In a reaction where ΔH is negative and ΔS is positive, what can be said about ΔG

In a reaction where ΔH is negative and ΔS is positive, what can be said about ΔG?

In a reaction where ΔH is negative and ΔS is positive, what can be said about ΔG?

Step 1: Understand what ΔH means. ΔH (enthalpy change) being negative means the reaction releases heat (exothermic).
Step 2: Understand what ΔS means. ΔS (entropy change) being positive means the disorder of the system increases.
Step 3: Know the formula for ΔG. ΔG (Gibbs free energy change) is calculated using the formula ΔG = ΔH - TΔS, where T is the temperature in Kelvin.
Step 4: Since ΔH is negative, this part of the equation will lower ΔG.
Step 5: Since ΔS is positive, TΔS will be a positive value, but because ΔH is negative, it will still keep ΔG negative.
Step 6: Conclude that with ΔH negative and ΔS positive, ΔG will always be negative at all temperatures, indicating the reaction is spontaneous.

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