Cu+→Cu2++Cu E∘=−0.15+0.50 =+0.35 V n=1 Cell II: Cu→Cu2++2e 2Cu++2e→2Cu 2Cu+→Cu2++Cu E∘=−0.325+0.50 =+0.175 V n=2

The $E^{\circ}$ for $C u^{2 +} / C u^{+}$ ; $C u^{+} / C u$ , $C u^{2 +} / C u$ are 0.15V, 0.50 V and 0.325 V respectively. The redox cell showing redox reaction $2 C u^{+} \to C u^{2 +} + C u$ is made. The $E^{\circ}$ of this cell reaction and $Δ G^{\circ}$ may be: