Use the van der Waals equation of state to calculate the pressure of 3.90 mol of N,0 at 453K in a 5.80 L vessel. Van der Waals constants can be found in the van der Waals constants table. atm Use the ideal gas equation to calculate the pressure under the same conditions. atm In a 17.00 L vessel, the pressure of 3.90 mol of N,O at 453 K is 8.53 atm when calculated using the ideal gas cquation and 8.42 atm when calculated using the van der Waals equation of state. Why is the percent difference in the pressures calculated using the two different equations greater when the gas is in the 5.80 L vessel compared to the 17.00 L vessel? O The molecular volume is a larger part of the total volume of the 5.80 L vessel. O The molecular volume is a smaller part of the total volume of the 5.80L vessel. The attractive forces between molecules become less of a factor at the higher pressure in the 5.80L vessel. O The attractive forces between molecules become a greater factor at the higher pressure in the 5.80 L vessel.

A particle is immersed in a gas. What would happen with the gas pressure the particleexperiences if the density of the gas was halved?. Explain.

23. What will happen if an inflated balloon is placed in front of a floor register 23. that blows a warm air? A. The balloon will get completely deflated B. The balloon will become larger. C. The balloon will become smaller. D. The balloon will maintain its size. E. All the above will happen.