(D) For the free expansion of an ideal gas,the external pressure $P_{ext} = 0$,therefore the work done $w = -P_{ext} \Delta V = 0$. Since the process

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(D) For the free expansion of an ideal gas,the external pressure $P_{ext} = 0$,therefore the work done $w = -P_{ext} \Delta V = 0$. Since the process is adiabatic,the heat exchange $q = 0$. According to the first law of thermodynamics,$\Delta U = q + w$. Since $q = 0$ and $w = 0$,the change in internal energy $\Delta U = 0$. For an ideal gas,$\Delta U = nC_v \Delta T$. Since $\Delta U = 0$,it follows that $\Delta T = 0$.

Class 11 Chemistry Thermodynamics First law of thermodynamics

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Choose the correct option for the free expansion of an ideal gas under adiabatic conditions from the following:

JEE MAIN 2024 All JEE MAIN

A
$q=0, \Delta T \neq 0, w=0$
B
$q=0, \Delta T < 0, w \neq 0$
C
$q \neq 0, \Delta T = 0, w = 0$
D
$q = 0, \Delta T = 0, w = 0$

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Choose the correct option for the free expansion of an ideal gas under adiabatic conditions from the following:

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Consider the reaction at $298 \ K$:$H_{2(g)} + Cl_{2(g)} \to 2HCl_{(g)}, \Delta H^o = -185 \ kJ$What is $\Delta U^o$ for this reaction? .....$kJ$

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Consider the reaction at $298 \ K$:
$H_{2(g)} + Cl_{2(g)} \to 2HCl_{(g)}, \Delta H^o = -185 \ kJ$
What is $\Delta U^o$ for this reaction? .....$kJ$