Thermodynamics, Statistical Thermodynamics, & Kinetics
3rd Edition
ISBN: 9780321766182
Author: Thomas Engel, Philip Reid
Publisher: Prentice Hall
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Textbook Question
Chapter 1, Problem 1.8CP
At sufficiently high temperatures, the van der Waals equation has the form
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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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- Use the approximation 1 x-1 1 x x2 to determine an expression for the virial coefficient C in terms of the van der Waals constants.arrow_forwardWhat is the van der Waals constant a for Ne in units of bar.cm6/mol2arrow_forwardA glass tumbler containing 243 cm3 of air at 1.00 102 kPa (the barometric pressure) and 20C is turned upside down and immersed in a body of water to a depth of 25.5 m. The air in the glass is compressed by the weight of water above it. Calculate the volume of air in the glass, assuming the temperature and barometric pressure have not changed.arrow_forward
- Gallium melts just above room temperature and is liquid overa very wide temperature range 130–2204 °C2, which means itwould be a suitable fluid for a high-temperature barometer.Given its density, dGa = 6.0 g>cm3, what would be the heightof the column if gallium is used as the barometer fluid andthe external pressure is 9.5 * 104 Pa?arrow_forwardIn a commonly used model of the atmosphere, the atmospheric pressure varies with altitude, h, according to the barometric formula:p = p0e–h/Hwhere p0 is the pressure at sea level and H is a constant approximately equal to 8 km. More specifically, H = RT/Mg, where M is the average molar mass of air and T is the temperature at the altitude h. This formula represents the outcome of the competition between the potential energy of the molecules in the gravitational field of the Earth and the stirring effects of thermal motion. Derive this relation by showing that the change in pressure dp for an infinitesimal change in altitude dh where the mass density is ρ is dp = −ρgdh. Remember that ρ depends on the pressure. Evaluate (a) the pressure difference between the top and bottom of a laboratory vessel of height 15 cm, and (b) the external atmospheric pressure at a typical cruising altitude of an aircraft (11 km) when the pressure at ground level is 1.0 atm.arrow_forwardThe virial equation of state may also be written as an expansion in terms of pressure: Z = 1 + B'p + ... The critical constants for water, H2O, are 218.3 atm. 55.3 cm3 mol-1 and 647.4 K. Assuming that the expansion may be truncated after the second term, calculate the value of the second virial coefficientB' at the critical temperature.arrow_forward
- Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g) How much MnO2(s) should be added to excess HCl(aq) to obtain 285 mL Cl2(g) at 25 °C and 95 kPa?arrow_forwardA sample of nitrogen initially at T = 25 oC and p = 4.0 atm triples its initial volume. What will be its final temperature and pressure if it expands reversibly adiabatically?arrow_forwardThe energy of the van der Waals bond, which is responsible for a number of the characteristics of water, is about 0.50 eV. (a) At what temperature would the average translational kinetic energy of water molecules be equal to this energy? (b) At that temperature, would water be liquid or gas? Under ordinary everyday conditions, do van der Waals forces play a role in the behavior of water?arrow_forward
- For an ideal gas obeying the ideal gas law, P = nRT/V , where R is the gas constant. Write the total differential dz and evaluate the partial derivativesarrow_forwardGallium melts just above room temperature and is liquid overa very wide temperature range (30–2204 °C), which means itwould be a suitable fluid for a high-temperature barometer.Given its density, dGa = 6.0 g/cm3, what would be the heightof the column if gallium is used as the barometer fluid andthe external pressure is 9.5 x104 Pa?arrow_forwardRearrange the van der Waals equation of state, p = nRT/(V − nb) − n2a/V2(Topic 1C) to give an expression for T as a function of p and V (with n constant). Calculate (∂T/∂p)V and confirm that (∂T/∂p)V = 1/(∂p/∂T)V.arrow_forward
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