The gibbs free energy of formation of MO and CO at temperature 1000 ∘C and 1900 ∘C are given.2M+O2→2MO ;ΔG1900 ∘C=−300 kJ/mol ΔG1000 ∘C=−921 kJ/mol2C+O2→2CO ;ΔG1900 ∘C=−624 kJ/mol ΔG1000 ∘C=−423 kJ/molMO+CΔ→M+CO↑The reaction is feasible at temperature x∘C then what is the value of x500:

The gibbs free energy of formation of MO and CO at temperature 1000 �

1.	The gibbs free energy of formation of MO and CO at temperature 1000 ∘C and 1900 ∘C are given.2M+O2→2MO ;ΔG1900 ∘C=−300 kJ/mol ΔG1000 ∘C=−921 kJ/mol2C+O2→2CO ;ΔG1900 ∘C=−624 kJ/mol ΔG1000 ∘C=−423 kJ/molMO+CΔ→M+CO↑The reaction is feasible at temperature x∘C then what is the value of x500:
Answer» The gibbs free energy of formation of $M O$ and $C O$ at temperature $1000^{\circ} C$ and $1900^{\circ} C$ are given. $2 M + O_{2} \to 2 M O; Δ G_{1900^{\circ} C} = - 300 kJ/mol$ $Δ G_{1000^{\circ} C} = - 921 kJ/mol$ $2 C + O_{2} \to 2 C O; Δ G_{1900^{\circ} C} = - 624 kJ/mol$ $Δ G_{1000^{\circ} C} = - 423 kJ/mol$ $M O + C Δ \to M + C O ↑$ The reaction is feasible at temperature $x^{\circ} C$ then what is the value of $\frac{x}{500}$ :