Van der Waals equation: In Exercise 14 at the end of Section 2.3, we discussed the ideal gas law, which shows the relationship among volume V , pressure p, and temperature T for a fixed amount (1...

Van der Waals equation: In Exercise 14 at the end of Section 2.3, we discussed the ideal gas law, which shows the relationship among volume V , pressure p, and temperature T for a fixed amount (1 mole) of a gas. But chemists believe that in many situations, the van der Waals equation gives more accurate results. If we measure temperature T in kelvins, volume V in liters, and pressure p in atmospheres (1 atm is the pressure exerted by the atmosphere at sea level), then the relationship for carbon dioxide is given by

What volume does this equation predict for 1 mole of carbon dioxide at 500 kelvins and 100 atm? (Suggestion: Consider volumes ranging from 0.1 to 1 liter.)