Determine the unknown property of a perfect gas

AI Thread Summary
The discussion focuses on determining the unknown temperature of a perfect gas, specifically argon, given its mass, pressure, and volume. The ideal gas law equation (PV=nRT) is applied, but there is confusion regarding the calculation of the number of moles of argon from its mass. Participants clarify that the molar mass of argon is approximately 40 g/mol, leading to a calculation of moles as 6.75 rather than 0.0067. The final temperature is recalculated, emphasizing the importance of accurate mole conversion in solving gas law problems. Accurate understanding of these concepts is crucial for correctly applying the ideal gas law.
thermo15378
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Homework Statement



two hundred seventy grams of argon at a pressure of 160kpa and a volume of 1.3 m^3.

Homework Equations


pv=nrt


The Attempt at a Solution



(160^3)(1.3) = (.27)(8.31)(t)

208=2.2437t
t=92.7
 
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thermo15378 said:

Homework Statement



two hundred seventy grams of argon at a pressure of 160kpa and a volume of 1.3 m^3.

Homework Equations


pv=nrt


The Attempt at a Solution



(160^3)(1.3) = (.27)(8.31)(t)

208=2.2437t
t=92.7
Not quite. n is the number of moles. How many moles of argon in .27 kg of argon?

AM
 
0.0067 is what i get for moles but when i plug in the formula I am getting 3649.12 and that cannnot be right.
 
thermo15378 said:
0.0067 is what i get for moles but when i plug in the formula I am getting 3649.12 and that cannnot be right.
What is the mass of one mole of Argon?

AM
 

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