00:01
This problem gives us the following equation.
00:03
N -a -h plus h -2 -o goes to n -a -o -h plus h -2.
00:13
And so the first thing we want to do is find the vapor pressure, vp, of h -2o at 35 degrees celsius, and that is equal to 42 .2 millimeters of mercury.
00:28
Now we can find the actual pressure of h2 by taking the pressure, which is given us 758 millimeters of mercury, and subtract the vapor pressure of h2, or of h2o, 42 .2 millimeters of mercury.
00:51
And that gives us the pressure of h2 to be 715 .8 millimeters of mercury, which if we divide by 760 to 760 to, to convert to atmospheres, we get 0 .948 atmospheres.
01:12
And so the next thing we can do is use the ideal gas law and equals pv over rt.
01:26
And we have all of these values...