Question
When an ideal gas expands at a constant temperature, $\Delta E=0$ for the change. Why?
Step 1
This means that the internal energy of the gas, which is directly related to its temperature, also remains constant. Mathematically, this can be represented as $\Delta E = 0$. Show more…
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When a real gas expands at a constant temperature, $\Delta E>0$ for the change. Why?
An ideal gas is initially at temperature $T$ and volume $V$. Its volume increases by $\Delta V$ due to an increase in temperature of $\Delta T$, pressure remaining constant. The quantity $\delta=\frac{\Delta V}{V \Delta T}$ varies with temperature as
Gaseous State
Exercises II
A gas expands against a non-zero external pressure while in thermal isolation from the surroundings. For this expansion a. $\Delta \mathrm{E}=\mathrm{q}$ b. $\Delta \mathrm{E}$ increases c. $\Delta \mathrm{E}$ does not change d. $\Delta \mathrm{E}$ decreases
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