Thermodynamic constant volume process

In summary: Q = nCvΔT, where n is the number of moles, Cv is the molar specific heat at constant volume, and ΔT is the change in temperature. Since the process is constant volume, there is no work done (W = 0). Therefore, the increase in internal energy (ΔU) is equal to the heat flow (Q). Using the ideal gas law, PV = nRT, you can solve for the final temperature (Tf) by rearranging the equation to Tf = (Q/nCv) + Ti, where Ti is the initial temperature. In summary, in a constant-volume process, 208 J of energy is
  • #1
keevenh
1
0

Homework Statement



In a constant-volume process, 208 J of energy is transferred by heat to 0.99 mol of an ideal monatomic gas initially at 290 K.
(a) Find the work done on the gas.

(b) Find the increase in internal energy of the gas.

(c) Find its final temperature.

I just don't know which equation to use and don't really know which direction to take.

Homework Equations



Pretty sure it involves ΔU=W+Q

The Attempt at a Solution


NIL
 
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  • #2
Start by drawing a PV diagram of the process.

The work done is the area under the P-V curve.
The equations you want are the ideal gas law, something to relate internal energy to work and heat, and something to relate change in internal energy to temperature in a constant volume process.
 
  • #3
keevenh said:

Homework Statement



In a constant-volume process, 208 J of energy is transferred by heat to 0.99 mol of an ideal monatomic gas initially at 290 K.
(a) Find the work done on the gas.

(b) Find the increase in internal energy of the gas.

(c) Find its final temperature.

I just don't know which equation to use and don't really know which direction to take.

Homework Equations



Pretty sure it involves ΔU=W+Q
Is there any work done? Plug that value into your equation.

Can you find the heat flow, Q? Plug that into your equation.

That will give you the change in internal energy.

How is Q related to change in temperature? (think: heat capacity of the gas).

AM
 

FAQ: Thermodynamic constant volume process

What is a thermodynamic constant volume process?

A thermodynamic constant volume process is a type of thermodynamic process in which the volume of a system remains constant throughout. This means that no work is done on or by the system, and all changes in energy are due to heat transfer.

How is a constant volume process different from other thermodynamic processes?

A constant volume process is different from other thermodynamic processes, such as constant pressure or adiabatic processes, because the volume of the system remains constant. This means that the pressure and temperature of the system can change, but the volume will not.

What is the equation for calculating the change in internal energy during a constant volume process?

The equation for calculating the change in internal energy during a constant volume process is ΔU = Q, where ΔU is the change in internal energy and Q is the heat transferred to the system.

How is a constant volume process represented on a thermodynamic diagram?

A constant volume process is represented on a thermodynamic diagram as a vertical line, as the volume remains constant while the pressure and temperature may change.

What are some real-world examples of constant volume processes?

Some real-world examples of constant volume processes include the heating of a closed container, where the volume of the container remains constant as the temperature inside increases, and the combustion of fuel in an internal combustion engine, where the volume of the cylinder remains constant as the fuel is ignited and expands to do work.

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