How Do You Calculate the Increase in Internal Energy for Neon in a Tank?

[PhysicStud01]

Homework Statement

Suppose that a tank contains 680 m3 of neon at an absolute pressure of 1.01x105 Pa. The temperature is changed from 293.2 to 294.3 K. What is the increase in the internal energy of the neon? [3.9x105 J]

Homework Equations

delta Q = delta U + delta W
pV = nRT

The Attempt at a Solution

there is no potential energy between them. all the kinetic of neon is kinetic since it is ideal gas
how do i find delta Q and delta W. should they be positve or negative?
i assume that an increase in temperature increases kinetic energy. so internal energy increase. delta U is positive?
can you please tell me how to proceed

 

[Chestermiller]

If the tank is rigid, what can you say about its change in volume? Given this, how much work is done on the surroundings?

Chet

 

[PhysicStud01]

If the tank is rigid, what can you say about its change in volume? Given this, how much work is done on the surroundings?

Chet

the volume won't change. but the pressure will.
i used P1 / T1 = P2 / T2 to find new pressure, then work = (delta p) V
but the answer was not correct

 

[Chestermiller]

the volume won't change. but the pressure will.
i used P1 / T1 = P2 / T2 to find new pressure, then work = (delta p) V
but the answer was not correct

Actually, if the volume doesn't change, zero work is done on the surroundings.

Irrespective of whether any work is done, what is the effect of temperature on the internal energy of an ideal gas? How many moles of neon are present in the tank?

Chet

 

[PhysicStud01]

Actually, if the volume doesn't change, zero work is done on the surroundings.

Irrespective of whether any work is done, what is the effect of temperature on the internal energy of an ideal gas?

Chet

internal energy increases since kinetic energy increases

 

[Chestermiller]

internal energy increases since kinetic energy increases

How many moles of neon are there in the tank? Quantitiatively (in terms of an algebraic equation), if the temperature of an ideal gas changes by ΔT, what is the change in the internal energy ΔU.

Chet

 

[PhysicStud01]

is it 1/2 k (delta T)?
i ca't obtain the answer with this too

 

[Chestermiller]

is it 1/2 k (delta T)?
i ca't obtain the answer with this too

Actually, it's 3/2 kΔT, and that's per molecule. What is the change in internal energy per mole? If you have n moles, what is ΔU? You still didn't tell me how many moles of neon are in the tank. You need this to determine the change in U. Do you know how to use the ideal gas law to calculate the number of moles in the tank?

Chet

 

[PhysicStud01]

Actually, it's 3/2 kΔT, and that's per molecule. What is the change in internal energy per mole? If you have n moles, what is ΔU? You still didn't tell me how many moles of neon are in the tank. You need this to determine the change in U. Do you know how to use the ideal gas law to calculate the number of moles in the tank?

Chet

from pV = nRT
but i don't know which temperature to use

 

[Chestermiller]

from pV = nRT
but i don't know which temperature to use

The number of moles in the tank doesn't change, and you're using the starting pressure and the starting volume in your calculation of the number of moles. So, does it make sense to you to use the final temperature or the starting temperature?

Chet

 

[PhysicStud01]

the starting one

 

[Chestermiller]

So how many moles of neon are there in the tank? And you still haven't answered my question about the algebraic relationship between ΔU and ΔT for n moles of an ideal gas.

Chet

 

[PhysicStud01]

So how many moles of neon are there in the tank? And you still haven't answered my question about the algebraic relationship between ΔU and ΔT for n moles of an ideal gas.

Chet

ok. thanks I got it.
but I still don't understand why work = (delta p) V cannot be used? if hte pressure changes, should not there be a work?

 

[Chestermiller]

Since when is work equal to distance times the change in force?

Chet