Physics for Scientists and Engineers
6th Edition
ISBN: 9781429281843
Author: Tipler
Publisher: MAC HIGHER
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Chapter 19, Problem 85P
To determine
To show the explicitly that the entropy change is zero for quasi-static adiabatic expansion.
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1 Point i in Fig. 20-19 represents
the initial state of an ideal gas at
temperature T. Taking algebraic
signs into account, rank the entropy
changes that the gas undergoes as it
moves, successively and reversibly,
from point i to points a, b, c, and d,
greatest first.
T+AT
T-AT
Volume
Pressure
A mole of an ideal gas is compressed isothermally at 298K. If the gas is compressed from 1 atm to 10 atm irreversibly using an external pressure of 10 atm, calculate the (a) entropy change of the system and the (b) entropy change of the universe for the process in J K-1.
A sample consisting of n moles of an ideal gas undergoes a reversible isobaric expansion from volume Vi to volume 3Vi . Find the change in entropy of the gas by calculating ∫fi dQ/T, where dQ = nCP dT.
Chapter 19 Solutions
Physics for Scientists and Engineers
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- Two moles of a monatomic ideal gas such as oxygen is compressed adiabatically and reversibly from a state (3 atm, 5 L) to a state with a pressure of 4 atm. (a) Find the volume and temperature of the final state. (b) Find the temperature of the initial state. (c) Find work done by the gas in the process. (d) Find the change in internal energy in the process. Assume Cv=5R and Cp=Cv+R for the diatomic ideal gas in the conditions given.arrow_forwardIs it possible for a system to have an entropy change if it neither absorbs nor emits heat during a reversible? transition? What happens it the process is irreversible?arrow_forwardFind the work done in the quasi-static processes shown below. The states are given as (p, V) values for the points in the PV plane: 1 (3 atm, 4 L), 2 (3 atm, 6 L), 3 (5 atm, 4 L), 4 (2 atm, 6 L), 5 (4 atm, 2 L), 6 (5 atm, 5 L) and 7 (2 atm, 5 L).arrow_forward
- Assume a sample of an ideal gas is at room temperature. What action will necessarily make the entropy of the sample increase? (a) Transfer energy into it by heat. (b) Transfer energy into it irreversibly by heat. (c) Do work on it. (d) Increase either its temperature or its volume, without letting the other variable decrease. (e) None of those choices is correct.arrow_forwardIn an isochoric process, heat is added to 10 mol of monoatomic ideal gas whose temperature increases from 273 to 373 K. What is the entropy change of the gas?arrow_forward(a) infinitesimal amount of heat is added reversibly to a system. By combining the first and second laws, show that dU=TdSdW. (b) When heat is added to an ideal gas, its temperature and volume change from T1 and V1 to T2 and V2 . Show that the entropy change of n moles of the gas is given by S=CnvlnT2T1nRlnV2V1 .arrow_forward
- A cylinder contains 500 g of helium at 120 atm and 20 . The valve is leaky, and all the gas slowly escapes isothermally into the atmosphere. Use the results of the preceding problem to determine the resulting change in entropy of the universe.arrow_forwardDoes the entropy increase for a Carnot engine for each cycle?arrow_forwardAn ideal gas is taken from an initial temperature Ti to a higher final temperature Tf along two different reversible paths. Path A is at constant pressure, and path B is at constant volume. What is the relation between the entropy changes of the gas for these paths? (a) SA SB (b) SA = SB (c) SA SBarrow_forward
- A monatomic ideal gas undergoes a quasi-static process that is described by the function pV=p1+3(vv1) , where the stating state is (p1,v1) and the final state (p2,v2) . Assume the system consists of n moles of the gas in a container that can exchange heat with the environment and whose volume can change freely. (a) Evaluate the work done by the gas during the change in the state. (b) Find the change in internal energy of the gas. (c) Find the heat input to the gas during the change. (d) What ale initial and final temperatures?arrow_forwardWhat is the entropy S of this system at a given temperature T, asT→∞, and T→0. We expect the entropy S to be 0 at T= 0. Does entropy increase as the temperature T increases?arrow_forwardCompute the change in entropy for an ideal dry gas of mass M which is heated at constant volume from T 1 to T 2 . Take M = 1 kg, T 1 = 300 K and T 2 = 310 K.arrow_forward
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