Calculate the volume occupied by $8.8 \,g$ of $CO_{2}$ at $31.1^{\circ} C$ and $1 \,bar$ pressure.
( $R=0.083 \,bar \,L \,K^{-1} \,mol^{-1}$ )

(N/A) Using the ideal gas equation: $pV = nRT = \frac{m}{M}RT$
Rearranging for volume: $V = \frac{mRT}{Mp}$
Given values:
$m = 8.8 \,g$
$M (CO_{2}) = 12 + 2 \times 16 = 44 \,g \,mol^{-1}$
$R = 0.083 \,bar \,L \,K^{-1} \,mol^{-1}$
$T = 31.1 + 273 = 304.1 \,K$
$p = 1 \,bar$
Substituting the values:
$V = \frac{8.8 \times 0.083 \times 304.1}{44 \times 1}$
$V = 0.2 \times 0.083 \times 304.1$
$V = 5.04806 \,L \approx 5.05 \,L$
Thus,the volume occupied is $5.05 \,L$.