00:05
This question gives us this reaction of s .o2 and o2 reacting to give s .o3.
00:12
And we're told that the flask initially contains 0 .1 atmospheres of s .o .2 and we're asked what the total pressure would be once the limiting reactant is completely consumed.
00:26
So first i want to talk about what the total pressure of this would be.
00:30
So we have three species here.
00:32
So the total pressure, according to dalton's law, would be the partial pressure of s .o .2 plus the partial pressure of o2, plus the partial pressure of s .o .3.
00:45
So at the beginning, say at the start, our total pressure is going to be 0 .1 atmospheres plus 0 .1 atmosphere.
00:59
So 0 .1 from s .02 and point 1 from 0 .2, and then none from s .03 at the beginning.
01:06
Total of 0 .2 atmospheres to start off with.
01:11
Now the limiting reactant is going to be the reactant that's used up the quickest.
01:15
So if i have s .o2, let's say, if i have 0 .1 atmospheres of 2, 2 moles of s .o .2 make 2 moles of s .3.
01:27
So i'll have the same amount of s .o .3...