McMurry - Chemistry 8th Edition - Chapter 10

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Ch.10 - Gases: Their Properties & Behavior

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McMurry 8th Edition

Ch.10 - Gases: Their Properties & Behavior

Problem 72a
Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s) + 2 HCl(aq) ¡ ZnCl₂(aq) + H₂(g) (a) How many liters of H₂ would be formed at 742 mm Hg and 15 °C if 25.5 g of zinc was allowed to react?
Problem 72b
Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s) + 2 HCl(aq) ¡ ZnCl₂(aq) + H₂(g) (b) How many grams of zinc would you start with if you wanted to prepare 5.00 L of H2 at 350 mm Hg and 30.0 °C?
Problem 73
Ammonium nitrate can decompose explosively when heated according to the equation 2 NH4NO31s2¡2 N21g2 + 4 H2O1g2 + O21g2 How many liters of gas would be formed at 450 °C and 1.00 atm pressure by explosion of 450 g of NH4NO3?
Problem 74
The reaction of sodium peroxide 1Na2O22 with CO2 is used in space vehicles to remove CO2 from the air and generate O2 for breathing: 2 Na2O21s2 + 2 CO21g2¡2 Na2CO31s2 + O21g2 (a) Assuming that air is breathed at an average rate of 4.50 L/min (25 °C; 735 mm Hg) and that the concentration of CO2 in expelled air is 3.4% by volume, how many grams of CO2 are produced in 24 h?
Problem 75a
Titanium(III) chloride, a substance used in catalysts for preparing polyethylene, is made by high-temperature reaction of TiCl₄ vapor with H₂: 2 TiCl₄(g) + H₂(g) → 2 TiCl₃(s) + 2 HCl(g) (a) How many grams of TiCl₄ are needed for complete reaction with 155 L of H₂ at 435 °C and 795 mm Hg pressure?
Problem 75b
Titanium(III) chloride, a substance used in catalysts for preparing polyethylene, is made by high-temperature reaction of TiCl₄ vapor with H₂: 2 TiCl₄(g) + H₂(g) → 2 TiCl₃(s) + 2 HCl(g) (b) How many liters of HCl gas at STP will result from the reaction described in part (a)?
Problem 76
A typical high-pressure tire on a bicycle might have a volume of 365 mL and a pressure of 7.80 atm at 25 °C. Suppose the rider filled the tire with helium to minimize weight. What is the mass of the helium in the tire?
Problem 77
Assume that you have 1.00 g of nitroglycerin in a 500.0-mL steel container at 20.0 °C and 1.00 atm pressure. An explosion occurs, raising the temperature of the container and its contents to 425 °C. The balanced equation is 4 C3H5N3O91l2¡ 12 CO21g2 + 10 H2O1g2 + 6 N21g2 + O21g2 (c) What is the pressure in atmospheres inside the container after the explosion according to the ideal gas law?
Problem 78
One of the largest sources of SO2 to the atmosphere is coal-fired power plants. Calculate the volume of SO2 in liters produced by burning 1 kg of coal that contains 2% sulfur. Assume all the sulfur is converted to SO2.
Problem 79
Smelting of ores to produce pure metals is an atmospheric source of sulfur dioxide. (a) Galena, the most common mineral of lead, is primarily lead(II) sulfide (PbS). The first step in the production of pure lead is to oxidize lead sulfide into lead(II) sulfite (PbSO3). Lead(II) sulfite is then thermally decomposed into lead(II) oxide and sulfur dioxide gas. Balance the following equation: PbSO3 (s) → heat → PbO (s) + SO2 (g). (b) How many liters of SO2 are produced at 1 atm and 300 °C if 250 g of PbSO3 is decomposed?
Problem 81
Natural gas is a mixture of many substances, primarily CH4, C2H6, C3Hg, and C4H10. Assuming that the total pressure of the gases is 1.48 atm and that their mole ratio is 94:4.0:1.5:0.50, calculate the partial pressure in atmospheres of each gas.
Problem 82
A special gas mixture used in bacterial growth chambers contains 1.00% by weight CO2 and 99.0% O2. What is the partial pressure in atmospheres of each gas at a total pressure of 0.977 atm?
Problem 83
A gas mixture for use in some lasers contains 5.00% by weight HCl, 1.00% H2, and 94% Ne. The mixture is sold in cylinders that have a volume of 49.0 L and a pressure of 13,800 kPa at 210 °C. What is the partial pressure in kilopascals of each gas in the mixture?
Problem 84
What is the mole fraction of each gas in the mixture described in Problem 10.83?
Problem 85
A mixture of Ar and N2 gases has a density of 1.413 g/L at STP. What is the mole fraction of each gas?
Problem 86a
A mixture of 14.2 g of H₂ and 36.7 g of Ar is placed in a 100.0-L container at 290 K. (a) What is the partial pressure of H₂ in atmospheres?
Problem 86b
A mixture of 14.2 g of H₂ and 36.7 g of Ar is placed in a 100.0-L container at 290 K. (b) What is the partial pressure of Ar in atmospheres?
Problem 87
A 20.0-L flask contains 0.776 g of He and 3.61 g of CO2 at 300 K. (a) What is the partial pressure of He in mm Hg?
Problem 88
A sample of magnesium metal reacts with aqueous HCl to yield H2 gas: Mg1s2 + 2 HCl1aq2¡MgCl21aq2 + H21g2 The gas that forms is found to have a volume of 3.557 L at 25 °C and a pressure of 747 mm Hg. Assuming that the gas is saturated with water vapor at a partial pressure of 23.8 mm Hg, what is the partial pressure in millimeters of mercury of the H2? How many grams of magnesium metal were used in the reaction?
Problem 89a
Chlorine gas was first prepared in 1774 by the oxidation of NaCl with MnO₂: 2 NaCl(s) + 2 H₂SO₄(l) + MnO₂(s) → Na₂SO₄(s) + MnSO₄(s) + 2 H₂O(g) + Cl₂(g) Assume that the gas produced is saturated with water vapor at a partial pressure of 28.7 mm Hg and that it has a volume of 0.597 L at 27 °C and 755 mm Hg pressure. (a) What is the mole fraction of Cl₂ in the gas?
Problem 89b
Chlorine gas was first prepared in 1774 by the oxidation of NaCl with MnO₂: 2 NaCl(s) + 2 H₂SO₄(l) + MnO₂(s) → Na₂SO₄(s) + MnSO₄(s) + 2 H₂O(g) + Cl₂(g) Assume that the gas produced is saturated with water vapor at a partial pressure of 28.7 mm Hg and that it has a volume of 0.597 L at 27 °C and 755 mm Hg pressure. (b) How many grams of NaCl were used in the experiment, assuming complete reaction?
Problem 90a
Natural gas is a mixture of hydrocarbons, primarily methane 1CH42 and ethane 1C2H62. A typical mixture might have Xmethane = 0.915 and Xethane = 0.085. Let's assume that we have a 15.50 g sample of natural gas in a volume of 15.00 L at a temperature of 20.00 °C. (a) How many total moles of gas are in the sample?
Problem 90b
Natural gas is a mixture of hydrocarbons, primarily methane (CH₄) and ethane (C₂H₆). A typical mixture might have X_methane = 0.915 and X_ethane = 0.085. Let's assume that we have a 15.50 g sample of natural gas in a volume of 15.00 L at a temperature of 20.00 °C. (b) What is the pressure of the sample in atmospheres?
Problem 90c
Natural gas is a mixture of hydrocarbons, primarily methane (CH₄) and ethane (C₂H₆). A typical mixture might have X_methane = 0.915 and X_ethane = 0.085. Let's assume that we have a 15.50 g sample of natural gas in a volume of 15.00 L at a temperature of 20.00 °C. (c) What is the partial pressure of each component in the sample in atmospheres?
Problem 91a
Gaseous compound Q contains only xenon and oxygen. When 0.100 g of Q is placed in a 50.0-mL steel vessel at 0 °C the pressure is 0.229 atm. (a) What is the molar mass of Q, and what is a likely formula?
Problem 91b
Gaseous compound Q contains only xenon and oxygen. When 0.100 g of Q is placed in a 50.0-mL steel vessel at 0 °C the pressure is 0.229 atm. (b) When the vessel and its contents are warmed to 100 °C, Q decomposes into its constituent elements. What is the total pressure, and what are the partial pressures of xenon and oxygen in the container?
Problem 92
What are the basic assumptions of the kinetic–molecular theory?
Problem 93
What is the difference between heat and temperature?
Problem 94
The average temperature at an altitude of 20 km is 220 K. What is the average speed in m/s of an N2 molecule at this altitude?
Problem 95
Calculate the average speed of a nitrogen molecule in m/s on a hot day in summer 1T = 37 °C2 and on a cold day in winter 1T = -25 °C2.