The volume occupied by one mole of an ideal gas at 273 K and $1.01 \times {10^5}{\text{ Pa}}$ is ${\text{22.4 d}}{{\text{m}}^{\text{3}}}$. What volume, in ${\text{d}}{{\text{m}}^{\text{3}}}$, is occupied by 3.20 g ${{\text{O}}_{\text{2}}}{\text{(g)}}$ at 273 K and $1.01 \times {10^5}{\text{ Pa}}$?

A.     2.24

B.     4.48

C.     22.4

D.     71.7

A

One respondent stated that he/she was not sure if memorization of standard pressure in Pa was required for this question. In this question candidates had first to calculate the amount occupied by 3.20 g of ${{\text{O}}_{\text{2}}}{\text{(g)}}$. This was found by dividing 3.20 by $32.00 = 0.100{\text{ mol}}$. Then, the volume in ${\text{d}}{{\text{m}}^{\text{3}}}$ was obtained by simply multiplying 0.100 by 22.4, giving an answer of ${\text{2.24 d}}{{\text{m}}^{\text{3}}}$, meaning A is the correct answer. The conditions of temperature and pressure were the same at 273 K and ${\text{1.01}} \times {\text{1}}{{\text{0}}^{\text{5}}}{\text{ Pa}}$. 49.15% of candidates got the correct answer.