For CaCO3(s) CaO(s) + CO2(g), take Delta H deg = +178 kJ mol^-1 and Delta S deg = +161 J K^-1mol^-1 (constant), with K_p = P_CO2/(1 bar) and R = 8.314 J mol^-1K^-1. Select the correct statement(s).

At 1200 K the equilibrium pressure of CO2 exceeds 1 bar

Delta G deg(298 K) approx +130 kJ mol^-1

At 1200 K the equilibrium pressure of CO2 exceeds 1 bar

At 1000 K the equilibrium pressure of CO2 is about 1.3 bar

Delta G deg(298 K) approx +130 kJ mol^-1

JEE Advanced levelOne or more correct optionsDifficulty 3 of 3td110

For $CaCO X_{3} (s) CaO (s) + CO X_{2} (g)$ , take $Δ H^{\circ} = + 178 kJ mo l^{- 1}$ and $Δ S^{\circ} = + 161 J K^{- 1} mo l^{- 1}$ (constant), with $K_{p} = P_{CO X_{2}} / (1 bar)$ and $R = 8.314 J mo l^{- 1} K^{- 1}$ . Select the correct statement(s).

Δ G^{\circ} (298) = 178000 - 298 (161) = 130 kJ

K_{p} = 1

when

Δ G^{\circ} = 0

T = 178000/161 = 1106 K

. At

1000 K

Δ G^{\circ} = 17000 J

and

K_{p} = e^{- 2.045} = 0.129 bar

, ten times smaller than the quoted

1.3

. At

1200 K

Δ G^{\circ} = - 15200 J

and

K_{p} = 4.59 > 1