Thermodynamics, Statistical Thermodynamics, & Kinetics
3rd Edition
ISBN: 9780321766182
Author: Thomas Engel, Philip Reid
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 1, Problem 1.17NP
Interpretation Introduction
Interpretation:The number of moles of the oxygen absorbed by the body of the athlete per minute needs to be determined.
Concept Introduction: The ideal gas equation is the equation which gives the relations between P,V, n and T of gases. It can be written as:
Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
A homeowner uses 4.00 × 103 m3 of natural gas in a year to heat a home. Assume that natural gas is all methane, CH4, and that methane is a perfect gas for the conditions of this problem, which are 1.00 atm and 20 °C. What is the mass of gas used?
Calculate the number of moles of air in the lungs assuming a capacity of 1.81 liters and a body temperature of 36.9ºC.
Gypsum (plaster of Paris : CaSO,. 2H,0) is produced by the reaction of calcium carbonate and sulfuric
acid. A certain lime stone analyzes: CaCO, 96.89 %; MgCO, 1.41 %; inerts 1.70 %. For 5 metric tons of limestone reacted completely, determine:
a. kg of anhydrous gypsum (CaSO,) produced. b. kg of sulfuric acid solution (98 wt%) required.
Chapter 1 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
Ch. 1 - Real walls are never totally adiabatic. Use your...Ch. 1 - The parameter a in the van der Waals equation is...Ch. 1 - Give an example based on molecule—molecule...Ch. 1 - Prob. 1.4CPCh. 1 - Prob. 1.5CPCh. 1 - The location of the boundary between the system...Ch. 1 - Prob. 1.7CPCh. 1 - At sufficiently high temperatures, the van der...Ch. 1 - Prob. 1.9CPCh. 1 - Prob. 1.10CP
Ch. 1 - Prob. 1.11CPCh. 1 - Prob. 1.12CPCh. 1 - Prob. 1.13CPCh. 1 - The mass of a He atom is less than that of an Ar...Ch. 1 - Prob. 1.15CPCh. 1 - Prob. 1.1NPCh. 1 - A compressed cylinder of gas contains 2.74103g of...Ch. 1 - Calculate the pressure exerted by Ar for a molar...Ch. 1 - A sample of propane C3H8 is placed in a closed...Ch. 1 - A gas sample is known to be a mixture of ethane...Ch. 1 - One liter of fully oxygenated blood can carry 0.18...Ch. 1 - Yeast and other organisms can convert glucose...Ch. 1 - A vessel contains 1.15 g liq H2O in equilibrium...Ch. 1 - Consider a 31.0 L sample of moist air at 60.C and...Ch. 1 - Prob. 1.10NPCh. 1 - Prob. 1.11NPCh. 1 - A rigid vessel of volume 0.400m3 containing H2 at...Ch. 1 - A mixture of oxygen and hydrogen is analyzed by...Ch. 1 - An athlete at high performance inhales 3.75L of...Ch. 1 - Devise a temperature scale, abbreviated G, for...Ch. 1 - Aerobic cells metabolize glucose in the...Ch. 1 - Prob. 1.17NPCh. 1 - A mixture of 2.10103g of O2, 3.88103mol of N2, and...Ch. 1 - Prob. 1.19NPCh. 1 - Prob. 1.20NPCh. 1 - An initial step in the biosynthesis of glucose...Ch. 1 - Prob. 1.22NPCh. 1 - Assume that air has a mean molar mass of 28.9gmol1...Ch. 1 - When Julius Caesar expired, his last exhalation...Ch. 1 - Calculate the number of molecules per m3 in an...Ch. 1 - Prob. 1.26NPCh. 1 - A mixture of H2 and NH3 has a volume of 139.0cm3...Ch. 1 - A sealed flask with a capacity of 1.22dm3 contains...Ch. 1 - A balloon filled with 11.50 L of Ar at 18.7C and 1...Ch. 1 - Carbon monoxide competes with oxygen for binding...Ch. 1 - The total pressure of a mixture of oxygen and...Ch. 1 - Suppose that you measured the product PV of 1 mol...Ch. 1 - Liquid N2 has a density of 875.4kgm3 at its normal...Ch. 1 - Calculate the volume of all gases evolved by the...Ch. 1 - Prob. 1.35NPCh. 1 - A glass bulb of volume 0.198 L contains 0.457 g of...Ch. 1 - Prob. 1.37NPCh. 1 - Prob. 1.38NPCh. 1 - Many processes such as the fabrication of...Ch. 1 - Rewrite the van der Waals equation using the molar...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- The compression ratio in an automobile engine is the ratio of the gas pressure at the end of the compression stroke to the pressure in the beginning. Assume that compression occurs at constant temperature. The total volume of the cylinder in an automobile is 350 cm3, and the displacement the reduction in volume during the compression stroke is 309 cm3. What is the compression ratio in that engine?arrow_forwardWhat is the value of FP for a sample of gas whose temperature is -33.0 C and volume is 0.0250 L? What temperature is required to change the volume to 66.9 cm3?arrow_forwardperform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.arrow_forward
- Exhaled air contains 74.5% N2, 15.7% O2, 3.6% CO2, and 6.2% H2O (mole percent). (a) Calculate the molar mass of exhaled air. (b) Calculate the density of exhaled air at 37C and 757 mm Hg and compare the value you obtained with that of ordinary air (MM=29.0g/mol) under the same conditions.arrow_forwardThe gas in the discharge cell of a laser contains (in mole percent) 11% CO2, 5.3% N2, and 84% He. (a) What is the molar mass of this mixture? (b) Calculate the density of this gas mixture at 32C and 758 mm Hg. (c) What is the ratio of the density of this gas to that of air (MM=29.0g/mol)at the same conditions?arrow_forwardWhen limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete — the lime absorbs CO2 from the air and turns back into hard, durable limestone. Suppose a limekiln of volume 300.L is pressurized with carbon dioxide gas to 15.5atm, and heated to 950.0°C. When the amount of CO2 has stopped changing, it is found that 1.79kg of CaCO3 have appeared. Calculate the pressure equilibrium constant Kp this experiment suggests for the equilibrium between CaCO3 and CaO at 950.0°C. Round your answer to 2 significant digits. Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for Kp does not match the accepted value.arrow_forward
- Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 899. liters per second of dioxygen are consumed when the reaction is run at 265.°C and the dioxygen is supplied at 0.23atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits.arrow_forwardNitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 985. liters per second of dioxygen are consumed when the reaction is run at 241. °C and the dioxygen is supplied at 0.29 atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.arrow_forwardNitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 602. liters per second of dioxygen are consumed when the reaction is run at 222.°C and the dioxygen is supplied at 0.83atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. =____kg/sarrow_forward
- A closed container, thermally insulated from the outside and with negligible heat capacity, contains N moles of oxygen (diatomic gas) and N moles of neon (monoatomic gas) initially at 350°C. In the same container are placed 10 grams of ice initially at 0°C. If the final temperature of the water, after melting, is 5°C, how many moles of each gas was in the container?arrow_forwardWhal mass of C3H8 gas is required (o fil a 25.0 L propane tank to 385 kPa at 28 °C? A. 18.2 g B. 145 g C. 36.5 g D. 170 g E. 41.3 garrow_forwardThe emission of NO2 by fossil fuel combustion can be prevented by injecting gaseous urea into the combustion mixture. The urea reduces NO (which oxidizes in air to form NO2) according to the reaction:2 CO(NH2)2( g) + 4 NO( g) + O2( g)------------->4 N2( g) + 2 CO2( g) + 4 H2O( g)Suppose that the exhaust stream of an automobile has a flow rate of 2.55 L/s at 655 K and contains a partial pressure of NO of 12.4 torr. What total mass of urea is necessary to react completely with the NO formed during 8.0 hours of driving?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage Learning
Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Introductory Chemistry: An Active Learning Approa...
Chemistry
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Cengage Learning
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning