Consider the following half cells Cu s - Cu aq 2-2 e - - E 0-0-325 VCu aq - e - Cu s - E 0-0-50 VThe E 0 for the reaction 2 Cu aq - Cu aq 2- Cu s isA- 0-175 VB- 0-35 VC- 0-675 VD- 0-3375 V

The correct option is A 0.175 V(1) Cu_(s)→ Cu^2+_(aq) + 2e^ ; E^∘_1 = 0.325 V (2) Cu^+_(aq)+ e^ → Cu_(s) ; E^∘_2 = 0.50 V The required reaction is: n ...

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Byju's Answer

Standard XII

Chemistry

EMF

Consider the ...

Question

Consider the following half cells
$C u_{(s)} \to C u_{(a q)}^{2 +} + 2 e^{-}; E^{o} = - 0.325 V$
$C u_{(a q)}^{+} + e^{-} \to C u_{(s)}; E^{o} = 0.50 V$
The $E^{o}$ for the reaction $2 C u_{(a q)}^{+} \to C u_{(a q)}^{2 +} + C u_{(s)}$ is

0.175 V

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0.35 V

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0.675 V

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0.3375 V

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Solution

The correct option is A 0.175 V
(1) $C u_{(s)} \to C u_{(a q)}^{2 +} + 2 e^{-}; E_{1}^{\circ} = - 0.325 V$
(2) $C u_{(a q)}^{+} + e^{-} \to C u_{(s)}; E_{2}^{\circ} = 0.50 V$

The required reaction is: $2 C u_{(a q)}^{+} \to C u_{(a q)}^{2 +} + C u_{(s)}$

We need to combine the two above mentioned reactions so as to form the final reaction and the resultant standard EMF will be a summation of the $E^{o}$ of the combining reactions.

$E_{3}^{\circ} = - 0.325 + 0.5 = 0.175 V$

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Similar questions

Q. 1.

C u^{2 +} + 2 e^{-} ⟶ C u

E^{0} = 0.337 V

C u^{2 +} + e^{-} ⟶ C u^{+}

E^{0} = 0.153 V

Electrode potential,

E^{0}

for the reaction

C u^{+} + e^{-} ⟶ C u

Q. The standard reduction potentials EO, for the half reaction are as

Z n \to Z n^{+ +} + 2 e^{-}, E^{0} = 0.76 V

C u \to C u^{+ +} + 2 e^{-}, E^{0} = 0.34 V

The e.m.f. for the cell reaction,

Q. Which of the following reaction will provide maximum voltage?
Given:

Z n^{2 +} (a q) + 2 e^{-} \to Z n (s); E^{0} = - 0.76 V

C u^{2 +} (a q) + 2 e^{-} \to C u (s); E^{0} = 0.34 V

A g^{+} (a q) + e^{-} \to A g (s); E^{0} = 0.80 V

2 H^{+} (a q) + 2 e^{-} \to H_{2} (g); E^{0} = 0 V

N i^{2 +} (a q) + 2 e^{-} \to N i (s); E^{0} = - 0.25 V

Q. Which of the following metals, when coupled, will leads to a non-spontaneous cell reaction?
Given:

A u^{+} (a q) + e^{-} \to A u (s); E^{0} = 1.69 V

C u^{2 +} (a q) + 2 e^{-} \to C u (s); E^{0} = 0.34 V

P b^{2 +} (a q) + 2 e^{-} \to P b (s); E^{0} = - 0.13 V

F e^{2 +} (a q) + 2 e^{-} \to F e (s); E^{0} = - 0.44 V

C a^{2 +} (a q) + 2 e^{-} \to C a (s); E^{0} = - 2.87 V

Q. Which of the following metals will couple to provide a higher cell potential for a galvanic cell?

Z n^{2 +} (a q) + 2 e^{-} \to Z n (s); E^{0} = - 0.76 V

C u^{2 +} (a q) + 2 e^{-} \to C u (s); E^{0} = 0.34 V

N i^{2 +} (a q) + 2 e^{-} \to N i (s); E^{0} = - 0.25 V

P b^{2 +} (a q) + 2 e^{-} \to P b (s); E^{0} = - 0.13 V

F e^{2 +} (a q) + 2 e^{-} \to F e (s); E^{0} = - 0.44 V

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Consider the following half cells Cu(s)→Cu2+(aq)+2e− ; Eo=−0.325 V Cu+(aq)+e−→Cu(s) ; Eo=0.50 V The Eo for the reaction 2Cu+(aq)→Cu2+(aq)+Cu(s) is

Consider the following half cells
$C u_{(s)} \to C u_{(a q)}^{2 +} + 2 e^{-}; E^{o} = - 0.325 V$
$C u_{(a q)}^{+} + e^{-} \to C u_{(s)}; E^{o} = 0.50 V$
The $E^{o}$ for the reaction $2 C u_{(a q)}^{+} \to C u_{(a q)}^{2 +} + C u_{(s)}$ is