2nd law of thermodynamics Cell potential equation charging a battery vs using a battery 2nd law with entropy

G = negative = k>1 G = positive = k<1 k is close to 1, G is close to zero k is far from 1, G is far from zero delta G and the energy of the product is lower than that of the reactants 1. G = negative = k>1; G = positive = k as temperature goes to zero, entropy approaches a constant value thermodynamically unfavorable

entropy of an isolated system is never decreasing, only if it is in a 2 or more system T=100k spontaneous, low temperature, T delta S is small as matter disperses, entropy increase, so, going from solid to liquid to gas would increase entropy, whilst going from gas to liquid to solid would decrease it y + z --> Y+ + Z- (G<0)

voltage equation G, S, H 2nd law of thermodynamics cell potential, Ecell, electromotive force (emf)

2nd law with entropy galvanic cell vs electrolytic cell if a reaction is thermodynamically favorable is H > 0 and S > 0