Question

a sample of an unknown gas with a molar mads of 107.91 is placed in a vessel with a volume of 7.187 ml at a temperature 52.0 C. if the pressure is 7atm how many grams of this gas are present

Answer 1

Step-by-step explanation:

We have the equation
`PV = nRT`, where we will use
`R = 0.0821 (L(atm))/(K(mol))` .

As a result, we will have to convert the volume to liters and the temperature to kelvin...

`7.187`
`mL` =
`0.007187`
`L`

`52.0`
`C` =
`325.15`
`K`

Now we can plug in all the values to our equation (in the first line) to get about,

`(7)(0.007187) = n(0.0821)(325.15)`

`n = 0.001885` moles

To get our answer, we can multiply our moles value by the molar mass..

`(0.001885)107.91 = 0.203410`

So there are
`0.203410` grams of the gas present.