00:01
Hi, so we are to solve for the partial pressure of argon and then the total pressure in the flask in terms of atm.
00:08
So we know the mass of the gases in the mixture, we know the volume, and we know the temperature.
00:15
So we will be using the ideal gas equation pv is equivalent to nrt.
00:20
Let's start with the partial pressure of argon.
00:23
We're solving for pressure so we're arranging the equation we'll have n the number of moles are the ideal gas constant t the temperature over the volume so starting with partial pressure of argon the number of moles of argon we're given with the mass so 7 .97 grams of argon convert this to moles by dividing the molar mass of argon from the periodic table that's 39 .95 grams per mole and r is 0 .0821 liters atm per mole kelvin.
00:58
This is ideal gas constant.
01:00
Temperature is 65 degrees celsius.
01:03
Convert this to kelvin, add to 73 .15 and then the volume is 7 .28 liters.
01:11
Now cancel some units, grams of argon, moles, kelvin, liters and then we have atm, sterium winning unit.
01:18
And solving for this, we'll get 0 .7608 atm.
01:30
And let's write our final answer in three significant figures, 0 .7601 atm...