Write and balance the equation for the combustion of C6H14.

When we have a combustion reaction, what that means is that we're adding oxygen.

And for our hydrocarbons, our only products are going to be CO2 and water.

So, I'm going to start by writing the basics of our reaction.

So, we have C6H14 plus 02

yields C02 plus water.

And because this isn't going to start out balanced, I'm leaving some room for

my coefficients as I go through and balance the equation.

Now, I'm going to create a list of my elements so

that I can basically create a tally.

C, H and O of how many carbons, hydrogens, and

oxygens I have on both sides of the equation.

So, on the left side, I see I have 6 carbons, 14 hydrogens, and 2 oxygens.

On the right side, I have 1 carbon, 2 hydrogens and 3 oxygens.

So, now what I need to do is start putting in coefficients and adjusting my

totals until I get all the coefficients I need to have a balanced chemical equation.

So, I'm going to start by putting a six in front of the CO2,

so that I can balance the carbons.

So, that changes from one carbon to six carbons on the right, but

notice that it also changes the number of oxygens.

Now I have 12 plus one, or 13 oxygens on the right side of the equation.

So, now my carbons are balanced, now I'm going to look at the hydrogens, and

in order to balance the hydrogens, I need a 7 on the right side of the equation.

So, now I have 14 hydrogens, and that also changes the number of oxygens, so,

now I have 12 oxygens plus seven, or 19 oxygens.

Now at this point, both my carbons and my hydrogens are balanced.

It's only the oxygens that are, the not balanced.

And when I look at the left side,

what I notice is that I have oxygen all by itself.

So what I'm going to do, is for a moment, I'm going to pretend.