Posted by **Amber** on Monday, September 29, 2008 at 3:57pm.

One mole of a van der Waals gas with a=15.0 l^2 atm mol^−2 and b=0.015 l

mol^−1 is expanded reversibly and isothermally from 1 atm to 0.5 atm at a temperature of

300 K. Calculate w for this process, and compare it with that required to expand an ideal

gas between the same volumes (calculating the volumes will be one of the trickiest parts of

this problem).

## Answer This Question

## Related Questions

- Chemistry - Use van der Waals’ equation to calculate the pressure exerted by 2....
- Chemistry - The compound CH3F has van der Waals constants a = 5.009 atm•L2 /mol ...
- Chemistry - Using the van der Waals equation, determine the pressure of 436.0g ...
- Chemistry - 15.0 moles of gas are in a 6.00L tank at 298.15K. Calculate the ...
- ap chemistry - 1.95 mol of an ideal gas at 300 K and 3.00 atm expands from 16 L ...
- chemistry - I have a problem that states: Find the pressure of a sample of ...
- Chemistry - Each of the following processes is spontaneous as described. Which ...
- Chemistry - Using the van der Waals equation, calculate the pressure (in ...
- Chemistry..Please Help - HENRY'S LAW I did the first one im not sure how to do ...
- chemistry - A 9.96 mol sample of methane gas is maintained in a 0.836 L ...

More Related Questions