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Gibb's Energy and Nernst Equation

For the given...

Question

For the given cell reaction :
$C u^{2 +} (a q) + 2 C l^{-} (a q) \to C u (s) + C l_{2} (g)$
$E_{c e l l}^{\circ}$ is given as $- 1.02 V$ .
Which of the following is correct?

A

The given reaction is spontaneous

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B

Reaction will occur whenever

C u^{2 +}

and

C l^{-}

are brought together in an aqueous solution.

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C

The given reaction is non-spontaneous

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D

The reaction is in equilibrium

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Solution

The correct option is C The given reaction is non-spontaneous
For a given reaction to be spontaneous, $E_{c e l l}^{\circ} > 0$

For the reaction , since $E_{c e l l}^{\circ}$ has a negative value ,

So, the given reaction is a non-spontaneous redox reaction

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Similar questions

E_{c e l l}^{\circ}

, for the reaction (

C u^{2 +} (a q) + 2 C l^{-} (a q) \to C u (s) + C l_{2} (g)

- 1.02 V

.
Choose the correct statement.

Q. Which of the following is the cell representation for the given cell reaction?

Z n (s) + C u^{2 +} (a q) \to Z n^{2 +} (a q) + C u (s)

Q. The cell reaction of the given galvanic cell,

C u_{(s)} | C u_{(a q)}^{2 +} | | H g_{(a q)}^{2 +} | H g_{(l)}

Q. The reaction

C u^{2 +} (e q) + 2 C l^{⊖} (a q) \to C u (s) + C l_{2} (g)

E_{c e l l}^{⊖} = - 1.03 V

. This reaction:

Q. Which of the following represents the anode half-cell reaction for the following galvanic cell:

C u (s) | C u^{2 +} (a q) | | A g^{+} (a q) | A g (s)

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Gibb's Energy and Nernst Equation

Standard VII Chemistry

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