On the basis of information available from the reaction 4-3Al-O2-2-3Al2O3- - G-827 kJ-mol-1The minimum emf required to carry out the electrolysis of Al2O3 is- -F-96500 C mol-1-

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Standard X

Chemistry

Electrolysis and Electrolytes

On the basis ...

Question

On the basis of information available from the reaction
$\frac{4}{3} A l + O_{2} \to \frac{2}{3} A l_{2} O_{3}, Δ G = - 827 k J . m o l^{- 1}$

The minimum emf required to carry out the electrolysis of $A l_{2} O_{3}$ is:
$[F = 96500 C m o l^{- 1}]$

2.14 V

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4.28 V

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- 6.42 V

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8.56 V

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Solution

The correct option is A $2.14 V$
One mole of oxygen requires 4 moles of electrons.

The relationship between emf of cell and free energy change is $Δ G = - n F E_{c e l l} .$

Substitute values in the above expression.

$- 827000 \frac{J}{m o l} = - 4 \times 96500 \times E_{c e l l}$

$E_{c e l l} = 2.14 V .$

Hence, the correct option is $A$

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Similar questions

Q. On the basis of the information available from the reaction:

\frac{4}{3} A l + O_{2} \to \frac{2}{3} A l_{2} O_{3}, Δ G = - 827 k J m o l^{- 1}

O_{2}

, the minimum emf required to carry out the electrolysis of

A l_{2} O_{3}

[F = 96500 C m o l^{- 1}]

Q. On the basis of information available for the reaction:

\frac{4}{3} A l + O_{2} \to \frac{2}{3} A l_{2} O_{3}; △ G = - 827 k J / m o l

O_{2}

the minimum emf required to carry out an electrolysis of

A l_{2} O_{3}

is:
(Given:

1 F = 96500 C)

On the basis of information available from the reaction:
$\frac{4}{3} A l + O_{2} \to \frac{2}{3} A l_{2} O_{3} Δ G = - 827 K J / m o l$ of $O_{2}$ . The minimum e.m.f. required to carry out
electrolysis of $A l_{2} O_{3}$ is

Q. On the basic of information availbale from the relation

\frac{4}{3} A l + O_{2} \to \frac{2}{3} A l_{2} O_{3}, Δ G = - 827 {kJ mol}^{- 1}

O_{2}

, the minimum emf required to carry out electrolysis of

A l_{2} O_{3}

is:

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On the basis of information available from the reaction43Al+O2→23Al2O3,ΔG=−827 kJ.mol−1The minimum emf required to carry out the electrolysis of Al2O3 is:[F=96500 C mol−1]

The correct option is A 2.14 VOne mole of oxygen requires 4 moles of electrons.The relationship between emf of cell and free energy change is ΔG=−nFEcell.Substitute values in the above expression.−827000 Jmol=−4× 96500×Ecell Ecell=2.14 V.Hence, the correct option is A

On the basis of information available from the reaction
$\frac{4}{3} A l + O_{2} \to \frac{2}{3} A l_{2} O_{3}, Δ G = - 827 k J . m o l^{- 1}$

The minimum emf required to carry out the electrolysis of $A l_{2} O_{3}$ is:
$[F = 96500 C m o l^{- 1}]$