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

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

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The entropy of a metal is higher in its liquid state than in its solid state. Therefore, entropy change, `DeltaS` of the formed is in liquid state and metal oxide being reduced is in the solid state. Since the value of `T DeltaS` increases and that of `DeltaH` remains constant, therefore , the value of `DeltaG` becomes more on negative side and therefore, reaction becomes easier.
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Why is the reductio of a meal oxide easier if the metal foremd is in liquid state in the temoerature of reduction?

Statement-1: The reduction of a metal oxide is easier if the metal formed is in liquid state at he temperature of reduction. Statement-2: The value of entropy change DeltaS of the reduction process is more on +ve side when the metal formed is in liquid state and the metal oxide being reduced in a solid state. Thus, the value of the DeltaG becomes more or negative side.