Answer :
Final answer:
The molar mass of the unknown gas is calculated using the rearranged Ideal Gas Law to find the number of moles, and then taking the mass of the sample divided by this number. The resulting molar mass is around 50 g/mol, so the closest answer is option c) 49.6 g/mol.
Explanation:
The subject of your question involves using the Ideal Gas Law to find the molar mass of an unknown substance.In this case, you would rearrange the the ideal Gas equation, PV=nRT, to solve for n, the number of moles. Here, P is the pressure, V is the volume, R is the ideal gas constant, and T is the temperature. However, because we're after the molar mass, we'll divide the mass of the sample by the number of moles we get. Once all the units have been properly converted and the gas constant for the correct pressure units is chosen, we'd plug in:
n = PV/RT = (639 mmHg * 0.828 L) / (62.363 L*mmHg/K*mol * 311.65K) ≈ 0.034 mol
Then Molar mass = Mass of sample/moles ≈ 1.70g / 0.034 mol = 50 g/mol. So the molar mass of this compound is around 50 g/mol, which would best align with option c) 49.6 g/mol.
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