- #1
luysion
- 35
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Hi, I've recently started studying chemistry and have being going over gibbs free energy.. I understand it is a driving force causing chemical and physical changes but during my course of reading I did have some queries stem to mind.
1) In relation to equilibrium why is it that a reaction occurs such that G is minimum ? I.e. i read that the reason neither the forward nor reverse reaction proceeds to completion during equilibrium is because Gibbs Free Energy is at a minimum. Is this due to no driving force being provided?
2) When gibbs free energy is positive it indicates the forward reaction (e.g. A --> B) is non-spontaneous why does it still occur? I read something about the reaction still proceeds but the pressure of the product does not read 10^5 P i.e. standard pressure?
im really confused on this bit can somone please simplify this
cheers for any help
1) In relation to equilibrium why is it that a reaction occurs such that G is minimum ? I.e. i read that the reason neither the forward nor reverse reaction proceeds to completion during equilibrium is because Gibbs Free Energy is at a minimum. Is this due to no driving force being provided?
2) When gibbs free energy is positive it indicates the forward reaction (e.g. A --> B) is non-spontaneous why does it still occur? I read something about the reaction still proceeds but the pressure of the product does not read 10^5 P i.e. standard pressure?
im really confused on this bit can somone please simplify this
cheers for any help