# Need chem help What volume is occupied by 1.00 kg of helium at 5.00◦C at a pressure of 735 Torr?

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- lenpol7Lv 71 month ago
Using the Ideal Gas Equation

PV = nRT

V = nRT/P

Where

n = moles(He) = 1000g / 4 = 250 moles

R = Gas Constant 8.413.

T = temperature in Kelvvin K (5 + 273 = 278

P = pressure in Pascals(Pa) 98,19213 Pa

Hence

V = 250 x 8.314 x 278 / 98192

V = 5.88 m^3 ( NOT dm^3 nor cm^3, but cubic metres).

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- pisgahchemistLv 71 month ago
Ideal gas equation problem ....

PV = nRT ................ ideal gas equation

PV = mRT / M ......... n=m/M ... m=mass, M=molar mass

V = mRT / (PM) ....... solve for V

V = 1000g x 62.36Ltorr/molK x 278.15K / 735 torr / 4.00 g/mol

V = 5.90x10^3 L ....... to three significant digits

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- davidLv 71 month ago
1Kg == 1000/4 = 250 moles

V = nRT/P = (250)(62.4)(278)/735

V = 5900 L

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