Question

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

Answer 1

In the liquid state, the entropy of the system is higher than that in the solid state. The value of AG° becomes more negative, (i.e. $\Delta $G = $\Delta $H — T$\Delta $S) and the reduction becomes more spontaneous

Answer 2

Answer:

the temperature of the substance in liquid state in higher.

Explanation:

the Ellington diagram suggests that the value of angle G for the formation of metal oxide increases as the temperature increases. the reduction of metal oxide to metal is possible if the gibbs energy is negative.

therefore the reduction of metal oxide to metal is easier if the metal obtained in liquid state

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