Calculate Molar Mass of Gas: 0.6536 g/L @ 37C & 787 torr

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To calculate the molar mass of a gas with a density of 0.6536 g/L at 37°C and 787 torr, the ideal gas law (PV = nRT) was applied, resulting in a calculated molar mass of approximately 16.05 g/mol. The discussion highlights confusion regarding the next steps after finding the molar mass. Participants suggest that the molecular formula of the gas might be CH4, as it closely matches the calculated molar mass. The conversation emphasizes the importance of understanding the relationship between density, temperature, pressure, and molar mass in gas calculations. Overall, the thread focuses on the calculation process and identifying the molecular formula based on the derived molar mass.
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Calculate the molar mass of a gas that has a density of 0.6536 g/L at 37C and 787 torr. What do you think the?

My attempt:

I used n= PV/RT and calculated the number of moles to be 16.0548g/mol.

The second part is where I am confused. Anyone help?
 
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chemistry4all said:
Calculate the molar mass of a gas that has a density of 0.6536 g/L at 37C and 787 torr. What do you think the?

My attempt:

I used n= PV/RT and calculated the number of moles to be 16.0548g/mol.

The second part is where I am confused. Anyone help?

Second part? Eh?
 


oops didnt finish the last sentence. It is "What do you think you think the molecular formula of the gas is?


I think its CH4 because that's the only molecule I can find that has a MM close to 16g.
 
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