Question

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A certain mass of nitrogen gas occupies a volume of 8.82 L at a pressure of 7.80 atm. At what pressure will the volume of this sample be 11.20 L? Assume constant temperature and ideal behavior.

Answer 1

To find the pressure of the nitrogen gas According to boyle's law PV = P, V2 P, and V, are the initial pressure and volume of the gas P, and V, are the final pressure and volume of the gas P = 7.80 atm Vi = 8.82L V, = 11.20L Py = ? PV = P, V2 P, 7.80atm 8.82 11.20L = 6.14 atm Hence the pressure of the nitrogen gas = 6.14 atm

(6) To find the volume of the gas According to combined gas law PV PV T, T, where P= initial pressure V, = initial volume T = initial temperature Py = final pressure V = final volume Ty = final temperature Given that P = 1.60 atm Py = 0.986 atm Vi = 3.60L V, = ? Change the temaparature to kelvin T = 14.40+273K = 287.4K T, = 19.80+273K = 292.8K PV P, V2 TL T, 1.60 atm x 3.60L 0.986 atm x V, 287.4K 292.8K Cross multiplication are allowed 1.60 atm x 3.60L x 292.8K = 287.4K *0.986 atm V v 1.60 atm x 3.60L x 292.8K 287.4K *0.986 atm 1.60x3.60x292.8, 287.4x0.986 V, = 5.95L Hence the volume of the gas = 5.95L 201

To find the pressure of the gas Given that Use the ideal gas law: PV = nRT p = pressure V = volume n=n moles of any gas R = gas constant T = temperature in kelvin p=? V = 12.5 L n = 73.5 mole R = 0.0821 L atm/Kmol T = 89.00°C+273K = 362K PV =nRT P=nRT 73.5moles x 0.0821L atm/K molx 362K 12.5L = 174 atm Hence the pressure of the gas = 174 atm