The workdone in an adiabatic change in an ideal gas depends upon only :
A.change in its pressure
B.change in its specific heat
C.change in its volume
D.change in its temperature
Solution & Explanation
### Related Formula
Delta W = -Delta U = -n C_v Delta T$$\Delta W = -\Delta U = -n C_v \Delta T$$
### Core Logic
In an adiabatic system, no heat exchange occurs (Q=0$Q=0$). By the first law of thermodynamics, Delta W = -Delta U$\Delta W = -\Delta U$. Since internal energy U$U$ depends explicitly on temperature metrics, the total work output shifts uniquely based on temperature variation Delta T$\Delta T$.
### Chapter Mix
Class 11 Physics: Thermodynamics
More Thermodynamics Previous-Year Questions — Page 6
Q38jee_main_2024_31_jan_morningIsobaric Process
The given figure represents two isobaric processes for the same mass of an ideal gas, then
A Volume vs Temperature (V-T) graph showing two straight lines starting from the origin representing distinct constant pressures P1 and P2.
### Related Formula
PV = nRT$PV = nRT$
### Core Logic
From the Ideal Gas Law:
V = left(fracnRPright) T$$V = \left(\frac{nR}{P}\right) T$$
In a V-T$V-T$ graph, the equation of the line represents y = mx$y = mx$, where the slope m$m$ is:
textSlope = fracnRP$$\text{Slope} = \frac{nR}{P}$$textSlope propto frac1P$$\text{Slope} \propto \frac{1}{P}$$
Thus, a higher slope corresponds to a lower pressure.
### Step 2: Compare Slopes
From the given figure, the slope of line 2 is greater than the slope of line 1:
(textSlope)_2 > (textSlope)_1$$(\text{Slope})_2 > (\text{Slope})_1$$
Therefore, inversely:
P_2 < P_1$P_2 < P_1$
or P_1 > P_2$P_1 > P_2$.
### Pattern Recognition
In V-T graphs, steeper lines mean lower Pressure. In P-T graphs, steeper lines mean lower Volume. It's an inverse inverse slope relationship.
### Evaluation Rubric / Model Answer
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### Chapter Mix
Class 11 Physics: Thermodynamics
More Thermodynamics Questions — jee_main_2025_29_jan_morning
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