00:01
Hello, so today we're going to be looking at a day where it's a sunny day and it's 20 degrees celsius, and the pressure is 748 millimeters of mercury, and we have 0 .42 parts per million by volume of ozone.
00:18
So we want to find out how much ozone, how many molecules of ozone we have, and what the partial pressure is.
00:35
So, well, what are we given? when given the temperature, the pressure, and we want to find it in one liter of volume, so we know the volume.
00:45
And we know this concentration.
00:48
So we should probably use the ideal gas law.
00:58
If we just plug in the way that what we know about ozone right now, we don't really know the partial pressure or the moles, so we would kind of get stuck.
01:12
But we know the overall temperature, the overall pressure, and the overall volume.
01:19
So we can solve for the total moles of gas in one liter.
01:26
And since the ideal gas law, the equal amounts of moles will occupy the same volume, we can find out how many moles of ozone we have.
01:40
So let's convert.
01:43
This to atmospheres so 748 millimeters of mercury divided by 760 which is in one atmosphere we have one liter trying to solve for the moles and you have 0 .082 .06 and the temperature is 20 degrees celsius we needed in kelvin.
02:19
So add 273, so that would be 293...