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The standard free energy of formation of $M g O$ and $C O$ at temperature $1000 ° C$ and $2000 ° C$ are given below (they refer to the reaction involving one mole of oxygen at one atmosphere pressure). The free energy change to the reaction.
$2 M g + O_{2} \to 2 M g O △ G_{1000^{\circ} C =} - 941 k J / m o l △ G_{2000^{\circ} C =} - 341 k J / m o l 2 C + O_{2} \to 2 C O △ G_{1000^{\circ} C =} - 439 k J / m o l △ G_{2000^{\circ} C =} - 628 k J / m o l$
The following reaction is feasible at :
$2 M g O + 2 C \to 2 M g + C O$

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At $1000 ° C$ temperature

At $2000 ° C$ temperature

Both (1) and (2)

None of these

answer is B.

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Detailed Solution

At $1000 ° C$

$2 M g + O_{2} \to 2 M g O △ G_{1000^{\circ} C =} - 941 k J / m o l 2 C + O_{2} \to 2 C O △ G_{1000^{\circ} C =} - 439 k J / m o l$

$2 M g O + 2 C \to 2 M g + C O △ G$ is $+ v e$ so reaction is nonspontaneous

At $2000 ° C$

$2 M g + O_{2} \to 2 M g O △ G_{2000^{\circ} C =} - 341 k J / m o l 2 C + O_{2} \to 2 C O △ G_{2000^{\circ} C =} - 628 k J / m o l$

$2 M g O + 2 C \to 2 M g + C O △ G$ is $- v e$ so reaction is spontaneous

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