(C) For the free expansion of an ideal gas,the process is adiabatic,so $q = 0$. Since the expansion occurs against zero external pressure $(P_{ext} =

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(C) For the free expansion of an ideal gas,the process is adiabatic,so $q = 0$. Since the expansion occurs against zero external pressure $(P_{ext} = 0)$,the work done is $W = -P_{ext} \Delta V = 0$. According to the first law of thermodynamics,$\Delta U = q + W$. Since $q = 0$ and $W = 0$,$\Delta U = 0$. For an ideal gas,internal energy $U$ is a function of temperature only,so $\Delta U = 0$ implies $\Delta T = 0$.

Class 11 Chemistry Thermodynamics First law of thermodynamics

Medium

Which of the following is the correct option for the free expansion of an ideal gas under adiabatic conditions?

AIPMT 2011 All AIPMT

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

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If $100 \ L$ of an ideal gas at a pressure of $2 \ atm$ is compressed isothermally and reversibly to a final volume of '$X$' $L$ and releases $460.6 \ L \ atm$ of heat,the final volume '$X$' (in $L$) is

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Derive the relationship between $\Delta H$ and $\Delta U$ for an ideal gas. Explain each term involved in the equation.

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$A$ gas occupies $1.5 \ L$ at $S.T.P.$ It is provided with $300 \ J$ of heat so that its volume becomes $2 \ L$ at a pressure of $1 \ atm$. The value of $\Delta U$ for the process is.....joule.

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The gas absorbs $100 \ J$ and is simultaneously compressed by a constant external pressure of $1.50 \ atm$ from $8 \ L$ to $2 \ L$ volume. Hence $\Delta U$ will be ..... $J$.

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Which one of the following is applicable for an adiabatic expansion of an ideal gas?

EasyAP EAMCET 2015

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Which of the following is the correct option for the free expansion of an ideal gas under adiabatic conditions?

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If $100 \ L$ of an ideal gas at a pressure of $2 \ atm$ is compressed isothermally and reversibly to a final volume of '$X$' $L$ and releases $460.6 \ L \ atm$ of heat,the final volume '$X$' (in $L$) is

Derive the relationship between $\Delta H$ and $\Delta U$ for an ideal gas. Explain each term involved in the equation.

$A$ gas occupies $1.5 \ L$ at $S.T.P.$ It is provided with $300 \ J$ of heat so that its volume becomes $2 \ L$ at a pressure of $1 \ atm$. The value of $\Delta U$ for the process is.....joule.

The gas absorbs $100 \ J$ and is simultaneously compressed by a constant external pressure of $1.50 \ atm$ from $8 \ L$ to $2 \ L$ volume. Hence $\Delta U$ will be ..... $J$.

Which one of the following is applicable for an adiabatic expansion of an ideal gas?

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