![]() 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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