A sample of hydrogen gas was collected over water at 21 degrees C and 685 mm Hg. The Volume of the container was 7.80 L. Calculate the mass of H2(g) collected.
(Vapor pressure of water at 21 degreesC is 18.6 mm Hg)
Can anyone please verify that the answer is n=PV/RT where.......
P = (685-18.9)/760 = .877 atm
V = 7.80 L
R = .0821 L*atm/Mol *K
T = 21+273.15 = 294.15
(.877(7.80) / .0821(294.15) =.283 mol H2 = .283(2) = .566 g H2
2006-11-24 03:59:30 · 2 answers · asked by smithwss 2 in Science & Mathematics ➔ Chemistry
Thank You scurvybc & ag_iitkgp!
2006-11-24 08:22:54 · update #1
well aside from that you said the vapor pressure is 18.6 and put 18.9 in your calculations, it looks great! Besides, even with that difference, it doesn't change the answer at all, its still .877 atm with both values.
2006-11-24 04:06:12 · answer #1 · answered by scurvybc 3 · 0⤊ 0⤋
It is.
2006-11-24 04:24:01 · answer #2 · answered by ag_iitkgp 7 · 0⤊ 0⤋