11. A rigid 9.80 L container is charged with 0.900 mol of helium gas at 25.0 C. An identical container is charged with 0.900 mol of carbon dioxide gas at the same temperature. Use the van der Waals equation of state with the data below to predict the difference in pressure between the two containers. The van der Waals equation of state is (P + a(n/V)²)(V-nb) = nRT Gas a (m Pa/mol²) b (m³/mol) He 3.457E-3 2.37E-5 CO₂ 0.3640 4.267E-5 Enter the value with the appropriate number of significant figures. Pa Hint: Solve the van der Waals equation for pressure: P = nRT/(V-nb) - a(n/V)² Use SI units! Grade This Exercise

11. A rigid 9.80 L container is charged with 0.900 mol of helium gas at 25.0 C. An identical container is charged with 0.900 mol of carbon dioxide gas at the same temperature. Use the van der Waals equation of state with the data below to predict the difference in pressure between the two containers. The van der Waals equation of state is (P + a(n/V)²)(V-nb) = nRT Gas a (m Pa/mol²) b (m³/mol) He 3.457E-3 2.37E-5 CO₂ 0.3640 4.267E-5 Enter the value with the appropriate number of significant figures. Pa Hint: Solve the van der Waals equation for pressure: P = nRT/(V-nb) - a(n/V)² Use SI units! Grade This Exercise

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter8: Gases

Section: Chapter Questions

Problem 156CP

See similar textbooks

Similar questions

A cylinder of compressed gas is labeled Composition (mole %): 4.5% H2S, 3.0% CO2, balance N2. The pressure gauge attached to the cylinder reads 46 atm. Calculate the partial pressure of each gas, in atmospheres, in the cylinder.
5-107 If 60.0 g of NH3 occupies 35.1 L under a pressure of 77.2 in. Hg, what is the temperature of the gas, in °C?
You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find out which, you have decided to measure its molar mass. (a) First, yon determine that the density of the gas is 5.60 g/L at a pressure of 0.971 atm and a temperature of 18.2 C. Calculate the molar mass and identify the compound. (b) To check the results from part (a), you decide to measure the molar mass based on the relative rales of effusion of the unknown gas and CO2. You find that CO2 effuses at a rate of 0.050 mol/min, whereas the unknown phosphorus fluoride effuses at a rate of 0.028 mol/min. Calculate the molar mass of the unknown gas based on these results.
In the anaerobic oxidation of glucose by yeast, CO2 is produced: If 1.56 L of CO2 were produced at 22.0 C and 0.965 atm, what mass of C6H12O6 is consumed by the yeast? Assume the ideal gas law applied.
Under what conditions does the behavior of a real gas begin to differ significantly from the ideal gas law?
The density of air 20 km above Earths surface is 92 g/m3. The pressure of the atmosphere is 42 mm Hg, and the temperature is 63 C. (a) What is the average molar mass of the atmosphere at this altitude? (b) If the atmosphere at this altitude consists of only O2 and N2, what is the mole fraction of each gas?