3 THE FIRST AND SECOND LAWSOne mole of an ideal gas (c₁ = × R) at T = 325.0 K and p = 3.00 bar undergoes the followingprocesses -(1) A reversible adiabatic expansion until the final pressure is half its initial pressure.(2) Following the process in (1) the gas is further expanded irreversibly against an external psure of 0.500 bar while keeping the temperature constant.For the individual processes (1) and (2) calculate -(a) q(b) w(c) AU(d) AH(e) AS (for system, surroundings and totab

Let's break down the problem step by step:Given data:T1=325.0KP1=3.00barCv=25Rn=1moleFor an…

Answered: 3 THE FIRST AND SECOND LAWS One mole of…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter1: Gases And The Zeroth Law Of Thermodynamics

Section: Chapter Questions

Problem 1.64E: Show that = T/p for an ideal gas.

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(c) An ideal monoatomic gas at 1 bar and 300 K is expanded adiabatically against a constant pressure of 0.5 bar until the final pressure is 0.5 bar. Given that the Cy is 1.5R, calculate (i) (ii) heat per mole. work per mole.
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.
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.)

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