00:01
For part a of this problem, let's remember that the mac of chloroform is 77%, and 77 % is the exact same thing, is saying .77.
00:12
So if we want to find the partial pressure that we need, we'll have that pressure, which we denote by the letter p, is equivalent to 760 multiplied by 0 .77 over 100, and we'll find that the partial pressure we need is 5 .852 millimeters of mercury.
00:35
Now for part b, we have to take note of a couple things before we can do a calculation.
00:42
Let's know that the pressure of chloroform, pardon me, will be equivalent to 5 .852 atm over 760.
00:54
Let's know that the volume of air is equivalent to 10 liters.
00:59
We will use this later on in the calculation.
01:02
And all that this is saying is that we'll simply take 5 .852 and divided by 760 to get our pressure in atm.
01:14
Because remember, previously we had our units in millimeters of mercury.
01:19
When we do that calculation, we'll get that our performance.
01:24
Pressure essentially is 7 .7 times 10 to the negative third.
01:30
And now what we can do is we can say, well, this value we just calculated is equivalent to the moles of chloroform divided by simply the total moles of our reaction.
01:44
And that allows us to rearrange this to say the moles of chloroform is roughly equal to 7 .7 times 10 to the negative third multiplied by our total moles...