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(a) Could 131 g of xenon gas in a vessel of volume 1.0 dm3 exert a pressure of 20 atm at
Chapter 1, Problem 1.1(a)(choose chapter or problem)
(a) Could 131 g of xenon gas in a vessel of volume \(1.0\ \mathrm{dm}^3\) exert a pressure of 20 atm at \(25^{\circ} \mathrm{C}\) if it behaved as a perfect gas? If not, what pressure would it exert?
(b) What pressure would it exert if it behaved as a van der Waals gas?
Questions & Answers
QUESTION:
(a) Could 131 g of xenon gas in a vessel of volume \(1.0\ \mathrm{dm}^3\) exert a pressure of 20 atm at \(25^{\circ} \mathrm{C}\) if it behaved as a perfect gas? If not, what pressure would it exert?
(b) What pressure would it exert if it behaved as a van der Waals gas?
ANSWER:Step 1 of 3
Given data:
Mass of xenon gas: 131 g
The volume of the vessel: \(1 \mathrm{dm}^{3} / 1 \mathrm{~L}\)
Temperature: \(25^{\circ} \mathrm{C} / 298 \mathrm{~K}\)
Atomic mass of xenon: 131 g/mol
The number of moles of xenon can be calculated as follows:
\(\mathrm{n}=\frac{\mathrm{w}}{\mathrm{M}} (1)\)
Where,
n = number of moles
w = Mass of the gas
M = Molar mass of the gas
By putting the values of w and M in equation 1, we get:
\(\begin{aligned}
\mathrm{n} & =\frac{131 \mathrm{~g}}{131 \mathrm{~g} / \mathrm{mol}} \\
& =1 \mathrm{~mol}
\end{aligned}\)