posted by Tyran on .
A 32.0 mL sample of hydrogen is collected over water at 20.0 degrees celcius and 750.0 torr. What is the volume of the dry gas at STP?
I forgot to add-- Vapor pressure of water at 20.0 degrees celcius is 17.5 torr.
(P1V1)/T1 = (P2V2/T2)
P1 = 750 torr - vapor pressure H2O @ 20 degrees Celsius (note the correct spelling of Celsius).
V1 = 32 mL
T1 = change C to Kelvin.
P2 and T2 are STP; i.e., 760 torr and 273 K.
Post your work if you get stuck.
What do you mean by P1, meaning 750 torr - vapor pressure H2O @ 20 degrees Celsius?
750 torr - 17.5 torr = ?? torr = P1.
According to Dalton's Law of Partial Pressure, the total pressure is the sum of the partial pressures in the gas.
P(gas) + P(water) = total P = 750 torr. That's what you started with in the problem.
i don't understand the P2 and T2 part with the STP