[Hemidol]

The compound NF3 has van der Waals constants a = 3.580 atm•L²/mol² and b = 0.0545 L/mol. Using both the ideal gas law and van der Waals’s equation, calculate the pressure expected for 18 mol of NF3 gas in a 6.00-L container at 30 °C.


Not sure how to approach. Any help appreciated.

[renge ishyo]

Plug the data into the appropriate formula and solve for P.

For the ideal gas law, use:

PV = nRT

For the Van der Waal's Equation, use:

(P + (n²a)/V²)(V-nb) = nRT

[Hemidol]

= 3.580 (18/6.00)^2 * 6 - 0.0545*18
= 161.71218 



(P x a(n/V)2)(V - bn) = nRT is what I used

thus:


P = nRT / V
= 161.71218 / 6.00
=26.95atm