An Introduction to Thermal Physics
1st Edition
ISBN: 9780201380279
Author: Daniel V. Schroeder
Publisher: Addison Wesley
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Textbook Question
Chapter 4.2, Problem 12P
Explain why an ideal gas taken around a rectangular PV cycle, as considered in Problems 1.34 and 4.1, cannot be used (in reverse) for refrigeration.
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A 2 mole sample ideal gas is confined in a cylinder that is carried through a closed cycle. The gas is initially at 63 atm. First, its
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3 P;
Isothermal
C
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Problem #2
For heat exchange between a thermal reservoir at 300 K and a constant volume system
containing one mole of monatomic ideal gas:
a) Derive the equation for the total change in entropy for a designed initial system
temperature Tj.
b) Plot AStotal vs. Tsys for the initial system temperature ranging from 160 K to 500 K in
increments of 10 K (i.e., Tsys = 160 K, 170 K, ... , 500 K). Use Matlab, Excel or similar
plotting software for your plot. Label the plot axes and include units.
%D
Thermodynamics
Answer the following with complete solutions. write legibly.
A Carnot engine has an efficiency of 30%. Its efficiency is to be increased to 50%. By what must the temperature of the source be increased if the sink is at 300 K?
Chapter 4 Solutions
An Introduction to Thermal Physics
Ch. 4.1 - Prob. 1PCh. 4.1 - At a power plant that produces 1 GW ( 109 watts)...Ch. 4.1 - A power plant produces 1 GW of electricity, at an...Ch. 4.1 - It has been proposed to use the thermal gradient...Ch. 4.1 - Prove directly (by calculating the heat taken in...Ch. 4.1 - To get more than an infinitesimal amount of work...Ch. 4.2 - Why must you put an air conditioner in the window...Ch. 4.2 - Can you cool off your kitchen by leaving the...Ch. 4.2 - Prob. 9PCh. 4.2 - Suppose that heat leaks into your kitchen...
Ch. 4.2 - What is the maximum possible COP for a cyclic...Ch. 4.2 - Explain why an ideal gas taken around a...Ch. 4.2 - Under many conditions, the rate at which heat...Ch. 4.2 - Prob. 14PCh. 4.2 - In an absorption refrigerator the energy driving...Ch. 4.2 - Prob. 16PCh. 4.2 - Prob. 17PCh. 4.3 - Prob. 18PCh. 4.3 - The amount of work done by each stroke of an...Ch. 4.3 - Derive a formula for the efficiency of the Diesel...Ch. 4.3 - The ingenious Stirling engine is a true heat...Ch. 4.3 - A small-scale steam engine might operate between...Ch. 4.3 - Prob. 23PCh. 4.3 - Calculate the efficiency of a Rankine cycle that...Ch. 4.3 - In a real turbine, the entropy of the steam will...Ch. 4.3 - A coal-fired power plant, with parameters similar...Ch. 4.3 - In Table 4.1, why does the entropy of water...Ch. 4.3 - Imagine that your dog has eaten the portion of...Ch. 4.4 - Liquid HFC-134a at its boiling point at 12 bars...Ch. 4.4 - Consider a household refrigerator that uses...Ch. 4.4 - Suppose that the throttling valve in the...Ch. 4.4 - Suppose you are told to design a household air...Ch. 4.4 - Prob. 33PCh. 4.4 - Consider an ideal Hampson-Linde cycle in which no...Ch. 4.4 - The magnetic field created by a dipole has a...Ch. 4.4 - Prob. 36PCh. 4.4 - A common (but imprecise) way of stating the third...
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- An ideal gas initially at pressure P0, volume V0, and temperature T0 is taken through the cycle described in the figure below. (Assume n=4 and m=7). (a) Find the net work done by the gas per cycle in terms of P0 and V0. (Substitute numeric values for n and m, do not use the variables n and m.)Wenv = (b) What is the net energy Q added to the system per cycle? (Use the following as necessary: P0 and V0.)Q = (c) Obtain a numerical value for the net work done per cycle for 1.00 mol of gas initially at 0°C. Hint: Recall that the work done by the system equals the area under a PV curve. In kj.arrow_forwardA monatomic ideal gas initially has a temperature of 330k and preassure of 3x105 Pa. The gas expands from a volume of 500cm3 to a volume of 1500cm3. Calculate the work done by the gas (in Joules) if the expansion is isothermal. Calculate the change in internal energy (in Joules), if the expansion is adiabatic. I know that the first two questions have the same results, but, why the work equals the change in internal energy? I know that in adiabatic expansion the work done equals the change in internal energy(which is negative). To calculate the work I could use the same formula as the first question, so, is that the reason for they to be equal? I was trying to calculate the result for the last question using the formula Δu = g/2*n*r*Δt, so, how can I find the change in internal energy considering this fomula and get to the same result?arrow_forwardAn ideal gas initially at P, V, and T, is taken through a cydle as shown below. (Let the factor n - 3.3.) P B P, V. (a) Find the net work done on the gas per cycle for 2.45 mol of gas initially at 0°C. kJ (b) What is the net energy added by heat to the system per cycle?arrow_forward
- In a heat engine, 2.00 mol of a diatomic gas are carried through the cycle ABCDA, shown in Figure. (The PV diagram is not drawn to scale.) The segment AB represents an isothermal expansion, and the segment BC is an adiabatic expansion. The pressure and temperature at A are 5.00 atm and 600 K. The volume at B is twice the volume at A. The pressure at D is 1.00 atm. A) What is the pressure at B? B) What is the temperature at C? C) Find the total work done by the gas in one cycle.arrow_forwardIn a heat engine, 2.00 mol of a diatomic gas are carried through the cycle ABCDA, shown in Figure. (The PV diagram is not drawn to scale.) The segment AB represents an isothermal expansion, and the segment BC is an adiabatic expansion. The pressure and temperature at A are 5.00 atm and 600 K. The volume at B is twice the volume at A. The pressure at D is 1.00 atm.A) What is the pressure at B?B) What is the temperature at C?C) Find the total work done by the gas in one cycle.arrow_forwardAn ideal monatomic gas is contained in a cylinder with a movable piston so that the gas can do work on the outside world, and heat can be added or removed as necessary. (Figure 1) shows various paths that the gas might take in expanding from an initial state whose pressure, volume, and temperature are po, Vo, and To respectively. The gas expands to a state with final volume 4V. For some answers it will be convenient to generalize your results by using the variable R₂ = Vfinal/Vinitial, which is the ratio of final to initial volumes (equal to 4 for the expansions shown in the figure.) The figure shows several possible paths of the system in the pV plane. Although there are an infinite number of paths possible, several of those shown are special because one of their state variables remains constant during the expansion. These have the following names: Adiabatic: No heat is added or removed during the expansion. • Isobaric: The pressure remains constant during the expansion. ● •…arrow_forward
- SP 2P AT Q1 Q= 6 D 2V, Q A 1.00-mol sample of a monatomic ideal gas is taken through the cycle shown. At point A, the pressure, volume, and temperature are P₁ = 0.6 atm, V₁ = 1.8 m³, and T₁, respectively. Find the efficiency of an engine operating in this cycle. Write your efficiency in decimal form and round your answer to the nearest hundredth (i.e. if your efficiency is 0.867, round it to 0.87). Take 1 atm = 101300 Pa.arrow_forwardThe attached images have 3 parts, solve those 3 parts and also because of limited images to upload, this is the 4th part, iam typing here: Calculate the total change in entropy for entire system, in J/K.arrow_forwardAn ideal monatomic gas is contained in a cylinder with a movable piston so that the gas can do work on the outside world, and heat can be added or removed as necessary. (Figure 1) shows various paths that the gas might take in expanding from an initial state whose pressure, volume, and temperature are po, Vo, and To respectively. The gas expands to a state with final volume 4V. For some answers it will be convenient to generalize your results by using the variable R₂ = Vfinal/Vinitial, which is the ratio of final to initial volumes (equal to 4 for the expansions shown in the figure.) The figure shows several possible paths of the system in the pV plane. Although there are an infinite number of paths possible, several of those shown are special because one of their state variables remains constant during the expansion. These have the following names: Adiabatic: No heat is added or removed during the expansion. ● Isobaric: The pressure remains constant during the expansion. ● •…arrow_forward
- Now, let's use this property of logarithms to learn something about the number of microstates available to a molecular system. The absolute entropy of a system is related to the number of microstates available to it via Boltzmann's formula S = kB In W. If a system containing one mole of an ideal gas has an entropy of 167.7 J/K, how many microstates does it have? Report the order of W, as we have defined it above, and you should use scientific notation, 1.23E45, and report 3 (three) significant figures.arrow_forwardAn ideal gas initially at pi,vi, and ti is taken through a cycle as shown below. (Let the factor n=4.0. Note, this is the factor by which volume and pressure increases, NOT the number of moles of gas. )arrow_forwardOne mole of an ideal monoatomic gas is put through a cycle consisting of the following reversible steps: Isothermal compression from 2 atm and 10 L to 20 atm and 1 L Isobaric expansion to return the gas to the original volume of 10 L Cooling at constant volume to bring the gas to the original pressure and temperature. Illustrate the steps on a P-V curve. Calculate q, w, ΔU, ΔH, and ΔS for each step and for the cycle.arrow_forward
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