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.

The following table shows the values of the van der Waals constants a and b for CH₄ and NO₂. Which of the two gases is expected to be close to the ideal behavior at low temperatures?

The volume occupied by the particle of gases represents a quarter of the van der Waals constant b.

Incorporating this statement into the ideal gas law, calculate the fraction of the volume in a container actually occupied by Ne atoms at 126.7 kPa pressure and 15 °C. 

Calculate the volume of 10.00 mol of helium at 100.0 atm and 300.0 K using both the ideal gas equation and the Van der Waals equation. Explain the difference in values obtained.

For 1-mol sample of gas in a 1-L container, the graph for the change in pressure as the temperature increases is shown below. The four plots represent an ideal gas and three real gases: sulfur dioxide (SO₂), argon (Ar), and ammonia (NH₃).

Given the van der Waals constants below, assign the gases (SO₂, Ar, NH₃) to their corresponding plots (A, B, C).