Question

wally fluoride is an imaginary gaseous
compound with a molar mass of 314.2 g/mol.
(a) What is the density of wollmanium fluoride at 425 K
and 165 torr?

Answer 1

Answer:

$\rho =1.96\frac{g}{L}$

Explanation:

Hello there!

In this case, since this imaginary gas can be modelled as an ideal gas, we can write:

$PV=nRT$

Which can be written in terms of density and molar mass as shown below:

$\frac{P}{RT} =\frac{n}{V} \\\\\frac{P}{RT} =\frac{m}{MM*V}\\\\\frac{P*MM}{RT} =\frac{m}{V}=\rho$

Thus, by computing the pressure in atmospheres, the resulting density would be:

$\rho = \frac{165/760 atm * 314.2 g/mol}{0.08206\frac{atm*L}{mol*K}*425K} \\\\\rho =1.96\frac{g}{L}$

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