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Ad libitum [116K]
3 years ago
7

The standard cell potential Ec for the reduction of silver ions with elemental copper is 0.46V at 25 degrees celsius. calculate

ΔG for this reaction.
*** Please explain the reactions since I’m very confused as to wich side I should put the electrons.
Ex: Cu-> Cu2+ + 2e
Chemistry
1 answer:
Cloud [144]3 years ago
7 0

Answer : The \Delta G for this reaction is, -88780 J/mole.

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.

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Verdich [7]

Answer:

There is  2.52 kJ of energy released (option 4)

Explanation:

Step 1: Data given

The enthalpy of fusion of methanol (CH3OH) is 3.16 kJ/mol

Mass of methanol = 25.6 grams

Molar mass of methanol = 32.04 g/mol

Step 2: Calculate moles of methanol

Moles methanol = mass methanol / molar mass methanol

Moles methanol = 25.6 grams / 32.04 g/mol

Moles methanol = 0.799 moles

Step 3: Calculate energy transfer

Energy  transfer = moles * enthalpy of fusion

Energy = 0.799 moles * 3.16 kJ/mol

Energy = 2.52 kJ released

There is  2.52 kJ of energy released

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The Pauli Exclusion Principle tells us that no two electrons in an atom can have the same four quantum numbers.
Anuta_ua [19.1K]

Answer:

See explanation

Explanation:

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