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17 Nov 2019
Calculate the pressure exerted at 1000 K by 2 moles of C2H6 in a volume of 0.5 dm3 behaving as: (a) a perfect gas and (b) a van der Waals gas. [The van der Waals parameters for C2H6 are a = 5.562 dm6 atm mol-2 and b = 0.0638 dm3 /mol]. By what percentage does pressure obtained for the perfect gas deviate from the van der Waals prediction?
The vapor pressure of H2O at body temperature is 47 Torr. What is the partial pressure of dry air in our lungs when the total pressure is 760 Torr?
If the rms speed of CO2 molecules near the surface of Mars is 355 m/s, what is the surface temperature?
Calculate the pressure exerted at 1000 K by 2 moles of C2H6 in a volume of 0.5 dm3 behaving as: (a) a perfect gas and (b) a van der Waals gas. [The van der Waals parameters for C2H6 are a = 5.562 dm6 atm mol-2 and b = 0.0638 dm3 /mol]. By what percentage does pressure obtained for the perfect gas deviate from the van der Waals prediction?
The vapor pressure of H2O at body temperature is 47 Torr. What is the partial pressure of dry air in our lungs when the total pressure is 760 Torr?
If the rms speed of CO2 molecules near the surface of Mars is 355 m/s, what is the surface temperature?
Jean KeelingLv2
7 Jan 2019