We must measure the change in energy or change in heat. H is the measurement of how much energy it contains within it. So delta S is the measure of randomness or chaos or movement, as in the particles or compounds. So it's going from a high disorder to a low disorder. It's actually just saying my delta S is decreasing in value. My delta S is going from high to low, it's going to be negative. So my delta S and then with a numerical value of it. So over here, the products it's all solids. So you have a high amount of disorder over here. So we have, this is a solid state, this is a gaseous state, this is a solid state. How much disorder or chaos is actually happening within the system. So iron and oxygen were high in energy, then it released the energy when it became rust or Fe2O3.ĭelta S, we have to look at the states of matter. So it does require energy or releases energy when this reaction occurs. But this, it does have a delta H and I'm going to say this is the reaction. Formation reactions you're only allowed to have one mole of a product. So this actually is a formation reaction, well not really, because it doesn't have one mole. Iron and oxygen combine together to make rust. What about a process? Well process we use half delta H's. They do have some sort of amount of energy and movement within it. Every substance has measurement of disorder or chaos and movement. So there is no delta H but there is an S, and S is measuring the movement, or the disorder or the chaos in this oxygen has. However oxygen isn't made, therefore it doesn't have the energy, it doesn't need energy to create because it is naturally created.
They are constant moving, so they do have mass measurement. They can turn this way, if they want to turn this way. They can squeeze together, they can stretch apart. So oxygen can be together, it can be stretched apart, these bonds are mobile. So it moves in space, so S is the movement, measurement of randomness, disorder, movement. O2 looks like this double-bonded, it's a lot of electrons around it, that's too many. What about delta S? What the heck is that? But since we don't make elements, the delta H for elements is zero. So it's not actually what is in the heat that it actually contains just as compound, it's actually how the compound is made, how much energy it takes to make that compound. For elements it's always zero, even the o2 or the diatomics. It actually is a process going from its elements reforming that. For compounds, when we're talking of the delta H, it's a formation of that. So if we have an element, elements have a delta H of zero, always. So we're going to have elements and compounds. S is the measurement of this disorder and randomness and movement, within a particle or a process. We can however measure S, and this is how we do it. We don't have the means of measuring that. You cannot have this H by itself, we can't measure it. We can only measure the change it undergoes through a chemical process. We cannot decipher how much heat or energy something has in it. Well H is the measurement of heat or energy, but it's a measurement of the transfer of heat or energy. We can however talk about just straight up H and S, let's do that. That's because we typically talk about changes, reactions or processes that actually happen in Chemistry. It's a measurement of randomness or disorder. Now I'm just giving very simplified definitions, but you should have these in your heads.ĭelta S is entropy.
This measurement of heat or energy transfer. And the reason I made my H capitalised, is because that's how I remember that delta H is enthalpy. Let's decide what delta H and delta S are.
DELTA H AND DELTA S FOR O2 WEBOOK FREE
Thus although the free energy always falls when a gas expands or a chemical reaction takes place spontaneously, there need be no compensating increase in energy anywhere else.Tips on understanding the difference between delta H and delta S. Free Energy is not energy: A much more serious difficulty with the Gibbs function, particularly in the context of chemistry, is that although G has the units of energy (joules, or in its intensive form, J mol –1), it lacks one of the most important attributes of energy in that it is not conserved.This is most commonly in the form of electrical work (moving electric charge through a potential difference), but other forms of work (osmotic work, increase in surface area) are also possible.
By "useful", we mean work other than that which is associated with the expansion of the system. The “free” part of the older name reflects the steam-engine origins of thermodynamics with its interest in converting heat into work: ΔG is the maximum amount of energy which can be “freed” from the system to perform useful work.
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