100cc of propane is ignited along with 100cc of oxygen under constant pressure and

temperature. Then which of the following statements are correct?

$\underset{\text{1\hspace{0.17em}mole}}{{\text{C}}_{\text{3}}{\text{H}}_{\text{8}}}\text{\hspace{0.17em}+\hspace{0.17em}}\underset{\text{5\hspace{0.17em}mole}}{{\text{5O}}_{\text{2}}}\to \underset{\text{3\hspace{0.17em}moles}}{{\text{3CO}}_{\text{2}}}{\text{\hspace{0.17em}+\hspace{0.17em}4H}}_{\text{2}}\text{O}$

100 cc propane requires 500 cc  ${\text{O}}_{\text{2}}$ for combustion But available oxygen is  only 100cc. Hence ${\text{O}}_{\text{2}}$is limiting reagent

100 cc oxygen is sufficient for the combustion of only 20 cc of propane. So, 80 cc propane is left over without combustion.  ${\text{CO}}_2$ formed is 60 cc. Oxygen is completed consumed.