Chemical equation maker for word plus#

Each molecule has two oxygen atoms, so I have six oxygens on the left, and I have two times three oxygens on the right, or I have six oxygens. On the left-hand side? I have three molecules of dioxygen. On the right-hand side? I have four aluminum atoms. And now you can verify how many aluminums do we have on each side? Well I have four aluminumĪtoms on the left-hand side, and how many do I have

And then one times two, one times two is two. There is implicitly a one right over here. Let's multiply all of these, all of the number of molecules by two. Is to get rid of this 1.5, to turn it into a whole number, This is the product - aluminum, aluminum, aluminum oxide. Yielding in the reaction - these are the reactants,

Chemical equation maker for word plus#

So I had aluminum plus dioxygen, a molecule of two oxygens, The chemical equation first in the form that it was before. So instead of two aluminum atoms, let me have four aluminum. This is going to be a three, this is going to be a two right over here.

So if we multiplied both sides by two, we're going to do that. Sides by the same number that gets rid of having thisįraction or this decimal here. This makes it very similar to what you did in algebra,Īn algebraic equation. So what can we do? Well, you can imagine that Notion of a half molecule, which is kind of this bizarre notion. But the convention is that we don't like writing '1.5 molecules.' We don't like having this Oxygen atoms on this side and three oxygen atoms on this side. So one thing that you might say is, 'Okay, well how do I go from two to three? 'I could multiply by 1.5.' So I could multiply by 1.5, and if I multiply 1.5 times two, that's going to be three. I now have two aluminums,Īnd so it looks like the aluminums are balanced,Īnd they are indeed balanced. I have one aluminum here, 'well why don't I just double the number 'of aluminums right over here?' I could just write a two in front of it, so now this has two aluminums, so I no longer have one aluminum here. To say, 'Okay, if I've got 'two aluminums here and So how do we do that? Well one thing might be The number of oxygens, this number and that Number should be the same, and we have to balance Of aluminums on both sides, this number and this Just have miraculously an oxygen atom appear out of nowhere.

And then over here in theĪluminum oxide molecule, we have three.

Of aluminums on both sides, and the same thing is And so aluminum just can'tĪppear out of thin air by virtue of some magical reaction. The right-hand side? Well on the right-hand Here on the left-hand side, how many aluminums do we have? Well on the left-hand You might notice that you don't have the same number 'What do I have to balance?' Well if you look carefully, And so you might say, 'Okay, well what's 'the balancing business all about? 'I have a chemical reaction. And the aluminum oxide molecule has two aluminum atoms and three oxygen atoms. The appropriate conditions they will react to form aluminum oxide. So if I take an atom ofĪluminum and I add it to a dioxygen molecule, so a molecule that has two oxygens with it, under Is a chemical equation? Well this is a chemicalĮquation right over here. If we work through this carefully and methodically,Īnd we also appreciate the art of balancing chemical equations, that it's actually not too bad. Equations is one of those concepts in chemistry that