At 0° the density of oxygen at 1 atm is 1.43 g/L. The oxygen which occupied 1.5 L at STP was compressed at 0°C to 600 atm, and the volume was observed to be 4 cc, in violation of Boyle’s law. What was the final density of oxygen?

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536 g/L

857 g/L

8.57g/L

53.6 g/L

answer is A.

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Detailed Solution

Given,
density, d = 1.43 g /L
Volume, ν= 15L
Volume,v2 = 4cc
d2 = ?
Density as the gas behaves non-ideally,

$\begin{array}{l} F i n a l d e n s i t y (d) = \frac{Initial Mass}{Final Volume} \\ \Rightarrow d = \frac{1.43 \times 1.5}{0.004} \\ \Rightarrow d = 536 g/L \end{array}$

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