Which of the following conditions will lead to a decrease in Gibbs Free Energy?

Which of the following conditions will lead to a decrease in Gibbs Free Energy?

Step 1: Understand what Gibbs Free Energy (G) is. It helps predict if a reaction will happen spontaneously.
Step 2: Know the formula for Gibbs Free Energy: G = H - TS, where H is enthalpy, T is temperature, and S is entropy.
Step 3: Identify the conditions that affect G. Focus on enthalpy (ΔH), temperature (T), and entropy (ΔS).
Step 4: Recognize that for an exothermic reaction, ΔH is negative (ΔH < 0). This means the reaction releases heat.
Step 5: Realize that increasing temperature (T) can affect the TS term in the equation. If T increases, TS increases.
Step 6: Understand that if ΔH is negative and T increases, the negative TS term can outweigh the negative ΔH, leading to a decrease in G.
Step 7: Conclude that increasing temperature for an exothermic reaction can make the reaction more spontaneous by decreasing Gibbs Free Energy.

No concepts available.