Thermodynamics, Statistical Thermodynamics, & Kinetics
3rd Edition
ISBN: 9780321766182
Author: Thomas Engel, Philip Reid
Publisher: Prentice Hall
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Chapter 2, Problem 2.1NP
A 3.75 mole sample of an ideal gas with
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. A 2.50 mole sample of a perfect gas for which Cv,m = 3R/2 (assume constant over T-range) undergoes the following two-step process: (1) from an initial state of the gas described by T = 13 ºC and P = 1.75 x 105 Pa, the gas undergoes an isothermal expansion against a constant pressure of 3.75 x 104 Pa until the volume has doubled. (2) subsequently, the gas is cooled at constant volume. The temperature falls to -24ºC. Calculate q, w, ∆U, and ∆H for each step and for the overall process.
1. 0.1m3 of an ideal gas at 300 K and 1 bar is compressed adiabatically to 8 bar. It is then cooled at constant volume and further expanded isothermally so as to reach the condition from where it started.
Determine the following with aid of a NEAT DIAGRAM
a. Pressure at the end of constant volume cooling
b. Change in internal energy during the constant volume process
c. Net work done and heat transferred during the cycle.
Assume, Cp = 14.3 kJ/kgK and Cv = 10.2 kJ/kgK.
One mole of a monatomic ideal gas begins in a state withP 5 1.00 atm and T 5 300 K. It is expanded reversiblyand adiabatically until the volume has doubled; then it isexpanded irreversibly and isothermally into a vacuumuntil the volume has doubled again; and then it is heatedreversibly at constant volume to 400 K. Finally, it is compressed reversibly and isothermally until a inal state withP 5 1.00 atm and T 5 400 K is reached. Calculate DSsysfor this process. (Hint: There are two ways to solve thisproblem—an easy way and a hard way.)
Chapter 2 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
Ch. 2 - Electrical current is passed through a resistor...Ch. 2 - Two ideal gas systems undergo reversible expansion...Ch. 2 - You have a liquid and its gaseous form in...Ch. 2 - Prob. 2.4CPCh. 2 - For a constant pressure process, H=qp. Does it...Ch. 2 - A cup of water at 278 K (the system) is placed in...Ch. 2 - In the experiments shown in Figure 2.4a and 2.4b,...Ch. 2 - What is wrong with the following statement? Burns...Ch. 2 - Why is it incorrect to speak of the heat or work...Ch. 2 - You have a liquid and its gaseous form in...
Ch. 2 - Prob. 2.11CPCh. 2 - Explain how a mass of water in the surroundings...Ch. 2 - A chemical reaction occurs in a constant volume...Ch. 2 - Explain the relationship between the terms exact...Ch. 2 - In the experiment shown in Figure 2.4b, the weight...Ch. 2 - Discuss the following statement: If the...Ch. 2 - Discuss the following statement: Heating an object...Ch. 2 - An ideal gas is expanded reversibly and...Ch. 2 - An ideal gas is expanded reversibly and...Ch. 2 - An ideal gas is expanded adiabatically into a...Ch. 2 - Prob. 2.21CPCh. 2 - Prob. 2.22CPCh. 2 - A student gets up from her chair and pushes a...Ch. 2 - Explain why ethene has a higher value for CV,m at...Ch. 2 - Prob. 2.25CPCh. 2 - Prob. 2.26CPCh. 2 - A 3.75 mole sample of an ideal gas with Cv,m=3R/2...Ch. 2 - The temperature of 1.75 moles of an ideal gas...Ch. 2 - A 2.50 mole sample of an ideal gas, for which...Ch. 2 - A hiker caught in a thunderstorm loses heat when...Ch. 2 - Count Rumford observed that using cannon boring...Ch. 2 - A 1.50 mole sample of an ideal gas at 28.5C...Ch. 2 - Calculate q, w, U, and H if 2.25 mol of an ideal...Ch. 2 - Calculate w for the adiabatic expansion of 2.50...Ch. 2 - Prob. 2.9NPCh. 2 - A muscle fiber contracts by 3.5 cm and in doing so...Ch. 2 - A cylindrical vessel with rigid adiabatic walls is...Ch. 2 - In the reversible adiabatic expansion of 1.75 mol...Ch. 2 - A system consisting of 82.5 g of liquid water at...Ch. 2 - A 1.25 mole sample of an ideal gas is expanded...Ch. 2 - A bottle at 325 K contains an ideal gas at a...Ch. 2 - A 2.25 mole sample of an ideal gas with Cv,m=3R/2...Ch. 2 - Prob. 2.17NPCh. 2 - An ideal gas undergoes an expansion from the...Ch. 2 - An ideal gas described by Ti=275K,Pi=1.10bar, and...Ch. 2 - In an adiabatic compression of one mole of an...Ch. 2 - The heat capacity of solid lead oxide is given by...Ch. 2 - Prob. 2.22NPCh. 2 - Prob. 2.23NPCh. 2 - Prob. 2.24NPCh. 2 - Prob. 2.25NPCh. 2 - A 2.50 mol sample of an ideal gas for which...Ch. 2 - A 2.35 mole sample of an ideal gas, for which...Ch. 2 - Prob. 2.28NPCh. 2 - A nearly flat bicycle tire becomes noticeably...Ch. 2 - Prob. 2.30NPCh. 2 - Prob. 2.31NPCh. 2 - Consider the isothermal expansion of 2.35 mol of...Ch. 2 - An automobile tire contains air at 225103Pa at...Ch. 2 - One mole of an ideal gas is subjected to the...Ch. 2 - Prob. 2.35NPCh. 2 - A pellet of Zn of mass 31.2 g is dropped into a...Ch. 2 - Calculate H and U for the transformation of 2.50...Ch. 2 - A 1.75 mole sample of an ideal gas for which...Ch. 2 - Prob. 2.39NPCh. 2 - Prob. 2.40NPCh. 2 - The Youngs modulus (see Problem P2.40) of muscle...Ch. 2 - DNA can be modeled as an elastic rod that can be...Ch. 2 - Prob. 2.43NPCh. 2 - Prob. 2.44NP
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- oxygen is compressed polytropically in a cylinder from 1.5 bar, 15oC to 4.2bar in such a way that 1/3 of the work input is rejected as heat to the cylinder valves. Calculate final temperature of the gas. take Cv = 0.649 and m = 32 kgarrow_forward1) A sample containing 1.50 mol of an ideal gas with CV,m = 20.8 J K−1 mol−1isinitially at 230 kPa and 315 K. It undergoes a reversible adiabatic expansion until itspressure reaches 170 kPa. Calculate the final volume V2; the final temperature T2, andthe work w done by the system.arrow_forward1 mole of an ideal gas with CV,m = 5/2 R undergoes transformation either (I) or (II) from aninitial temperature (Ti) = 250 K and initial pressure (Pi) = 1.00 bar. CV,m denotes molar heatcapacity at constant volume.(I) 1 mol of gas undergoes a reversible adiabatic expansion until the final pressure (Pf) ishalf of its initial value. The surroundings are at 250 K and 0.500 bar.(II) 1 mol of gas undergoes an adiabatic expansion against a constant external pressure(Pex) of 0.500 bar until the final pressure (Pf) is equal to half of its initial value. Thesurroundings are at 300 K and 0.500 bar.a) Calculate the change in entropy of the system (ΔSsys) (in unit J K-1 ) for each (I) and (II). b) Calculate the change in entropy of the surroundings (ΔSsur) (in unit J K-1 ) for each (I) and (II). c) Calculate the total change in entropy (ΔStot) (in unit J K-1 ) for each (I) and (II). d) State which of the process [(I) or (II)] is a spontaneous process.arrow_forward
- Predict the output of energy as heat from the combustion of 1.0 dm3 of octane at 298 K and 1 bar. Its mass density is 0.703 g cm−3.arrow_forwardOne mol of an ideal gas is heated at a constant external pressure of 200 kPa. Calculate the enthalpy involved and change in internal energy during this process upon the temperature change from 100 oC to 25.0 oC. Molar specific heat capacity CV = 3/2 R and the universal gas constant is 8.3145 J‧mol-1·K-1.arrow_forwardA closed cylinder contains 1.0 mole of ideal monatomic gas at 300 oC and 4.0 bar.Insulating the cylinder so that there is no heat exchange with the surroundings, the gas isexpanded to 200 oC and 1.0 bar producing 1247 J of work.a) Is this process reversible or irreversible?b) What is the change in enthalpy (∆H) of the gas?c) What is the change in internal energy (∆U) of thegas?arrow_forward
- Consider one mole of a simple ideal gas enclosed in a cylindrical piston with rigid impermeable adiabatic walls. The piston has a cross sectional area ofA = 0.10 m^2 and the cylinder enclosing the gas has a height of h = 1.0 cm. The gas inside the piston has a temperature T = 300.K. Recall that the internal energy for an ideal gas is U= n cV,mT, where cV,m= 1.5 R is the molar heat capacity for the ideal gas. mass m = 15.3E3kg is placed on the top of the piston, but that the piston top remains rigid. The external pressure applied is 1.5E6 Pa. Determine the equilubrium volume for the gas.arrow_forwardConsider one mole of a simple ideal gas enclosed in a cylindrical piston with rigid impermeable adiabatic walls. The piston has a cross sectional area ofA = 0.10 m^2 and the cylinder enclosing the gas has a height of h = 1.0 cm. The gas inside the piston has a temperature T = 300.K. Recall that the internal energy for an ideal gas is U= n cV,mT, where cV,m= 1.5 R is the molar heat capacity for the ideal gas. mass m = 15.3E3kg is placed on the top of the piston, but that the piston top remains rigid. The external pressure applied is 1.5E6 Pa. The equilubrium volume for the gas is 1.6E-3 m^3. Suppose that the piston is now allowed to move within the cylinder, but that the walls remain adiabatic and impermeable so that no heat flows into the gas. The gas system will ultimately move to a new equilibrium state. We will now characterize the final equilibrium state and the changes resulting from the process. Define the (Total System) = (the gas enclosed in the cylinder) plus (the mass placed…arrow_forwardA 1.5 mol of perfect gas molecules with Cpm = 20.8) K-1 mol-1 is initially at 230 kPa and 315 K. It undergoes reversible adiabatic expansion until its pressure reaches 170 kPa. Calculate the final volume and temperature and the work donearrow_forward
- Can the variation of specific heat Cp with pressure at a given temperature be determined from a knowledge of P, V,T data alone? Explain your answer by any mathematical expression possible.arrow_forward1. A chemical reaction takes place in a container fitted with a piston of cross-sectional area 75.0 cm2 . As a result of the reaction, the piston is pushed out through 25.0 cm against an external pressure of 150 kPa. Calculate the work done by the system.arrow_forwardYou have a gas held isothermally at 297 K whose volume changes from 0.2 m^3 to 9.0 m^3, what is the change in internal energy? Use the fact that the internal pressure of this gas is approximately constant at 100 MPa under these conditions.arrow_forward
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