$A$ sample of gas is compressed from an initial volume of $2V_0$ to $V_0$ using three different processes.
First: Using reversible isothermal.
Second: Using reversible adiabatic.
Third: Using irreversible adiabatic under a constant external pressure.
Then
First: Using reversible isothermal.
Second: Using reversible adiabatic.
Third: Using irreversible adiabatic under a constant external pressure.
Then
- AFinal temperature of gas will be highest at the end of second process.
- BFinal temperature of gas will be highest at the end of third process.
- CEnthalpy change of sample will be highest in isothermal process (magnitude wise).
- DFinal pressure of gas will be highest at the end of second process.
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Similar Questions
Which one of the following is always not negative?
Easy
View SolutionGiven below are two statements:
Statement $I$: For an ideal gas,heat capacity at constant volume is always greater than the heat capacity at constant pressure.
Statement $II$: In a constant volume process,no work is produced and all the heat withdrawn goes into the chaotic motion and is reflected by a temperature increase of the ideal gas.
Statement $I$: For an ideal gas,heat capacity at constant volume is always greater than the heat capacity at constant pressure.
Statement $II$: In a constant volume process,no work is produced and all the heat withdrawn goes into the chaotic motion and is reflected by a temperature increase of the ideal gas.
Latent heat of vaporisation of a liquid at $500 \ K$ and $1 \ atm$ pressure is $20.0 \ kcal/mol$. What will be the change in internal energy $(\Delta E)$ of $3 \ mol$ of liquid at same temperature in $kcal$?
Medium
View SolutionConsider the following reaction :
$2A (g) + B (g) \rightarrow 2D(g)$
$\Delta U^{\circ} = -10 \text{ kJ mol}^{-1}$ and $\Delta S^{\circ} = -44 \text{ J K}^{-1} \text{ mol}^{-1}$ at $298 \text{ K}$.
Identify the correct option with $\Delta G^{\circ}$ for the reaction and spontaneity of the reaction at $298 \text{ K}$.
(Given : $R = 8.31 \text{ J mol}^{-1} \text{ K}^{-1}$)
$2A (g) + B (g) \rightarrow 2D(g)$
$\Delta U^{\circ} = -10 \text{ kJ mol}^{-1}$ and $\Delta S^{\circ} = -44 \text{ J K}^{-1} \text{ mol}^{-1}$ at $298 \text{ K}$.
Identify the correct option with $\Delta G^{\circ}$ for the reaction and spontaneity of the reaction at $298 \text{ K}$.
(Given : $R = 8.31 \text{ J mol}^{-1} \text{ K}^{-1}$)
DifficultNEET 2026
View SolutionThe enthalpy change for the reaction of $50.00 \ mL$ of ethylene with $50.00 \ mL$ of $H_2$ at $1.5 \ atm$ pressure is $\Delta H = -0.31 \ kJ$. The value of $\Delta E$ will be (in $kJ$)
Medium
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