A reaction has Delta H deg = -60.0 kJ mol^-1 and Delta S deg = -150 J mol^-1K^-1, both independent of temperature (R = 8.314 J mol^-1K^-1). Select all correct statements.

The reaction is spontaneous under standard conditions below 400 K

At 500 K, Delta G deg = +15.0 kJ mol^-1

The reaction is spontaneous under standard conditions below 400 K

K increases as the temperature is raised

At 500 K, Delta G deg = +15.0 kJ mol^-1

JEE Advanced levelOne or more correct optionsDifficulty 3 of 3td216

A reaction has $Δ H^{\circ} = - 60.0 kJ mo l^{- 1}$ and $Δ S^{\circ} = - 150 J mo l^{- 1} K^{- 1}$ , both independent of temperature ( $R = 8.314 J mo l^{- 1} K^{- 1}$ ). Select all correct statements.

Δ G^{\circ} = 0

T = Δ H^{\circ} /Δ S^{\circ} = 400 K

; with

Δ S^{\circ} < 0

the reaction is spontaneous below it. At

298 K

Δ G^{\circ} = - 60000 + 298 \times 150 = - 15300 J

and

K = e^{6.175} = 481 < 1 0^{3}

. The reaction is exothermic, so

K

falls as

T

rises. At

500 K

Δ G^{\circ} = - 60000 + 75000 = + 15.0 kJ mo l^{- 1}