At constant pressure and temperature, which statement is true?Group of answer choicesAll reactions for which ΔS < 0 are spontaneous.All reactions for which K < 1 are spontaneous.All reactions for which ΔG < 0 are spontaneous.All reactions for which ΔH < 0 are spontaneous.
Question
At constant pressure and temperature, which statement is true?Group of answer choicesAll reactions for which ΔS < 0 are spontaneous.All reactions for which K < 1 are spontaneous.All reactions for which ΔG < 0 are spontaneous.All reactions for which ΔH < 0 are spontaneous.
Solution
The statement that is true at constant pressure and temperature is: "All reactions for which ΔG < 0 are spontaneous."
Here's why:
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ΔS < 0: This refers to the change in entropy. If ΔS is less than 0, it means the system is becoming more ordered, which is not necessarily indicative of spontaneity.
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K < 1: This refers to the equilibrium constant. If K is less than 1, it means the reaction favors the reactants, not the products, so the reaction is not necessarily spontaneous.
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ΔG < 0: This refers to the change in Gibbs free energy. If ΔG is less than 0, it means the reaction releases energy, making it spontaneous. This is the correct answer.
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ΔH < 0: This refers to the change in enthalpy. If ΔH is less than 0, it means the reaction is exothermic, or releases heat. While this often correlates with spontaneity, it's not a guarantee, as it doesn't account for entropy.
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