00:01
Okay, this is chapter 11, section problem 84.
00:05
The question is, the vapor pressure of ccl3f at 300k is 856 tor.
00:13
If 11 .5 grams of ccl3f is enclosed in a one liter container, is any liquid present? if so, was the mass of the liquid.
00:24
So when i did this first, i thought, okay, well, what if this were all? gas, if all 11 .5 grams of the ccl 3f were a gas, what would the pressure there be? so to do this, i utilize the ideal gas law.
00:42
So pv is equal to energy.
00:44
If you rearrange that to get the pressure, pressure is going to be equal to moles times the gas constant time temperature divided by the volume.
00:52
And if i plugged all that in, so first i converted the grams to moles and then multiplied by the gas constant, which leaving it in tours per, liters per mole kelvin is 62 .364, multiplied by the temperature, divided by the volume.
01:14
I got 1566 .6 .4 tor.
01:18
And that is more than the pressure by the vapor pressure.
01:23
So clearly some of this is going to be left over as a liquid.
01:26
So we could have just started with this calculation down here.
01:33
So to calculate how many moles of gas is actually able to be formed, we just rearrange the ideal gas a little bit differently.
01:40
So to calculate the number of moles possible, just rearranges...