Thermodynamics, Statistical Thermodynamics, & Kinetics
3rd Edition
ISBN: 9780321766182
Author: Thomas Engel, Philip Reid
Publisher: Prentice Hall
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Chapter 5, Problem 5.43NP
An ideal gas sample containing 1.75 moles for which
- It is expanded reversibly and adiabatically until the volume triples.
- It is reversibly heated at constant volume until T increases to 275 K.
- The pressure is increased in an isothermal reversible compression until
Calculate q, w,
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1) Consider a system consisting of 1.5 mol CO2 (g), initially at 15°C and 9.0 atm and confined to a cylinder of cross-section 100.0 cm2 , The sample is allowed to expand adiabatically against an external pressure of 1.5 atm until the piston has moved outwards through 15 cm. Assume that carbon dioxide may be considered a perfect gas with CV,m = 28.8 J K-l mol-1 , and calculate;
(a) q,
(b) w,
(c) ∆U,
(d) ∆T,
(e) ∆S.
Suppose that attractions are the dominant interaction between gas molecules, and the equation of state is p = nRT/V – n2a/V2.
Determine the work (W(non-ideal gas)) of reversible, isothermal expansion of such a gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol, T = 300 K, and a = 3.621 atm-L2/mol2. Watch your units.
Determine the work (W(ideal gas) of reversible, isothermal expansion of an ideal gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol and T = 300 K.
Show the difference W(non-ideal) – W(ideal). If all your calculations are done correctly, this result shows you the effect of attractive interaction between gas particles on the work done by the system.
A 1.65 mole sample of an ideal gas for which Cv, m = 3/2 R undergoes the following two-step process: (a) From an initial state of the gas described by T = 14.5 oC and P = 2x104 Pa, the gas undergoes isothermal expansion against a constant external pressure of 1.0x104 Pa until the volume has doubled. (b) Then the gas is cooled to constant volume. The temperature drops to -35.6 oC. Calculate q, w, ΔH, ΔU for each step and for the overall process.
Chapter 5 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
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- gas undergoes an adiabatic expansion from 10 − 3 m 3 to 8 × 10 − 3 m 3 . The adiabatic line for the gas is given by P 3 V 5 = C (C is a constant). (a) Calculate the reversible work performed along the adiabatic line if the initial pressure is 10 5 P a and the initial volume = 10 − 3 m 3 . (b) What is the value of the constant C ? What is the unit of C ? (c) The gas reaches the final state in a two step process. An expansion at a constant initial pressure to the final volume followed by a decrease in pressure to the final volume 8 × 10 − 3 m 3 . What is the reversible work and heat in this process?arrow_forwardA sample consisting of 2.80 mol of diatomic perfect gas molecules at 250 K is compressed adiabatically until its temperature reaches 300 K. Given that Cy= 27.5 J K-1 mol-1, calculate q, w, AU, AH, and AS.arrow_forwardConsider a system consisting of 1.5 mol CO2 (g), initially at 15 C and 9.0 atm and confined to a cylinder of cross-section 100.0 cm², The sample is allowed to expand adiabatically against an external pressure of 1.5 atm until the piston has moved outwards through 15 cm. Assume that carbon dioxide may be considered a perfect gas with Cr,m = 28.8 J K'mol', and calculate (a) q, (b) w, (c) AU, (d) AT, (e) AS.arrow_forward
- The molar heat capacity of oxygen at constant pressure can be expressed as follows: Cp,m = a + bT, where a = 6.15 cal mol-1 K-1and b = 0.0031 cal mol-1 K-2. a) 2 mols of oxygen have been heated up reversibly from 27 ºC to 127 ºC, at a constant pressure of 1 atm. Calculate the w, q, ΔU and ΔH of the process. b) Same thing, assuming an isocoric process. The oxygen behaves as an ideal gas.arrow_forwarda) Suppose that attractions are the dominant interaction between gas molecules, and the equation of state is p = nRT/V – n2a/V2. Determine the work (W(non-ideal gas)) of reversible, isothermal expansion of such a gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol, T = 300 K, and a = 3.621 atm-L2/mol2. Watch your units. (b) Determine the work (W(ideal gas) of reversible, isothermal expansion of an ideal gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol and T = 300 K. (c) Show the difference W(non-ideal) – W(ideal). If all your calculations are done correctly, this result shows you the effect of attractive interaction between gas particles on the work done by the system.arrow_forwardThe constant-volume heat capacity of a gas can be measured by observing the decrease in temperature when it expands adiabatically and reversibly. The value of γ = Cp/CV can be inferred if the decrease in pressure is also measured and the constant-pressure heat capacity deduced by combining the two values. A fluorocarbon gas was allowed to expand reversibly and adiabatically to twice its volume; as a result, the temperature fell from 298.15 K to 248.44 K and its pressure fell from 202.94 kPa to 81.840 kPa. Evaluate Cp and Cvarrow_forward
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