Question

In answering this set of nine questions, you are encouraged to
draw a PV diagram, with P (pressure) on the y axis and V (volume)
on the x axis. Plot the three points A, B, and C on this
diagram.

1. Consider **10.0** liters of an ideal (monatomic)
gas at a pressure of **33.0** atm and a temperature of
**326** K. Call this state of the system A. Using the
ideal gas law, calculate the number of moles of gas present in the
system.

Number of moles, n =

2. The temperature of the system is reduced, keeping the volume
constant at **10.0** liters, until the pressure in the
system equals **13.0**. Call this state of the system
B. Calculate the temperature at this new state B in degrees
K.

Temperature at state B =

3. Now the gas is allowed to expand at constant pressure
(**13.0** atm) until the temperature is again equal to
**326** K. Call this state of the system C. Calculate
the volume of the gas at state C.

Volume at state C =

4. Now calculate the work done on or by the system when the system
moves back from state C to state A along the path CBA. Enter your
answer in joules with the correct sign.

Work along the path CBA, w =

5. Calculate the heat absorbed or liberated by the system when the
system moves from state C to state B. Note that the molar heat
capacity of an ideal gas under constant pressure is (5/2)R. Enter
your answer in joules with the correct sign.

Heat along the path C to B, q =

6. Using your results from the previous two questions, calculate
the heat absorbed or liberated by the system as it moves from state
B to state A. Enter your answer in joules with the correct
sign.

Heat along the path B to A, q =

7. What is the change in the internal energy of the system as the
system travels down the isotherm from state A to state C?

Change in internal energy down the isotherm =

8. How much work is done by the system as the system travels down
the isotherm from state A to state C? Enter your answer in joules
with the correct sign.

Work down the isotherm, w =

9. How much heat must be absorbed or liberated by the system as it
moves down the isotherm from A to C? Enter your answer in joules
with the correct sign.

Heat down the isotherm, q =

I got until number 3. I got 13.88 for #1, 175.51K for #2 and 20L for #3. May I ask for a help for rest of the problems?

Answer #1

1. moles, n=13.88

2. temp at B= 175.51 K

3. Volume at C= 20L

4. At A, P=33.0 atm, V=10 L, T=326 K

At B, P=13.0 atm, V=10 L, T=175.51 K

At C, P=13.0 atm, V=20 L, T=326 K

From C-B, w= P*(Vf-Vi)= (13 atm*101325 Pa/atm)*10= 1.31*10^7 J

From B-A, w= V*(P1-P2)= 10*(20atm*101325 Pa/atm)= 2.02*10^7 J

Total work from Cto B= 1.31*10^7+ 2.02*10^7= 3.33*10^7 J

5. Heat Cto B, q=mc(T2-T1)

Assuming the density to be 1

q=(20-10)*5/2*8.314(326-175.51)= 10*5/2*8.314*150.49

q= 31279.35 J

6. Heat from B to A, w= -P*delta V= -13(10-10)= 0 J

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