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Gibbs energy of formation triangleG(f)^(...

Gibbs energy of formation `triangleG_(f)^(G)` of MgO (s) and CO (g) at 1273 K and 2273 K are given below :
`triangleG_f [MgO (s)]= -941"kJ mol"^(-1)" at 1273 K"`
`triangleG_f [CO (g)]=-439"kJ mol"^(-1)" at 1273 K"`
`triangleG_f [MgO (s)] =-314"kJ mol"^(-1)" at 2273 K"`
`triangleG_f [CO (g)] =-628"kJ mol"^(-1)" at 2273 K"`
On the basis of above data, predict the temperature at which carbon can be used as a reducing agent for MgO (s).

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To determine the temperature at which carbon can be used as a reducing agent for MgO (s), we will analyze the Gibbs energy of formation values provided at two different temperatures. The process is spontaneous when the Gibbs free energy change (ΔG) is negative. ### Step-by-Step Solution: 1. **Identify the Gibbs Energies at 1273 K:** - ΔG_f [MgO (s)] = -941 kJ/mol - ΔG_f [CO (g)] = -439 kJ/mol ...
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