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Physics 7A F15 Exit Handout from DLM 15 FNTs 4.1.4-1) Complete
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Its question 4.2.1-2 on the attachment

This question refers to a process involving three moles of a diatomic gas (which behaves as an ideal gas, but as is typical near room temperature,with vibrational modes frozen out). The PV curve at right describes this process. Determine the energy transferred as work, the change in internal energy, and the energy transferred as heat in this process.

 In the PV diagram they give P initial as 60 Pa x 105 and P final as 55 Pa x 105. Temp initial is 337K and Temp final is 353K. Vol initial is 1.4 m3 x 10-3 and Vol final is 1.6 m3 x 10-3.

I know that delta E = Q+W and here Q+W cant be 0 because the heat entering the system changed the temperature and caused work to be done on the gas I believe. 


So I have been trying to figure this out for a while and I don't think I understand this topic very well. In my notes form lecture I have multiple equation about finding work and I'm not sure which one to use.  To solve for the internal energy change do I use the equation n*Cv*deltaT or do I multiply the change in pressure by the change in temperature? 




Physics 7A F15

 


 

Exit Handout

 


 

from DLM 15

 


 

FNTs

 

4.1.4-1) Complete Activity 4.1.4; Parts A3, A4, B5, and B6

 

4.1.1-5) Is it possible for an ideal gas to undergo an isobaric process in which ?U = 0? If so, sketch a

 

PV diagram for such a process.

 


 

4.2.1-2) Using multiple models simultaneously: This FNT refers

 

to a process involving three moles of a diatomic gas (which

 

behaves as an ideal gas, but as is typical near room temperature,

 

with vibrational modes frozen out). The PV curve at right

 

describes this process.

 


 

P [Pa × 10 5 ]

 


 

4.2.1-1) Use your results from Activity 4.2.1 to determine a value of the heat of vaporization of one

 

mole of water at 30?C and standard atmospheric pressure.

 

T = 337K

 

60.0

 


 

55.0

 

T = 353K

 


 

Determine the energy transferred as work, the change in internal

 

energy, and the energy transferred as heat in this process.

 


 

1.4

 

1.6

 

3

 

V [m × 10 -3 ]

 


 

P (Pa x 10 )

 


 

4.2.1-3

 

One mole of an unknown ideal gas (monatomic? diatomic? could be any number of

 

atoms in each molecule) completes a cyclic process shown in the

 

PV diagram at right.

 

5

 


 

a) What is the magnitude of the work done on the gas over one

 

complete cycle (I to II to III to I)? (Hint: think of this cycle as

 

three separate pieces that are summed-over to get the

 

complete cycle.)

 


 

3.0

 


 

b) What is the net change in internal energy of the gas over one

 

complete cycle? Explain how you determined this.

 


 

I

 


 

III

 


 

2.0

 

6.0

 

3

 

V (m x 10-3)

 


 

P [Pa × 10 5]

 


 

c) During the portion of the process going directly between points

 

III and I, 3000J of heat was removed. Using this information

 

determine whether this gas is monatomic diatomic, or what,

 

and explain the steps you used to determine this.

 


 

4.2.1-4) Two different processes (A) I to IIa to III,

 

and (B) I to IIb to III can take a mole of an ideal monatomic gas

 

from an initial state I to a final state III.

 

a) How much work is done on/by the gas in each step of both

 

processes (A) and (B)?

 

b) How much energy is transferred as heat to/from the gas in

 

each step of both process (A) and (B)?

 


 

II

 


 

8.0

 


 

4.0

 


 

2.0

 


 

III

 


 

IIa

 


 

IIb

 


 

I

 


 

(B)

 

5.0

 

10.0

 

V [m3 × 10 -3 ]

 


 

(A)

 


 

 







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