Help please. According to the ideal gas law, a 0.9601 mol sample of krypton gas in a 1.751 L container at 271.7 K should exert a pressure of 12.23 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For Kr gas, a = 2.318 L2atm/mol2 and b = 3.978E-2 L/mol.

How do you go about doing this?

Question

Help please. According to the ideal gas law, a 0.9601 mol sample of krypton gas in a 1.751 L container at 271.7 K should exert a pressure of 12.23 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For Kr gas, a = 2.318 L2atm/mol2 and b = 3.978E-2 L/mol.

How do you go about doing this?

aaronq · Answer

solve for pressure using each formula separately, then find the percent difference, i would take the ideal pressure as the point of reference, so:

$\dfrac{|P_{real}-P_{Ideal}|}{P_{ideal}}*100\%$

anonymous · Answer

Which formulas?

anonymous · Answer

Don't you just need the ideal gas law?

aaronq · Answer

oh wait, i didn't see you they had given you pressure in ideal conditions. Use the van der waals equation.

anonymous · Answer

got it! thank you so much Aaron!