Question 454: Thermodynamics & KTG

Question

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 :
![](https://imagex.cdn.examgoal.net/4nA8ahHVgMiVB6QjJ/pI5ohzNBYpIIzbFGCqRb5i8nEVzXv/JcIcGOuPCeq4IzmbsJwzkn/image.png)

Accepted Answer

In cyclic process, change in total internal energy is zero.
$\Delta {U_{cyclic}} = 0$
$\Delta {U_{BC}} = n{C_v}\Delta T = 1 	imes {{5R} \over 2}\Delta T$
where, ${C_v} = $ molar specific heat at constant volume.
For $BC,$ $\Delta T =  - 200\,K$
$	herefore$ $\Delta {U_{BC}} =  - 500R$

Answer

The change in internal energy in whole cyclic process is $250$ $R.$

Answer

The change in internal energy in the process $CA$ is $700$ $R$.

Answer

The change in internal energy in the process $AB$ is - $350$ $R.$

Answer

The change in internal  energy in the process $BC$ is - $500$ $R.$

Thermodynamics & KTG

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 :

Choose the correct answer: