# Math Help - Number of Moles

1. ## Number of Moles

Given: $2KClO_{3}(s) + heat \to 2KCl(s) + 3O_{2}$

How many moles of $O_2$ form as 3.0 mol of $KClO_{3}$ are totally consumed?

I see that the ratio between $O_2$ and $KClO_{3}$ is 3 : 2.

So since $KClO_{3}$ is 3.0 mol, then I figured $O_2$ must be $\boxed{4.5\,moles}$

Is this correct?

2. $\text{3.0 mol } KClO_{3} \times \frac{\text{3 mol } O_{2}}{\text{2 mol } KClO_{3} } = \text{4.5 mol } O_{2}$

Looks good to me.