Question

A sample of argon gas has a mass of 0.20 g, at , a pressure of 100 000 Pa and a temperature of 12 °C. Which volume does the gas occupy? A 1.2 x 104 cm3 B 5.0 cm 3 C 59 cm 3 D 119 cm 3


The answer is D why​

Answer 1

This problem is providing the mass of argon as 0.20 g, its pressure as 100,000 Pa and temperature as 12 °C so the volume it occupies is required and found to be D. 119 cm³  according to:

Ideal gas law

In chemistry, we use gas laws in order to comprehend the volume-temperature-mole-pressure behavior of gases. In this case, we refer to the ideal gas law as all of the aforementioned variables are taken into account:

$PV=nRT$

Thus, solving for the volume as required:

$V=\frac{nRT}{P}$

However, we should set the pressure in atmospheres, temperature in kelvins and convert the mass to moles as shown below:

$V=\frac{(0.20g*\frac{1mol}{40.0g})(0.08206\frac{atm*L}{mol*K})(12+273)K}{100000Pa*\frac{1atm}{101325Pa} }$

Then, we calculate the result in liters and then convert it to cubic centimeters:

$V=0.119L*\frac{1000cm^3}{1L} \\\\V=119cm^3$

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