11. A rigid 8.80 L container is charged with 0.700 mol of helium gas at 9.00 C. An identical container is charged with 0.700 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 correct numeric value with the appropriate number of significant figures. Express scientific notation like 4.29E-15 Pa

11. A rigid 8.80 L container is charged with 0.700 mol of helium gas at 9.00 C. An identical container is charged with 0.700 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 correct numeric value with the appropriate number of significant figures. Express scientific notation like 4.29E-15 Pa

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 152CP: You have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted...

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You have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/L. Assume ideal behavior and constant temperature and pressure. a. What is the mole fraction of He in the original mixture? b. The SO2 and O2 react to completion to form SO3. What is the density of the gas mixture after the reaction is complete?
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?
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)?
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.
93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
Calculate the molar volume of ethane at 1.00 atm and 0C and at 10.0 atm and 0C, using the van der Waals equation. The van der Waals constants are given in Table 5.7. To simplify, note that the term n2a/V2 is small compared with P. Hence, it may be approximated with negligible error by substituting nRT/P from the ideal gas law for V in this term. Then the van der Waals equation can be solved for the volume. Compare the results with the values predicted by the ideal gas law.
Consider a 5.00-L tank containing 325 g of H2O at a temperature of 275 C. (a) Calculate the pressure in the tank using both the ideal gas law and the van der Waals equation. (b) Which correction term, a(n/V)2 or bn, has the greatest influence on the pressure of this system?