At $25^{\circ} C$ and $1 \, atm$ pressure,the enthalpy of combustion of benzene$_{(l)}$ and acetylene$_{(g)}$ are $-3268 \, kJ \, mol^{-1}$ and $-1300 \, kJ \, mol^{-1}$,respectively. The change in enthalpy for the reaction $3 C_2H_{2(g)} \rightarrow C_6H_{6(l)}$ is $..... \, kJ \, mol^{-1}$.
- A$+324$
- B$+632$
- C$-632$
- D$-324$
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Which of the following is incorrect?
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View SolutionMatch the List-$I$ with List-$II$
List-$I$ Thermodynamic Process List-$II$ Magnitude in $kJ$ $A$. Work done in reversible, isothermal expansion of $2 \ mol$ of ideal gas from $2 \ dm^3$ to $20 \ dm^3$ at $300 \ K$. $I$. $4$ $B$. Work done in irreversible isothermal expansion of $1 \ mol$ ideal gas from $1 \ m^3$ to $3 \ m^3$ at $300 \ K$ against a constant pressure of $3 \ kPa$. $II$. $11.5$ $C$. Change in internal energy for adiabatic expansion of a $1 \ mol$ ideal gas with change of temperature $= 320 \ K$ and $\overline{C}_V = \frac{3}{2} R$. $III$. $6$ $D$. Change in enthalpy at constant pressure of $1 \ mole$ ideal gas with change of temperature $= 337 \ K$ and $\overline{C}_P = \frac{5}{2} R$. $IV$. $7$
Choose the correct answer from the option given below:
| List-$I$ Thermodynamic Process | List-$II$ Magnitude in $kJ$ |
| $A$. Work done in reversible, isothermal expansion of $2 \ mol$ of ideal gas from $2 \ dm^3$ to $20 \ dm^3$ at $300 \ K$. | $I$. $4$ |
| $B$. Work done in irreversible isothermal expansion of $1 \ mol$ ideal gas from $1 \ m^3$ to $3 \ m^3$ at $300 \ K$ against a constant pressure of $3 \ kPa$. | $II$. $11.5$ |
| $C$. Change in internal energy for adiabatic expansion of a $1 \ mol$ ideal gas with change of temperature $= 320 \ K$ and $\overline{C}_V = \frac{3}{2} R$. | $III$. $6$ |
| $D$. Change in enthalpy at constant pressure of $1 \ mole$ ideal gas with change of temperature $= 337 \ K$ and $\overline{C}_P = \frac{5}{2} R$. | $IV$. $7$ |
Choose the correct answer from the option given below:
DifficultJEE MAIN 2026
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