(A) Given: $P_1 = 5 \, atm$,$V_1 = 2 \, L$,$P_{ext} = 1 \, atm$,$P_2 = 1 \, atm$.Since the process is isothermal,$P_1 V_1 = P_2 V_2$.$V_2 = \frac{P_1

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(A) Given: $P_1 = 5 \, atm$,$V_1 = 2 \, L$,$P_{ext} = 1 \, atm$,$P_2 = 1 \, atm$.Since the process is isothermal,$P_1 V_1 = P_2 V_2$.$V_2 = \frac{P_1 V_1}{P_2} = \frac{5 \, atm \times 2 \, L}{1 \, atm} = 10 \, L$.The work done in an irreversible expansion is given by $W = -P_{ext} \Delta V$.$W = -1 \, atm \times (10 \, L - 2 \, L) = -8 \, L \cdot atm$.Converting to Joules $(1 \, L \cdot atm = 101.3 \, J)$:$W = -8 \times 101.3 \, J = -810.4 \, J$.The negative sign indicates that work is done by the system.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

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Two liters of $N_2$ gas at $0 \, ^\circ C$ and $5 \, atm$ pressure undergoes isothermal expansion against a constant external pressure of $1 \, atm$ until the pressure of the gas becomes $1 \, atm$. If the gas is ideal,what is the work done in the expansion in $J$?

A
$810.4$
B
$770.4$
C
$649.3$
D
$840.7$

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Mix Examples-Thermodynamics and Thermochemistry

$500 \ J$ of energy is transferred as heat to $0.5 \ mol$ of Argon gas at $298 \ K$ and $1.00 \ atm$. The final temperature and the change in internal energy respectively are $:$ Given $: R = 8.3 \ J \ K^{-1} \ mol^{-1}$

MediumJEE MAIN 2025

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Statement-$I$: Both internal energy $(U)$ and work $(w)$ are state functions.
Statement-$II$: During the free expansion of an ideal gas into vacuum,the work done is zero.
The correct answer is:

MediumAP EAMCET 2025

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For the reaction $X_2Y_{4(l)} \rightarrow 2XY_{2(g)}$ at $300 \ K$, the values of $\Delta U$ and $\Delta S$ are $2 \ kcal$ and $20 \ cal \ K^{-1}$ respectively. The value of $\Delta G$ for the reaction is (in $cal$)

MediumWBJEE 2015

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The $\Delta H$ and $\Delta S$ for a reaction at $1 \ \text{atm}$ pressure are $+30.558 \ \text{kJ}$ and $0.066 \ \text{kJ K}^{-1}$ respectively. The temperature at which the free energy change will be zero and below this temperature the nature of the reaction would be:

Medium

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An ideal gas undergoes a reversible cyclic process as shown in the figure. The work done in this process is: (in $,V_1P_1$)

Medium

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Two liters of $N_2$ gas at $0 \, ^\circ C$ and $5 \, atm$ pressure undergoes isothermal expansion against a constant external pressure of $1 \, atm$ until the pressure of the gas becomes $1 \, atm$. If the gas is ideal,what is the work done in the expansion in $J$?

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$500 \ J$ of energy is transferred as heat to $0.5 \ mol$ of Argon gas at $298 \ K$ and $1.00 \ atm$. The final temperature and the change in internal energy respectively are $:$ Given $: R = 8.3 \ J \ K^{-1} \ mol^{-1}$

Consider the following statements:Statement-$I$: Both internal energy $(U)$ and work $(w)$ are state functions.Statement-$II$: During the free expansion of an ideal gas into vacuum,the work done is zero.The correct answer is:

For the reaction $X_2Y_{4(l)} \rightarrow 2XY_{2(g)}$ at $300 \ K$, the values of $\Delta U$ and $\Delta S$ are $2 \ kcal$ and $20 \ cal \ K^{-1}$ respectively. The value of $\Delta G$ for the reaction is (in $cal$)

The $\Delta H$ and $\Delta S$ for a reaction at $1 \ \text{atm}$ pressure are $+30.558 \ \text{kJ}$ and $0.066 \ \text{kJ K}^{-1}$ respectively. The temperature at which the free energy change will be zero and below this temperature the nature of the reaction would be:

An ideal gas undergoes a reversible cyclic process as shown in the figure. The work done in this process is: (in $,V_1P_1$)

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Consider the following statements:
Statement-$I$: Both internal energy $(U)$ and work $(w)$ are state functions.
Statement-$II$: During the free expansion of an ideal gas into vacuum,the work done is zero.
The correct answer is: