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2 years ago

Is Cu^2+ + 2Br^- --> Cu + Br2 a spontaneous or non-spontaneous redox reaction?

Chemistry

1 answer:

lawyer [7]2 years ago

3 0

The reaction above is a spontaneous reaction

Cu^2+ + 2Br^- --> Cu + Br2

<h3>What is spontaneous redox reaction?</h3>

A spontaneous redox reaction is a special type of redox reaction which involves the release of energy where the electrons are transferred from from an anode to the cathode

General spontaneous redox reactions is found mostly in electrochemical cells

So therefore, the reaction above is a spontaneous reaction.

Cu^2+ + 2Br^- --> Cu + Br2

Learn more about spontaneous redox reactions:

brainly.com/question/4428247

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Solution :

The balanced cell reaction will be,

$Cu(s)+2Ag^+(aq)\rightarrow Cu^{2+}(aq)+2Ag(s)$

Here, magnesium (Cu) undergoes oxidation by loss of electrons, thus act as anode. silver (Ag) undergoes reduction by gain of electrons and thus act as cathode.

The half oxidation-reduction reaction will be :

Oxidation : $Cu\rightarrow Cu^{2+}+2e^-$

Reduction : $2Ag^++2e^-\rightarrow 2Ag$

Now we have to calculate the Gibbs free energy.

Formula used :

$\Delta G^o=-nFE^o$

where,

$\Delta G^o$ = Gibbs free energy = ?

n = number of electrons to balance the reaction = 2

F = Faraday constant = 96500 C/mole

$E^o$ = standard e.m.f of cell = 0.46 V

Now put all the given values in this formula, we get the Gibbs free energy.

$\Delta G^o=-(2\times 96500\times 0.46)=-88780J/mole$

Therefore, the $\Delta G$ for this reaction is, -88780 J/mole.

7 0

3 years ago

9. How many protons, neutrons, and electrons does 35C1l- have?

Alekssandra [29.7K]

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3 years ago

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Blababa [14]

Answer:

Explanation:

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3 years ago

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Answer: check explanation

Explanation:

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3 years ago

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