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[Hydrazine_Soup]

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Edited March 5, 2020 by Hydrazine_Soup

[Steel]

I'm pretty sure there's too little information given to solve the problem

[Hydrazine_Soup]

On 11/14/2016 at 11:55 PM, Steel said:

I'm pretty sure there's too little information given to solve the problem

I don't know what equations to use.

Edited March 5, 2020 by Hydrazine_Soup

[p1t1o]

[Spotted an error - Boltzmanns constant is measured in J/K not J/kg]

Molar volume of an ideal gas:

Vm = RT/p = volume of 1mole

And since you can work out the average energy of a particle, and we know that there are 6.023e23 particles in a mole, you can calculate the energy per unit volume and the energy per mole.

To get to energy per unit mass, I think you need to know something about the mass of the particles, at this point we know a bit about the amount of energy we have, but the mass present could be any value and still fit the data, the only thing that will change will be the velocity of the particles and we dont know that either.

Im loath to blame the question for missing a piece of data though, in my experience this usually means you missed something, which I easily could be doing, its been a while

 

[cfds]

In an ideal gas, p V=N k_B T holds true. Your total enthalpy is N 3/2 k_B T + p V = N 5/2 k_B T. Your enthalpy per particle is 5/2 k_B T

[p1t1o]

@danilon62 If you ever get to the bottom of this I hope you post here, Im dying to know!

[YNM]

Guess you can just use the usual internal energy :

E_int = (f/2)NkT

Then, by ideal gas law :

N = PV/kT

Substituting them gives

E_int = (f/2)PVT

Which, I hope, you have the volume information.

 

Also, heat != internal energy.

Edited November 17, 2016 by YNM