How Does Heating Affect the Pressure of an Ideal Gas in a Movable Piston Setup?

AI Thread Summary
The discussion centers on the behavior of an ideal gas in a movable piston setup when heat is added. Initially, the pressure of the gas is calculated to be 1.0145x10^5 Pa using the formula P= Patm + W/A. After heating, it is argued that the pressure remains the same because the piston reaches a new equilibrium position after moving. The reasoning suggests that while temperature increases, the volume change due to the piston moving compensates, maintaining pressure. Overall, the key point is that the pressure of the ideal gas remains constant at equilibrium despite the addition of heat.
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Homework Statement


An ideal gas in a cylinder occupies a volume of 0.065 m3 at room temperature (T = 293 K). The gas is confined by a piston with a weight of 100 N and an area of 0.65 m2. The pressure above the piston is equal to one atmosphere (atm = 1.013x10^5 Pa). The piston is free to move up and down.
What is the pressure of the ideal gas?
After heat is added (piston moves up), What is the pressure of the ideal gas?


Homework Equations



P= Patm + W/A

The Attempt at a Solution



For the first question, I found the pressure to equal 1.0145x10^5 Pa by using the equation I provided [P=1.013x10^5 + (100/.65)]

Is that right?

For the second question I figured the pressure would be the same because after the heat is added, the piston moves initially and then is again fixed in equilibrium (not moving). If there was a net force caused from a larger internal or external pressure, the piston would continue moving. But, since it is in equilibrium the pressure would stay the same...? The pressure builds up when the temp is increased, but since the piston is pushed up and stops, the volume has been increased resulting in equilibrium.
 
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Good logic, your argument is right.

ehild
 
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