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Chemistry 56 Online
OpenStudy (anonymous):

Will medal "Determine the partial pressure of the hydrogen collected in the gas collection tube." I'm having trouble wuth this, I know I have to do this: partial pressure H2 = total pressure - vapor pressure of water. I know the vapor pressure of water, it's 18.7 torr, but I don't know how to know the total pressure. Just in case here's the rest of the info I gathered: Volume of collected gas mL, 28 : Barometric pressure, 1.1 : Room temp Celsius, 21

OpenStudy (anonymous):

ok, I think that helped, if i did this right I have 14 moles

OpenStudy (anonymous):

I have to do PV=nRT

OpenStudy (anonymous):

\[P 28 = 14 R 294.15\]

OpenStudy (anonymous):

Idk what R to use, would I use the same one as in the video? I'm going to assume that's the one I use

OpenStudy (anonymous):

so \[P28=14\times8.315 m ^{3} Pa/moles K \times 294.15\]

OpenStudy (inexilewetrust):

That seems right to me, but I need a second opinion. I am really rusty on this. I get it, but I am not completely sure.

OpenStudy (inexilewetrust):

@e.mccormick @bibby @shamim @Directrix

OpenStudy (anonymous):

@dtan5457

OpenStudy (somy):

units pay attention to units you are using

OpenStudy (anonymous):

did I get the units wrong?

OpenStudy (somy):

if u r using L for volume atm for pressure R = 0.08206 if you are using m3 for volume Pa for pressure R = 8.31

OpenStudy (somy):

from the working u showed yes, the unit that u used for volume is incorrect

OpenStudy (anonymous):

oh ok, so I should've used the first one you mentioned?

OpenStudy (somy):

yeah if thats easier for you :)

OpenStudy (somy):

dont forget about temperature bein in Kelvin unit, in both cases

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