Question

A 0.133 mol sample of gas in a 525 ml container has a pressure of 312 torr. The temperature of the gas is ________ °c.

Answer 1

`-253.2 ^(\circ)C`

Step-by-step explanation:

First of all, we need to convert the pressure of the gas from torr to Pa. We know that:

1 torr = 133.3 Pa

So, the pressure in Pascals is

`p=(312 torr)(133.3 Pa/torr)=4.16\cdot 10^4 Pa`

Then we also have:

n = 0.133 number of moles of the gas

`V=525 mL=0.525 L=5.25\cdot 10^(-4) m^3` volume of the gas

The ideal gas equation states that

`pV=nRT`

where R is the gas constant and T the absolute temperature. Solving the equation for T, we find

`T=(pV)/(nR)=((4.16\cdot 10^4 Pa)(5.25\cdot 10^(-4) m^3))/((0.133 mol)(8.314 J/mol K))=19.8 K`

In Celsius, it becomes

`T=19.8 K-273=-253.2 ^(\circ)C`