Thermodynamics, Statistical Thermodynamics, & Kinetics
3rd Edition
ISBN: 9780321766182
Author: Thomas Engel, Philip Reid
Publisher: Prentice Hall
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Chapter 1, Problem 1.32NP
Suppose that you measured the product PV of 1 mol of a dilute gas and found that
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For many purposes we can treat propane (C₂H) as an ideal gas at temperatures above its boiling point of −42. °C.
Suppose the temperature of a sample of propane gas is raised from 17.0 °C to 32.0 °C, and at the same time the pressure is decreased by 5.0%.
Does the volume of the sample increase, decrease, or stay the same?
If you said the volume increases or decreases, calculate the percentage change in
the volume. Round your answer to the nearest percent.
increase
decrease
stays the same
%
x10
X
Ś
?
18
Ar
For many purposes we can treat butane (C,H10)
as an ideal gas at temperatures above its boiling point of – 1. °C.
3
Suppose the pressure on a 8.0 m° sample of butane gas at 11.0°C is reduced to one-third its initial value.
O yes
Is it possible to change the temperature of the butane at the same time such that
the volume of the gas doesn't change?
olo
O no
If you answered yes, calculate the new temperature of the gas. Round your
answer to the nearest °C.
Explanation
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An experiment was done to determine the value of the ideal gas constant (R). Hydrogen gas was generated and collected at a given temperature and pressure. 1.44 x 10-3 moles of hydrogen gas occupied 35.9 mL at 758.0 mmHg and 23.2 oC. Based on these values, calculate the experimentally determine value of R (L⋅⋅atm/mol⋅⋅K).
Using the unrounded number from the previous problem, determine the percent error for the experimentally determined value of R.
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...
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- At the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove this statement by calculating the density of an ideal gas in g/cm3 at the conditions of the critical point and comparing it with the experimental value. Compute the experimental value from the fact that a mole of CO2 at its critical point occupies 94 cm3.arrow_forwardA 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.arrow_forwardWhich of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substancearrow_forward
- A 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_forward5-107 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?arrow_forwardThe sudden appearance of hot gaseous products in a small initial volumeleads to rapid increases in pressure and temperature, which give the rocketits thrust. What total pressure of gas would be produced at 800°C by igniting 7.00 × 105 kg NH4ClO4 (a typical charge of the booster rockets in the space shuttle) and allowing it to expand to fill a volume of 6400 m3 (6.40 × 106L)? Use the ideal gas lawarrow_forward
- 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?arrow_forwardWhile ethanol CH3CH2OH is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene CH2CH2 with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 2.0L flask at 21.°C with 5.0atm of ethylene gas and 4.2atm of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains 3.7atm of ethylene gas and 2.9atm of water vapor. The engineer then adds another 1.7atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.arrow_forwardConsider the following situation: You have a 50 L tank of compressed air at 15 atm and 100 ºC. You then pass the compressed air through a "titanium getter" which contains fragments of hot titanium metal. The purpose of the "getter" is to remove oxygen gas from the sample as Ti reacts with oxygen to form solid TiO2 (known as titania). Once the purified air is passed through the getter is it cooled back down to 100 ºC and fills another 50 L storage tank. If air typically contains about 20% oxygen, what could the pressure in the storage tank be? Question 2 options: A) 12 atm B) 15 atm C) 18 atm D) 24 atmarrow_forward
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