![]() ![]() So, we're going to haveĪ release of energy here, but our entropy decreases. So, over here, if we are dealing, our Delta H is less than zero. Now, over here, we have some permutations of Delta H's and Delta S's, and whether they're spontaneousĭepends on the temperature. Some intuitive sense that this is not going to be spontaneous. This is a combination, if Delta H is greater than zero, and if this is less than zero, than this entire term We would require some energy, and the disorder is going to go down. That get close to each other, but their electrons say, "Hey, no, no." In order for us to bond, we would have to get toĪ higher energy state. So, that's, you know, youĬan imagine these two atoms, or maybe these molecules Reaction needs to increase, and your entropy is going to decrease. Now, what about this one down here? This one down here, Delta So, this one over here, I'm gonna make all the spontaneous ones, I'm gonna square them Delta G is, not just Delta, Delta G is less than zero. That this is a natural thing that would actually occur. And, when they get close to each other, their electrons may be, say hey, "Wait, there's a better configuration here "where we can go into lower energy states, "where we can release energy "and in doing so, "these differentĬonstituents can part ways." And so, you actually Happen spontaneously, regardless of what the temperature is. This makes a lot of sense that this is going to Disorder increases the number of states that my system can take on increases. ![]() And, you could think about this as, so let's see, we're gonna release energy. So, this means we're going to release, we're going to release energy here. Is less than zero, and our entropy increases, our enthalpy decreases. So, in this scenario over here, if our change in enthalpy If this expression over here is negative, our reaction is going to be spontaneous. ![]() Now, let's think a little bitĪbout why that makes sense. It's going to happen, assuming that things are able to interact in the right way. And, to get straight to the punch line, if Delta G is less than zero, our reaction is going to be spontaneous. Use change in Gibbs Free Energy to predict whether a reaction is going to spontaneously happen, whether it's going to be spontaneous. Gonna think about it in the context of how we can Josiah Willard Gibbs, he defined this to think about, well, how much enthalpy is going to be useful for actually doing work? How much is free to do useful things? But, in this video, we're But, as we'll see, it makesĪ lot of intuitive sense. So, 'S' is entropy and it seems like this bizarre formula that's So, that's a change in enthaply minus temperature times change in entropy, change in entropy. So, this is a change in enthalpy which you could view as heat content, especially because this formula applies if we're dealing with constant And, it says that theĬhange in Gibbs Free Energy is equal to the change, and See this famous formula which is going to help To be spontaneous or not, which is super useful inĬhemistry and biology. Usefulness in determining whether a reaction is going To explore Gibbs Free Energy a little bit in this video. ![]()
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