One gram sample of $NH_4NO_3$ is decomposed in a bomb calorimeter. The temperature of the calorimeter increases by $6.12 \ K$. The heat capacity of the system is $1.23 \ kJ/K$. What is the molar heat of decomposition for $NH_4NO_3$ in $kJ/mol$?
- A$-7.53$
- B$-398.1$
- C$-16.1$
- D$-602$
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Similar Questions
If standard molar enthalpy change and standard molar internal energy change measured in a bomb calorimeter are equal,which one of the following statements is correct?
An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If $T_i$ is the initial temperature and $T_f$ is the final temperature,which of the following statements is correct?
MediumAIEEE 2006
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
View SolutionMatch the following items in List-$I$ with their corresponding expressions in List-$II$.
List-$I$ List-$II$ $A$. At constant volume the change in internal energy of a system $I$. $W = -2.303 nRT \log \frac{V_f}{V_i}$ $B$. Isothermal irreversible change $II$. $W_{adiabatic} = \Delta U$ $C$. Isothermal reversible change $III$. $q_V = \Delta U$ $D$. Adiabatic change $IV$. $W = -p_{ex} (V_f - V_i)$ $V$. $\Delta U = \Delta H - \Delta nRT$
| List-$I$ | List-$II$ |
| $A$. At constant volume the change in internal energy of a system | $I$. $W = -2.303 nRT \log \frac{V_f}{V_i}$ |
| $B$. Isothermal irreversible change | $II$. $W_{adiabatic} = \Delta U$ |
| $C$. Isothermal reversible change | $III$. $q_V = \Delta U$ |
| $D$. Adiabatic change | $IV$. $W = -p_{ex} (V_f - V_i)$ |
| $V$. $\Delta U = \Delta H - \Delta nRT$ |
An ideal gas expanded irreversibly against $10 \ bar$ pressure from $20 \ L$ to $30 \ L$. Calculate $Q$ if the process is isoenthalpic. $(1 \ L \ bar = 100 \ J)$
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