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And all I did is I wrote this third equation, but I wrote it in reverse order. The good thing about this is I now have something that at least ends up with what we eventually want to end up with. What are we left with in the reaction? Isn't Hess's Law to subtract the Enthalpy of the left from that of the right? So they tell us, suppose you want to know the enthalpy change-- so the change in total energy-- for the formation of methane, CH4, from solid carbon as a graphite-- that's right there-- and hydrogen gas. Now, this reaction right here, it requires one molecule of molecular oxygen. Calculate delta h for the reaction 2al + 3cl2 3. And let's see now what's going to happen. How do you know what reactant to use if there are multiple?
You can only use the (products - reactants) formula when you're dealing exclusively with enthalpies of formation. And then you put a 2 over here. Let me just rewrite them over here, and I will-- let me use some colors. I'll just rewrite it. So two oxygens-- and that's in its gaseous state-- plus a gaseous methane. You do basically the same thing: multiply the equations to try to cancel out compounds from both sides until youre left with both products on the right side. For example, CO is formed by the combustion of C in a limited amount of oxygen. And it is reasonably exothermic. So it's positive 890. Nowhere near as exothermic as these combustion reactions right here, but it is going to release energy. Calculate delta h for the reaction 2al + 3cl2 is a. All we have left on the product side is the graphite, the solid graphite, plus the molecular hydrogen, plus the gaseous hydrogen-- do it in that color-- plus two hydrogen gas. Actually, I could cut and paste it. So let me just copy and paste this. From the given data look for the equation which encompasses all reactants and products, then apply the formula.
You use the molar enthalpies of the products and reactions with the number of molecules in the balanced equation to find the change in enthalpy of the reaction. So this is the fun part. And when we look at all these equations over here we have the combustion of methane. But the reaction always gives a mixture of CO and CO₂.
But our change in enthalpy here, our change in enthalpy of this reaction right here, that's reaction one. How do we get methane-- how much energy is absorbed or released when methane is formed from the reaction of-- solid carbon as graphite and hydrogen gas? Created by Sal Khan. Calculate delta h for the reaction 2al + 3cl2 2. So this produces carbon dioxide, but then this mole, or this molecule of carbon dioxide, is then used up in this last reaction.
It will produce carbon-- that's a different shade of green-- it will produce carbon dioxide in its gaseous form. And this reaction right here gives us our water, the combustion of hydrogen. Consider the reaction 2Al (g) + 3Cl(2) (g) rArr 2Al Cl(3) (g). The approximate volume of chlorine that would react with 324 g of aluminium at STP is. So those are the reactants. Those were both combustion reactions, which are, as we know, very exothermic. CH4 in a gaseous state. This reaction produces it, this reaction uses it. And if you're doing twice as much of it, because we multiplied by 2, the delta H now, the change enthalpy of the reaction, is now going to be twice this.
That's what you were thinking of- subtracting the change of the products from the change of the reactants. Let me do it in the same color so it's in the screen. Here, you have reaction enthalpies, not enthalpies of formation, so cannot apply the formula. Now, let's see if the combination, if the sum of these reactions, actually is this reaction up here. And we have the endothermic step, the reverse of that last combustion reaction. But if we just put this in the reverse direction, if you go in this direction you're going to get two waters-- or two oxygens, I should say-- I'll do that in this pink color. What happens if you don't have the enthalpies of Equations 1-3? This is our change in enthalpy. And now this reaction down here-- I want to do that same color-- these two molecules of water.
About Grow your Grades. So this produces it, this uses it. Now, before I just write this number down, let's think about whether we have everything we need. So we could say that and that we cancel out.
So it is true that the sum of these reactions is exactly what we want. So if this happens, we'll get our carbon dioxide.