A reaction has Delta H deg = +30.0 kJ mol^-1 and Delta S deg = +100 J K^-1mol^-1, both independent of temperature. Select the correct statement(s).

At 250 K, Delta G deg = +5.0 kJ mol^-1

The reaction is spontaneous under standard conditions at all temperatures below 300 K

JEE Advanced levelOne or more correct optionsDifficulty 3 of 3td105

A reaction has $Δ H^{\circ} = + 30.0 kJ mo l^{- 1}$ and $Δ S^{\circ} = + 100 J K^{- 1} mo l^{- 1}$ , both independent of temperature. Select the correct statement(s).

AAt $300 K$ , $K = 1$
BAt $400 K$ , $K > 1$
CAt $250 K$ , $Δ G^{\circ} = + 5.0 kJ mo l^{- 1}$
DThe reaction is spontaneous under standard conditions at all temperatures below $300 K$

Δ G^{\circ} = 30000 - 100 T

J. At

250 K

30000 - 25000 = + 5000 J

. At

400 K

- 10000 J

, so

K > 1

. At

300 K

Δ G^{\circ} = 0

, so

K = 1

. Below

300 K

Δ G^{\circ} > 0

, so the reaction is non-spontaneous there; the statement claiming spontaneity at all temperatures below

300 K

is false.