The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: (V-nb) = nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? What are the units of b? Fraction For carbon dioxide the numerical value of a is 3.592 and the numerical value of b is 0.0429. atm Use the van der Waals equation to calculate the pressure of a ロ回

The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: (V-nb) = nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? What are the units of b? Fraction For carbon dioxide the numerical value of a is 3.592 and the numerical value of b is 0.0429. atm Use the van der Waals equation to calculate the pressure of a ロ回

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 143CWP: A certain flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon...

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Helium gas, He, at 22C and 1.00 atm occupied a vessel whose volume was 2.54 L. What volume would this gas occupy if it were cooled to liquid-nitrogen temperature (197C)?
A certain flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon is at sea level where the temperature is 25C and the barometric pressure is 730 torr. The balloon then rises to an altitude of 6000 ft, where the pressure is 605 torr and the temperature is 15C. What is the change in volume of the balloon as it ascends from sea level to 6000 ft?
Consider the following unbalanced chemical equation: ^Sfr) + O2(g) —? Cu2O(s) + SO2(g) What volume of oxygen gas, measured at 27.5 °C and 0.998 atm. is required to react with 25 g of copper!I) sulfide? What volume of sulfur dioxide gas is produced under the same conditions?
Hyperbaric oxygen therapy is used to treat patients with carbon monoxide poisoning as well as to treat divers with the bends. In hyperbaric oxygen therapy, a patient is placed inside a 7.0-ft cylinder with a 3.0-ft diameter, which is then filled with oxygen gas to a total pressure of 2.50 atm. Assuming the patient takes up 32.0% of the chambers volume , what volume of O2(g) from a gas cylinder at 25 C and 95 atm is required to fill the chamber to a total pressure of 2.50 atm at 25 C7 Assume the hyperbaric chamber initially contains air at 1.00 atm before O2(g) is added.
A 0.105-g sample of a gaseous compound has a pressure of 561 mm Hg in a volume of 125 mL at 23.0 C. What is its molar mass?
You have a helium balloon at 1.00 atm and 25C. You want to make a hot-air balloon with the same volume and same lift as the helium balloon. Assume air is 79.0% nitrogen and 21.0% oxygen by volume. The lift of a balloon is given by the difference between the mass of air displaced by the balloon and the mass of gas inside the balloon. a. Will the temperature in the hot-air balloon have to be higher or lower than 25C? Explain. b. Calculate the temperature of the air required for the hot- air balloon to provide the same lift as the helium balloon at 1.00 atm and 25C. Assume atmospheric conditions are 1.00 atm and 25C.
Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?
Raoul Pictet, the Swiss physicist who first liquefied oxygen, attempted to liquefy hydrogen. He heated potassium formate, KCHO2, with KOH in a closed 2.50-Lvessel. KCHO2(s)+KOH(s)K2CO3(s)+H2(g) If 75.0 g of potassium formate reacts in a 2.50-L vessel, which was initially evacuated, what pressure of hydrogen will be attained when the temperature is finally cooled to 25C? Use the preceding chemical equation and ignore the volume of solid product.
In the text, it is stated that the pressure of 4.00 mol of Cl2 in a 4.00-L tank at 100.0 C should be 26.0 atm if calculated using the van der Waals equation. Verify this result, and compare it with the pressure predicted by the ideal gas law.