In order to balance it, we're going to have six oxygens on the reactant side. On this side we have one, two, three, four, five, six oxygens. So O H, and actually let me write this right over here, so Of these water molecules? So, let's draw another Say, "okay, we have four hydrogens here, "we only have two here." Well, what if we had two So now we've balanced the carbons, two carbons on the reactant side. We're just going to have another molecule. Or if you want to do it, if you want to have it more visual, you could write it, okay, we're just going to The actual structure here, so let's write the two out front. We're definitely producing carbon dioxide, but how many carbon dioxides do we produce for each molecule of ethylene? And so that's where we say, "Okay, we have two carbons here, "we want two carbons here." We don't want to change We don't want to do, we want to say, we're definitely You would be changing what this molecule is. Somehow write a subscript of two right over there, you would somehow be changing the structure, Your water right over here, this is an oxygen bonded to two hydrogens. Finally, water, actually I'm going to do this in a slightly different color. Carbon dioxide is a carbon, double bonded, to two oxygens each. Notice you have twoĬarbons and four hydrogens. Then each carbon isīonded to two hydrogens. It a little bit differently, let's draw each of these molecules So ethylene looks like this. And that's why we do notĬhange these subscripts. You can't change the number of constituents within the molecule. So the only thing that you can change when you're changing these is the number of molecules. When it's unbalanced, it just doesn't have the numbers right in terms of number of molecules. When you're balancing chemical reactions, the reaction itself is, even before it's balanced is describing something that happens. You're actually changing the reaction when you're doing that. It's no longer carbon dioxide, it's now this bizarre thing that doesn't really exist in nature. " And the reason why you can't do that is that's actually changing the molecule. Subscript little twos look, "so why not put a two right over there. Might have been thinking, "Why put this big two out front "of the entire carbon dioxide, "I like the way these little Is let's just put a two out front here and so now we have two for every molecule of ethylene and we're not done balancing And right now, I only have oneĬarbon on the product side. And so I would want twoĬarbons on the product side. And we've seen that, okay, if let's say, we're trying to balance thisĮquation right over here and we started with the carbons. We've now seen a couple of examples of balancingĬhemical equations.
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