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Why is the reduction of a metal oxide if...

Why is the reduction of a metal oxide if the metal formed is in liquid state at the temperature of reduction?

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The entropy is higher if the metal is in liquid state than when it is in solid state. The value of `Delta `S of the reduction process becomes more positive, as a result the `Delta `G becomes more negative when metal formed is in the molten state than in solid state. Thus reduction becomes easier.
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(A) Reduction of a metal oxide is easier if the metal formed is in liquid state at the temperature of reduction . (R) Delta G^(@) for the net reaction, reduction of metal oxide with the reductant, is more-ve when the metal formed is in molten state

(A) The reduction of metal oxide is easier if the metal is in liquid state at temp of reduction (R) Delta S is -ve and Delta G is + ve

Metal oxide is easily reduced if the metal is in molten state at the temperature of reduction. Explain.

The non – metal which is in solid state at room temperature

A liquid non metal at room temperature :

The metal which is liquid at room temperature

Name a metal which exists in liquid state.

A non-metal which is liquid at room temperature

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Give an example for reduction of metal oxide with carbon.

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