Ideal Gas Law: Solve 1.0x10-6 mmHg @ 40°C

AI Thread Summary
To determine the number of molecules in 1.00 cm³ at a pressure of 1.0x10^-6 mmHg and a temperature of 40°C, the ideal gas law (PV=nRT) is applied. The pressure must be converted from mmHg to Pascals, and the temperature should be converted to Kelvin for accurate calculations. Additionally, the volume of 1.00 cm³ needs to be converted to cubic meters. Following these conversions will yield the correct number of moles (n) and subsequently the number of molecules. Proper unit conversions are crucial to avoid erroneous results in the calculations.
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Homework Statement



Current vacuum technology can achieve a pressure of 1.0x10-6 mm of Hg. At this pressure, and at a temperature of 40.0 C, how many molecules are in 1.00cm3 ?


2. Homework Equations [/b


pv=nrt

The Attempt at a Solution

i solved it using the ideal gas equation and got a very large n value,after converting from mmHg to Pa? would that be the correct procedure?
 
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Please show your attempt at solving the problem.
 
quick few hints to doing this if your getting odd answers. a) temp needs to be converted to kelvin and b) the 1cm^3 needs to be correctly converted into m^3
 
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