The Ellingham diagram for zinc,magnesium,and | vedclass

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(B) In an Ellingham diagram,a metal oxide can be reduced by a reducing agent if the $\Delta G^\circ$ line of the reducing agent lies below the $\Delta

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$> 1100 \, ^\circ C$

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(B) In an Ellingham diagram,a metal oxide can be reduced by a reducing agent if the $\Delta G^\circ$ line of the reducing agent lies below the $\Delta G^\circ$ line of the metal oxide at a given temperature.The reduction reaction is $ZnO + C 	o Zn + CO$.From the provided Ellingham diagram,the line for the oxidation of carbon $(2C + O_2 	o 2CO)$ intersects the line for the oxidation of zinc $(2Zn + O_2 	o 2ZnO)$ at approximately $1000 \, ^\circ C$.For temperatures above $1000 \, ^\circ C$,the $\Delta G^\circ$ line for the formation of $CO$ lies below the $\Delta G^\circ$ line for the formation of $ZnO$. Therefore,carbon can act as a reducing agent for $ZnO$ only at temperatures greater than $1000 \, ^\circ C$.

The Ellingham diagram for zinc,magnesium,and carbon converting into corresponding oxides is shown below. To make the following reduction process spontaneous,the temperature should be:
$ZnO + C \to Zn + CO$

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The Ellingham diagram for zinc,magnesium,and carbon converting into corresponding oxides is shown below. To make the following reduction process spontaneous,the temperature should be:$ZnO + C \to Zn + CO$