The plot shows the variation of −$$ln$$ K_p versus temperature for the two reactions.

M(s) + $${1 \over 2}$$ O₂(g) $$ \to $$ MO(s) and

C(s) + $${1 \over 2}$$ O₂(g) $$ \to $$ CO(s)


Identify the correct statement :

The heats of combustion of carbon and carbon monoxide are –393.5 and –283.5 kJ mol^–1, respectively. The heat of formation (in kJ) of carbon monoxide per mole is :

The following reaction is performed at 298 K
2NO(g) + O₂ (g) $$\leftrightharpoons$$ 2NO₂ (g)
The standard free energy of formation of NO(g) is 86.6 kJ/mol at 298 K. What is the standard free energy of formation of NO₂(g) at 298 K? (KP = 1.6 × 10¹²)

For complete combustion of ethanol, C₂H₅OH(l) + 3O₂(g) $$\to$$ 2CO₂(g) + 3H₂O(l) the amount of heat produced as measured in bomb calorimeter, is 1364.47 kJ mol^–1 at 25^oC. Assuming ideality the Enthalpy of combustion, $$\Delta _CH$$, for the reaction will be : (R = 8.314 kJ mol^–1)