$C{H}_4$ burns in $O_2,$ producing $C{O}_2$ and $H_{2}O(g).$ What volume of carbon dioxide is produced when $1\mathrm{.}22L$ of $C{H}_4$ at $15C$ and $328$kPa reacts with $3\mathrm{.}0g$ of $O_2.$

$PV=RT$

$C{H}_4(g)+2_2{O}_2(g),C{O}_2(g)+,{?}_{2}O(g)$

a$)$ Balance the equation. $[$T$1].$ Determine limiting$/$excess reagent. $($T$3$ marks$)$

b$)$ What volume of $C{O}_2$ will be produced under these conditions? $($T$2$ marks$)$

Please help me do $6$ b and show the steps hoow you solve LR