16.0 g CO2 is 16.0/44 = 0.354 mols.
PV = nRT
P = nRT/V = 0.354*0.08203*302/3.23 = 2.72 atm absolute
2.72 atm x (14.7 psi/1 atm) = 39.9 psi absolute
Gauge pressure = 39.9 - 14.7 = ?
Pressurized carbon dioxide inflators can be used to inflate a bicycle tire in the event of a flat. These inflators use metal cartridges that contain 16.0 g of carbon dioxide.At 302 K , to what pressure (in psi) can the carbon dioxide in the cartridge inflate a 3.23 L mountain bike tire? (Note: The gauge pressure is the difference between the total pressure and atmospheric pressure. In this case, assume that atmospheric pressure is 14.7 psi.)
2 answers
turn 16 g of carbon dioxide to moles
(g/molar mass) (0.3636)
then plug into PV=nRT
P=(0.3636 moles of carbon dioxide)(0.0821)(302 temperature in kelvin)/ 3.23 volume in liters
this should equal to 2.79 atm
convert atm to psi by multiply 2.79 by 14.7
should b 41 psi, after this subtract 41 psi by 14.7
26.3 psi is the answer
(g/molar mass) (0.3636)
then plug into PV=nRT
P=(0.3636 moles of carbon dioxide)(0.0821)(302 temperature in kelvin)/ 3.23 volume in liters
this should equal to 2.79 atm
convert atm to psi by multiply 2.79 by 14.7
should b 41 psi, after this subtract 41 psi by 14.7
26.3 psi is the answer
1 answer