Posted by **Hannah** on Saturday, January 14, 2012 at 5:46pm.

According to the ideal gas law a 9.03 sample of oxygen gas in a 0.8112 container at 499k should exert a pressure of 456atm. By what % does the pressure calculated using van der waals equation differ from the ideal pressure?

For O2 gas a=1.36 L^2atm/mol2 and b=3.18e-2

Hint: %diff= 100 X (P ideal - P van der waal) / P ideal

I know that van der waals equation is

(P + a [n/v]^2) (v-bn) = nRT but I have no idea how to use this and my textbook does not give any examples. Thank you for your help!

- Chemistry -
**DrBob222**, Saturday, January 14, 2012 at 10:10pm
First, you omitted the units on the 9.03 WHAT in a 0.8112 WHAT container. I'm confused because you are confused. There is nothing here that you need an idea about. You have a and b, R, T, and n. Solve for P by van d equation, then use the usual PV = nRT and solve for P. Then follow the hint in the problem which tells you how to solve for the % difference.

## Answer this Question

## Related Questions

- Chemistry - For Carbon dioxide, for a volume of 500 mL and temperature of 100 ...
- Chemistry - The compound CH3F has van der Waals constants a = 5.009 atm•L2 /mol ...
- Chemistry - Using the information on the table of van der Waals Constants of ...
- Chemistry - Using the information on the table of van der Waals Constants of ...
- Chemistry - Using the information on the table of van der Waals Constants of ...
- chemistry - A 9.96 mol sample of methane gas is maintained in a 0.836 L ...
- Gases - van der waals - It turns out that the van der Waals constant b equals ...
- chemistry - If I contain 3 moles of gas in a container with a volume of 60 ...
- Chemistry-Please help - If 1.00mol of argon is placed in a 0.500- container at ...
- Chemistry - 15.0 moles of gas are in a 6.00L tank at 298.15K. Calculate the ...

More Related Questions