Delta G= Delta H- T Delta S, when phase separation occur, Gibbs free energy will be lower, then Delta G is negative. In this case, What are the changes of enthalpy and entropy, both lower? And which one should have larger change so that the gibbs free energy decreases?
Delta G= Delta H- T Delta S, when phase separation occur, Gibbs free energy will be lower, then Delta G is negative. In this case, What are the changes of enthalpy and entropy, both lower? And which one should have larger change so that the gibbs free energy decreases?
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But if the phase separation should have a decreased entropy, then there should be a very significant enthalpy drop to keep the energy negative.But isn't it a contradiction? Because the drops in entropy drives the fall in G more strongly. And this should be a spontaneous reaction which the temperature is low, considering the temperature of most living cells is around 310K. shouldn't the change of enthalpy should be more significant? And it is exothermic, will this thermal energy become the energy source of this process or it will decrease the rate of process by increasing the temperature?
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