For the reaction A + B $\to$ C + D,$\Delta$H° = +40 kJ and $\Delta$S° = +50 J/K.Therefore,the reaction under standard conditions is

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The spontaneity of a reaction can be determined using the Gibbs free energy change ($\Delta G^\circ$), which is calculated using the equation $\Delta G^\circ = \Delta H^\circ - T\Delta S^\circ$. For the reaction to be spontaneous, $\Delta G^\circ$ must be negative. Given $\Delta H^\circ = +40 kJ = +40000 J$ (since 1 kJ = 1000 J) and $\Delta S^\circ = +50 J/K$, the sign of $\Delta G^\circ$ depends on the temperature ($T$). Substituting the given values into the equation, we get $\Delta G^\circ = +40000 J - T(50 J/K)$. For $\Delta G^\circ$ to be negative, and thus the reaction to be spontaneous, the temperature must satisfy $T > 800 K$. This is because when $T = 800 K$, $\Delta G^\circ = 0$, and for $T > 800 K$, $\Delta G^\circ$ becomes negative.

For the Reaction a + B →\to→ C + D Δ\DeltaΔ H° = +40 KJ And

For the Reaction a + B $\to$ C + D $\Delta$ H° = +40 KJ And