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If Gibbs free energy is negative, then the process is spontaneous in the forward direction. If the Gibbs free energy is positive, then the process is nonspontaneous in the forward direction and spontaneous in the reverse direction.
When G is negative, the reaction is spontaneous and thermodynamically stable, and if G is positive the reaction is non-spontaneous and thermodynamically unstable. You can calculate this using the equation G = H - TS.
When ΔG is positive, the reaction is non-spontaneous and requires an input of energy to proceed towards the products. When ΔG is negative, the reaction is spontaneous and releases energy as it proceeds towards the products.
Prasanna Padmanabham 4I wrote:When the Gibbs Free Energy is negative it means that the forward reaction is spontaneous while if it is positive, it means that the reverse reaction is spontaneous.
Spontaneous means that it will occur on its own correct?
When the sign is negative, it means that the reaction is spontaneous. That is because the reaction would result in molecules being in their most stable state which would require less energy to maintain the bonds. As a result, the overall energy is negative because energy is being released. The same is for the opposite. When the sign is positive, the reaction is not spontaneous and therefore requires energy.
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