00:01
Hi, so to solve for this we have two questions here.
00:05
The first one we're solving for the molar mass given the density, the temperature, and the pressure.
00:11
So we will use this formula.
00:12
Density is equivalent to the pressure multiplied by the molar mass of the compound over r and then the temperature.
00:18
Rearranging this to solve for m, molar mass will have density multiplied by r, the ideal gas constant temperature in terms of kelvin divided by the pressure in terms of atm.
00:27
Now let's plug in the information that we have.
00:29
We have 8 .51, this is grams per liter, the density of the unknown gas and then r is 0 .0821 liters atm per mole kelvin.
00:42
Now for the temperature, we have 55 degrees celsius.
00:44
We have to convert this to kelvin.
00:46
We'll add to 3 .15.
00:48
Over pressure, we have 88 .6 kilopascal.
00:53
Convert this to atm using this conversion factor 101 .325 kilopascal is equivalent to 1 atm.
01:02
So let's cancel some units here.
01:04
We could cancel liters and we could cancel atm, cancel kilopascal and then we'd cancel kelvin.
01:12
As you can see the remaining units we have grams per mole and that's the unit for molar mass...