15.0 moles of gas are in a 3.00l tank at 23.4∘c . calculate the difference in pressure between methane and an ideal gas under these conditions. the van der waals constants for methane are a=2.300l2⋅atm/mol2 and b=0.0430 l/mol..

Using PV=nRT or the ideal gas equation, we substitute n= 15.0 moles of gas, V= 3.00L, R equal to 0.0821 L atm/ mol K and T= 296.55 K and get P equal to 121.73 atm. The Van der waals equation is (P + n^2a/V^2)*(V-nb) = nRT.  Substituting  a=2.300L2⋅atm/mol2 and b=0.0430 L/mol, P is equal to 97.57 atm. The difference is 121.73 atm- 97.57 atm equal to 24.16 atm.

Carbon based or cells?