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

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

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Entropy is more positive when the metal is in liquid state as compared with solid state, so `triangleG` becomes more –ve.]
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Why is the reduction of a metal oxide easier if the metal formed is in liquid state at the temperature of reduction?

(a) Suggest a condition under which magnesium could reduce alumina. (b) Although thermodynamically feasible, in practice magnesium metal is not used for the reduction of alumina in the metallurgy of aluminium. Why ? ( c) What is the reduction of a metal oxide easier if the metal formed is in liquid state at the temperature of reduction ? (d) At a site, low grade copper ores oare available and zinc and iron scraps are also available. Which of the two scraps would be more suitable for reducing the leached copper ore and why ?

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.