A cylinde with a piston in contact with a heat reservoir at 353 k.

AI Thread Summary
The discussion revolves around calculating the heat absorbed by a gas in a cylinder with a piston at a constant temperature of 353 K and pressure of 1.01 x 10^5 N/m², as the gas expands by 1.5E-5 m³. The initial suggestion is to use the formula p x v = w, leading to a calculated work of 1.15 J, but there is uncertainty about the role of temperature in the calculations. It is clarified that the temperature is essential for determining the number of moles of gas and other related factors, although the primary calculation focuses on work done at constant pressure. The conversation highlights the importance of understanding the relationship between pressure, volume, and heat in thermodynamic processes. Overall, the calculations appear correct as long as the assumptions about constant pressure and temperature hold true.
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A cylinde with a piston in contact with a heat reservoir at 353 k. While keeping this gas at constant temp and pressure of 1.01 x 10E5 n/m2 we permit he gas to expand by 1.5E-5 m3. How much heat does the gas absorb?

Is it just p x v = w and w = q to get an answer of 1.15 j? Cause i feel like the temp of the reservoir needs to be used somehow...
 
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the pressure and temperature is constant. So, the change in volume only depends on the work done by the gas and the constant pressure.

Work=integral of pressure times dV

So, yea, since the gas absorbs some heat, the particles will expand to a new volume and a dV of 1.5E-5m^3

If your calculations are correct, then you are fine.

The temperature would be used to calculate the amount of moles of the gas and other factors. They are letting you off easy on this. What physics are you in?
 

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