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?
7 answers
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.
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.
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
No
29.4 mL
2 answers