Question
60.0 mL of O2 was collected over water at a total pressure of 755 torr and a temp of 25C. The vapor pressure of water at 25C is 24 torr. How many moles of O2 were collected?
Could you please explain and show the steps? I know the answer is 2.36x10^-3.
Could you please explain and show the steps? I know the answer is 2.36x10^-3.
Answers
DrBob222
Ptotal = pO2 + pH2O
755 torr = pO2 + 24
pO2 = 755-24 = 731 torr
P in atm = 731/760 = ?
V = 0.060L
T = 298 K
R = 0.08206 L*atm/mol*K
Use PV = nRT and solve for n.
755 torr = pO2 + 24
pO2 = 755-24 = 731 torr
P in atm = 731/760 = ?
V = 0.060L
T = 298 K
R = 0.08206 L*atm/mol*K
Use PV = nRT and solve for n.