PV = nRT
where, P = pressure = 0.98 atm
V = 200 mL = 0.200 L
n = number of moles
R = Gas constant
T = temperature = 26 + 273 = 299 K
0.98 * 0.200 = n * 0.0821 * 299
0.196 = n * 24.5
n = 0.196 / 24.5 = 0.00800 mole
number of moles = mass / molar mass
0.008 mole = 0.49 g / molar mass
molar mass = 0.49 g / 0.008 mole = 61.3 g/mol
Therefore, molar mass of gas = 61.3 g/mol
12. Compute the molar mass of an unknown pure ideal gas if 3.88 g sample of the gas exerts a pressure of 0.524 atm at 25.1 °C in a container of 4.75 L in volume.
A sample of an unknown compound is vaporized at 200. °C. The gas produced has a volume of 2410. mL at a pressure of 1.00 atm, and it weighs 2·11 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits mol
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