If 7.46 g of gas occupies 2.89 L at 841 mm Hg and 27.63 degree celsius what is the molar mass of the gas?

Answer 1

Assume ideal gas, therefore use ideal gas law to calculate number of moles: n = PV/RT where R = 0.08206 L*atm/mol*K n = (1 atm)*(0.639 L) / (0.08206 L*atm/mol*K)*(300K) n = 0.02596 mol gas MW = mass/mol = 2.82 g/0.02596 mol or 108.6 g/mol

Answer 2

Remember that the molar mass is in units of g/mol. You're going to need to use the Ideal Gas Law: PV = nRT, where P is pressure in Torr(mm Hg), V is volume in L, n is the number of moles, R is the ideal gas constant(62.363 L*Torr(mm Hg)/K*mol), and T is the temperature in Kelvin (temperature in Celsius plus 273.16).

You know the volume, pressure, and temperature of the gas, so you can solve for n, the number of moles using the solved equation n = PV/RT. Once you have the number of moles, you can divide the number of grams of gas by the number of moles of gas to get the molar mass (g of gas/moles of gas).

Answer 3

PV/T = PV/T

0.961x1.00/300 = 1xV/273

V = 0.87451 L at stp ... 1 mole occupies 22.4 L at stp, so

0.87451 / 22.4 = 0.039040625 mole

1.25 g / 0.039040625mole = 32.02 g/mole

Answer 4

If it occupies 3.16 liters at STP, then that's 0.14 moles. 2.82g/0.14mol=20.14g/1mol, and that's the Atomic Mass of neon, so the gas is neon, and its atomic mass is 20.14 grams/mole.