I've just been told that ΔG=0 means "equilibrium".
By equilibrium they mean nothing happens? Or is there a reaction that has ΔG=0? If that reaction does exist, what's it?
Is there a reaction that has ΔG=0?
By equilibrium they mean nothing happens? Or is there a reaction that has ΔG=0? If that reaction does exist, what's it?
Is there a reaction that has ΔG=0?
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"At equilibrium" means that the forward and reverse reaction rates are the same (i.e., reactions are going on, but there is no NET increase in the amount of product or reactant made). In the reaction
A ==> B at equilibrium, A is converted to B, but B is converted back to A at the same rate. To say that there is NO reaction going on is false, but to say that there is no NET reaction, that is true.
If there truly is "no reaction" (i.e. no conversion of reactants to products), then delta G will have a very positive value, say +1,000 kJ/mole or something like that. In a spontaneous reaction, delta G is quite negative (more negative than -10 kJ/mole).
A ==> B at equilibrium, A is converted to B, but B is converted back to A at the same rate. To say that there is NO reaction going on is false, but to say that there is no NET reaction, that is true.
If there truly is "no reaction" (i.e. no conversion of reactants to products), then delta G will have a very positive value, say +1,000 kJ/mole or something like that. In a spontaneous reaction, delta G is quite negative (more negative than -10 kJ/mole).