Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Chapter 19, Problem 19.56E
Estimate the rate at which
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A 5.50-mole sample of NH3 gas is kept in a 1.85-L container at 309 K. If the van der Waals equation is assumed to give the correct answer for the pressure of the gas, calculate the percent error made in using the ideal-gas equation to calculate the pressure. (Use a = 4.17 atm·L2·mol−2 and b = 0.0371 L·mol−1 for the van der Waals equation.)
In dry atmospheric air, the four most abundant components are N2, X = 0.808; O2, X = 0.1915; Ar, X = 9.34x10-5; and CO2, X = 4.066x10-4. Calculate the partial pressure of O2, in torr, under standard atmospheric conditions.
A gas mixture being used to simulate the atmosphere of another planet consists of 320 mg of methane, 175 mg of argon, and 225 mg of nitrogen. The partial pressure of nitrogen at 300 K is 15.2 kPa. Calculate (a) the volume and (b) the total pressure of the mixture.
Chapter 19 Solutions
Physical Chemistry
Ch. 19 - Prob. 19.1ECh. 19 - What is the kinetic energy of a single atom of...Ch. 19 - Prob. 19.3ECh. 19 - One mole of Ne atoms confined to a volume of 10.0L...Ch. 19 - Prob. 19.5ECh. 19 - Prob. 19.6ECh. 19 - Prob. 19.7ECh. 19 - Prob. 19.8ECh. 19 - Prob. 19.9ECh. 19 - Prob. 19.10E
Ch. 19 - Prob. 19.11ECh. 19 - Interstellar space can be considered as having...Ch. 19 - Prob. 19.13ECh. 19 - SF6 is a gas at room temperature, 295K. What is...Ch. 19 - Prob. 19.15ECh. 19 - Prob. 19.16ECh. 19 - If relativistic effects were ignored, what...Ch. 19 - Prob. 19.18ECh. 19 - Prob. 19.19ECh. 19 - Prob. 19.20ECh. 19 - Prob. 19.21ECh. 19 - Prob. 19.22ECh. 19 - Prob. 19.23ECh. 19 - Prob. 19.24ECh. 19 - What is the ratio of vrms/vmostprob for any gas at...Ch. 19 - Prob. 19.26ECh. 19 - Prob. 19.27ECh. 19 - Prob. 19.28ECh. 19 - Prob. 19.29ECh. 19 - Prob. 19.30ECh. 19 - Prob. 19.31ECh. 19 - The previous exercise gives an expression for...Ch. 19 - Prob. 19.33ECh. 19 - Prob. 19.34ECh. 19 - Prob. 19.35ECh. 19 - What must the pressure be if the mean free path of...Ch. 19 - Prob. 19.37ECh. 19 - Prob. 19.38ECh. 19 - Prob. 19.39ECh. 19 - Explain why the molecular diameter for argon, at...Ch. 19 - Prob. 19.41ECh. 19 - Prob. 19.42ECh. 19 - Prob. 19.43ECh. 19 - A 1.00-mol sample of Xe gas is kept at a...Ch. 19 - Prob. 19.45ECh. 19 - Prob. 19.46ECh. 19 - Prob. 19.47ECh. 19 - Prob. 19.48ECh. 19 - Prob. 19.49ECh. 19 - Consider a gas mixture containing equal...Ch. 19 - The inverse of the collision rate, 1/z, is the...Ch. 19 - Prob. 19.52ECh. 19 - Prob. 19.53ECh. 19 - Prob. 19.54ECh. 19 - Prob. 19.55ECh. 19 - Estimate the rate at which Hg effuses out a hole...Ch. 19 - Prob. 19.57ECh. 19 - Knudsen effusion cells are used to determine vapor...Ch. 19 - Prob. 19.59ECh. 19 - Prob. 19.60ECh. 19 - Prob. 19.61ECh. 19 - Prob. 19.62ECh. 19 - Prob. 19.63ECh. 19 - Prob. 19.64ECh. 19 - Prob. 19.65ECh. 19 - Prob. 19.66ECh. 19 - Prob. 19.67ECh. 19 - Prob. 19.68ECh. 19 - Prob. 19.69ECh. 19 - Prob. 19.70ECh. 19 - Prob. 19.71ECh. 19 - Prob. 19.72ECh. 19 - Prob. 19.73E
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- Given that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?arrow_forwardA 2.0 L soda bottle is pressurized with 4.5 atm of CO2 at 298 K. If the temperature is increased to 317 K, what is the pressure of the CO2?arrow_forwardHow would the use of a volatile liquid affect the measurement of a gas using open-ended manometers vs. closed-end manometers?arrow_forward
- A sample of hydrogen is collected by displacing a sample of water with a temperature of 35C. The mixture has a total pressure of 114 kPa. What is the partial pressure of the dry hydrogen in kPa?arrow_forwardThe synthesis of ammonia from the elements is conducted at high pressures and temperatures: N2(g) + 3 H2(g) → 2 NH3(g) Suppose that at one stage in the reaction, 13 mol NH3, 31 mol N2, and 93 mol H, are present in the reaction vessel at a total pressure of 210 atm. Calculate the mole fraction of NH3 and its partial pressure.arrow_forwardIn dry atmospheric air, the four most abundant components are N2, X = 0.808; O2, X = 0.1915; Ar, X = 9.34x10-5; and CO2, X = 4.066x10-4. Calculate the partial pressure of Ar, in torr, under standard atmospheric conditions.arrow_forward
- 73. A 500.-mL sample of O2 gas at 24 °C was prepared by decomposing a 3% aqueous solution of hydrogen peroxide, H2 O2, in the presence of a small amount of manganese catalyst by the reaction 2H2 O2 (aq) → 2H2O (g) + The oxygen thus prepared was collected by displacement of water. The total pressure of gas collected was 755 mm Hg. What is the partial pressure of O2 in the mixture? How many moles of O2 are in the mixture? (The vapor pressure of water at 24 °C is 23 mm Hg.)arrow_forward.0380 of Mg strip reacted completely with 6 M HCL in the gas buret and 35.8 mL of hydrogen gas is collected over water at 20 c. The pressure of the "wet" hydrogen gas is adjusted to the outside atmospheric tempertature, a pressure of 747.50 torr. The vapor pressure of water at 20 c is 17.54 torr. using the volume of hydrogen gas collected and the universal gas law, PV = nRT, where R is the gas constant 0.08206 L•atm/mol•K, calculate the experimental number of moles of hydrogen produced.arrow_forwardSulfur dioxide reacts with oxygen in the presence of plati- num to give sulfur trioxide: 2 SO2(g) + O2(g) → 2 SO3(g) Suppose that at one stage in the reaction, 26.0 mol SO2, 83.0 mol O2, and 17.0 mol SO3 are present in the reaction vessel at a total pressure of 0.950 atm. Calculate the mole fraction of SO3 and its partial pressure.arrow_forward
- A gaseous mixture contains 435.0 Torr H2(g), 387.5 Torr N2(g), and 85.3 Torr Ar(g). Calculate the mole fraction, χ, of each of these gases.arrow_forward1) A gas mixture at 300 K consists of 320 mg of methane, 175 mg of argon, and 225 mg of neon. The partial pressure of neon at 300 K is 8.87 kPa. a) Calculate the volume of the mixture b) Calculate the total pressure of the mixturearrow_forward.53 In the Dumas-bulb technique for determining the molar mass of an unknown liquid, you vaporize the sample of a liquid that boils below 100 °C in a boiling-water bath and determine the mass of vapor required to fill the bulb. From the following data, calculate the molar mass of the unknown liquid: mass of unknown vapor, 1.012 g; volume of bulb, 354 cm; pressure, 742 torr; temperature, 99 °C. 3.arrow_forward
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