Spontaneity of Reaction at 300 K

Hard General Chemistry Thermodynamics And Thermochemistry

Consider a chemical reaction at equilibrium represented by the equation:

A(g) + B(g) <=> C(g) + D(g)

At a certain temperature, the enthalpy change (ΔH) for the reaction is +50 kJ/mol, and the entropy change (ΔS) is +150 J/(mol·K). Which of the following statements is true regarding the spontaneity of this reaction at a temperature of 300 K?

The reaction is spontaneous at 300 K because ΔG < 0.

The reaction is non-spontaneous at 300 K because ΔG > 0.

The reaction is at equilibrium at 300 K, so ΔG = 0.

The reaction is spontaneous at 300 K only under high-pressure conditions.

Hint

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