For carbon dioxide gas (CO₂), the constants in the van der Waals equation are a = 0.364 J ⋅ m³/mol² and b = 4.27 × 10⁻⁵ m³/mol. (a) If 1.00 mol of CO₂ gas at 350 K is confined to a volume of 400 cm³, find the pressure of the gas using the ideal-gas equation and the van der Waals equation. (b) Which equation gives a lower pressure? Why? What is the percentage difference of the van der Waals equation result from the ideal-gas equation result? (c) The gas is kept at the same temperature as it expands to a volume of 4000 cm³. Repeat the calculations of parts (a) and (b). (d) Explain how your calculations show that the van der Waals equation is equivalent to the ideal-gas equation if n/V is small?