Problem: The vapor pressure of CCl3F at 300 K is 856 torr. If 12.5 g of CCl3 F is enclosed in a 1.2 L container, calculate the number of moles of CCl3F in the gas phase.

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FREE Expert Solution

We are asked to calculate the number of moles of CCl3F in the gas phase.


Use the ideal gas law : 

PV = nRTn = PVRT 


Convert the values need to be consistent with  R. 

R = 0.08206 L-atm/mol-K

P = 856 torr × 1 atm760 torr  = 1.12 atm

V = 1.2 L

T = 300 K 


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Problem Details

The vapor pressure of CCl3F at 300 K is 856 torr. If 12.5 g of CCl3 F is enclosed in a 1.2 L container, calculate the number of moles of CCl3F in the gas phase.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Scott's class at OLE MISS.