JEE Mains · Physics · STD 11 - 11. thermodynamics
One mole of a diatomic ideal gas undergoes a cyclic process \(ABC\) as shown in figure. The process \(BC\) is adiabatic. The temperatures at \(A, B\) and \(C\) are \(400\ K, 800\ K \) and \(600\ K\) respectively. Choose the correct statement
- A The change in internal energy in the process \(CA\) is \(700\ R\)
- B The change in internal energy in the process \(AB\) is \( -350R\)
- C The change in internal energy in the process \(BC\) is \(-500R\)
- D The change in internal energy in whole cyclic process is \(250R \)
Answer & Solution
Correct Answer
(C) The change in internal energy in the process \(BC\) is \(-500R\)
Step-by-step Solution
Detailed explanation
In cyclic process, change in total internal energy is zero. \(\Delta {U_{cyclic}} = 0\) \(\Delta {U_{BC}} = n{C_v}\Delta T = 1 \times \frac{{5R}}{2}\Delta T\) \(Where,{C_v} = molar\,specific\,heat\,at\,constant\,volume.\) \(For\,BC,\Delta T = - 200K\)…
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