A 15.0 g sample of MgCO₃ is placed in a 1.0 L reaction vessel along with excess HNO₃. The following reaction then occurs at 350 K: MgCO₃(s) + 2 HNO₃(aq) → Mg(NO₃)₂(aq) + H₂O(l) + CO₂(g). Use the van der Waals equation to calculate the pressure of CO₂(g) in the vessel, taking into account the volume of the non-gaseous products. The constants for CO₂(g) are a = 3.607 atm L²/mol² and b = 0.04286 L/mol. Assume the non-gaseous products occupy a total volume of 111.6 mL.

What is the purpose of the van der Waals equation in describing the behavior of real gases?

Using the ideal van der Waals equation and then the ideal gas equation, calculate the pressure of a 3.524-mol sample of N₂ gas in a 0.8500-L flask at 415°C. Within the limits of the significant figures justified by these parameters, will the ideal gas equation overestimate or underestimate the pressure? If so, by how much? For N₂, a = 1.39 L²atm/mol² and b = 0.0391 L/mol.