How do I do this stoichiometry problem

(Part 1 of 3)

If 5.96 mol of ethane (C2H6) undergo combustion according to the unbalanced equation

C2H6 + O2 −> CO2 + H2O,

how much oxygen is required?
Answer in units of mol.

(Part 2 of 3)

How much CO2 is formed?
Answer in units of mol.

(Part 3 of 3)

How much H2O is formed?
Answer in units of mol.

First, let's balance the equation. You may use the electron balance method, but since it's hard to write this here, I'll just balance it. Here we go:
2C2H6 + 7O2 -> 4CO2 + 6H2O

Let's see the molar proportions:
2 mol ethane react with 7 mol oxygen
5.96 mol -> x mol oxygen
Solve for x: x=5.96*7/2=20.86 mol O2

We do the same with the other two:
2 mol C2H6 -> 4 mol CO2
5.92 mol -> x mol CO2
x=5.92*4/2=11.84 mol CO2

2 mol C2H6 -> 6 mol H2O
5.92 mol -> x mol H2O
x=5.92*6/2=17.76 mol H2O

I didn't explain much but I hope you did understand me :)