Problem: Calculate the pressure (atm) that CCl4 will exert at 43 °C if 1.20 mol occupies 33.5 L, assuming that Part A  CCl4 obeys the ideal-gas equation: Part B  CCl4 obeys the van der Waals equation. (Values for the van der Waals constants are a = 20.4, b = 0.1383.)

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Problem Details

Calculate the pressure (atm) that CCl4 will exert at 43 °C if 1.20 mol occupies 33.5 L, assuming that 

Part A  CCl4 obeys the ideal-gas equation: 


Part B  CCl4 obeys the van der Waals equation. (Values for the van der Waals constants are a = 20.4, b = 0.1383.)



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Our tutors have indicated that to solve this problem you will need to apply the Van der Waals Equation concept. You can view video lessons to learn Van der Waals Equation. Or if you need more Van der Waals Equation practice, you can also practice Van der Waals Equation practice problems.

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