A vessel contains 3.2 ~g of dioxygen gas at STP (273.15 K and 1 atm...

A vessel contains

3.2 \mathrm{~g}

of dioxygen gas at STP (273.15

\mathrm{K}

and 1 atm pressure). The gas is now transferred to another vessel at constant temperature, where pressure becomes one third of the original pressure. The volume of new vessel in

\mathrm{L}

is : (Given - molar volume at STP is

22.4 \mathrm{~L}

)

Options

A6.72
B2.24
C22.4
D67.2

Correct answer

A. 6.72

Step-by-step solution

No. of moles of

\mathrm{O}_2=\frac{\text{ Given weight

} \mathrm{O}_2}{\text{ Mol. weight of } \mathrm{O}_2} =\frac{3.2}{32}=0.1

Molar vol. at

\mathrm{STP}=0.1 \times 22.4=2.24 \mathrm{~L} \mathrm{P}_1=1 \mathrm{~atm}, \mathrm{~V}_1=2.24 \mathrm{~L}, \mathrm{P}_2=\frac{1}{3} \mathrm{~atm}, \mathrm{~V}_2=

? According to Boyle's law :

\mathrm{P}_1 \mathrm{~V}_1=\mathrm{P}_2 \mathrm{~V}_2

\begin{aligned} \therefore 1 \times 2.24 & =\frac{1}{3} \times \mathrm{V}_2 \\ \mathrm{~V}_2 & =2.24 \times 3 \\ & =6.72 \mathrm{~L} \end{aligned}

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