Question

What is the pressure in torr that a 0.44-g sample of carbon dioxide gas will exert at a temperature of 46.2°C when it occupies a volume of 5.00 L?

Answer 1

`31.92`

Explanation:

To solve this problem we will use the ideal gas law equation:

`PV=nRT`

To find pressure we divided both sides by `V`

`(PcancelV)/cancelV=(nRT)/V`

`P=(nRT)/V`

First we need to convert the temperature to K so we add `212`

`46.2°C +212K=258.2K`

Now we also need to find the number of moles first we find the molar mass of `CO_2`, which is 44. We take our `.44` and divided by `44`.

`("gram sample of carbon dioxide")/("molar mass of " CO_2)`

`(.44 " grams")/(44 " Molar mass")=.01 " moles"`

Now we have:

`n=.01`

`R=0.0806` This is the universal gas constant

`T=258.2K`

`V=5.00L`

Let's plug it in:

`P=(.01"moles"(0.0806(Lxxatm)/(molxxK)(258.2K)))/(5.00L)`

`P=.042 " atm"`

To find the torr you multiply:

`.042xx760=31.92`