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 :

A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following :

For the reaction,
A(g) + B(g) $$ \to $$ C(g) + D(g), $$\Delta $$H^o and $$\Delta $$S^o are, respectively, − 29.8 kJ mol⁻¹ and −0.100 kJ K⁻¹ mol⁻¹ at 298 K. The equilibrium constant for the reaction at 298 K is :

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 :