(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

An ideal gas undergoes a reversible process 1-2-3-4-5. The stage from 1-2 as well as isobaric 2-3 and isochoric 4-5 stages are represented by linear segments. The Stage 2-3 is isothermal. The following relations are true:

V_2=2*V_1

p_2=1.5*p_1

V_3=4*V_1

V_4=6*V_1

T_5=T_1

The initial states are V_1=3m^3 and p_1 = 2.5 atm.

Assuming that the internal energy of an ideal gas depends only on temperature, find the total heat recieved by the gas during the entire process also find change in enthalpy (H_1-H_5).

2. Relevant equations

pv=nRT

dw=p(v)dv

dw=pdv (isobaric)

dw=nRT*ln(v_f-v_i) isothermic

Q=U+W

H=U+pV

U=n*c_v*T+n*u_0 *****

3. The attempt at a solution

So far I have calculated all the pressures and volumes for all points (in atm and m^3):

P_1=3

V_1=2.5

p_2=3.75

V_2=6

p_3=1.875

V_3=12

p_4=1.875

V_4=18

p_5=5/12

V_5=18

After that I started trying to find either n or T, but I am guessing the point of the problem is to solve it without those. So moving on to find Q total, I noticed that without T, this problem involves at least 4 unknowns. So my troubles come in calculating the work from 1-2 since pressure is non constant and not any special type of process, and from eliminating n and T from the equation for q total.

****This is also the chapter in the book before we talk about the energy of an ideal gas, so I am assuming that we are not to use that equation, but just in case there it is.

1. The problem statement, all variables and given/known data

2. Relevant equations

3. The attempt at a solution

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# Homework Help: Ideal Gas Under A (Complex) Reversible Process

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