The heat liberated when $1.89 \ g$ of benzoic acid is burnt in a bomb calorimeter at $25^{\circ} C$ increases the temperature of $18.94 \ kg$ of water by $0.632^{\circ} C$. If the specific heat of water at $25^{\circ} C$ is $0.998 \ cal / (g^{\circ} C)$,then find the heat of combustion of benzoic acid.
- A$2540 \ kJ \ mol^{-1}$
- B$1975 \ kJ \ mol^{-1}$
- C$3240 \ kJ \ mol^{-1}$
- D$2825 \ kJ \ mol^{-1}$
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Similar Questions
Calculate $\Delta H_f^o$ of $SiH_2$ from the following reactions:
$Si_2H_{6(g)} + H_{2(g)} \to 2SiH_{4(g)}, \Delta H = -11.7 \ kJ/mol$
$SiH_{4(g)} \to SiH_{2(g)} + H_{2(g)}, \Delta H = +239.7 \ kJ/mol$
$\Delta H_f^o(Si_2H_{6(g)}) = 80.3 \ kJ/mol$
$Si_2H_{6(g)} + H_{2(g)} \to 2SiH_{4(g)}, \Delta H = -11.7 \ kJ/mol$
$SiH_{4(g)} \to SiH_{2(g)} + H_{2(g)}, \Delta H = +239.7 \ kJ/mol$
$\Delta H_f^o(Si_2H_{6(g)}) = 80.3 \ kJ/mol$
Medium
View SolutionMatch List-$I$ with List-$II$
List-$I$ List-$II$ $A$. Spontaneous process $I$. $\Delta H < 0$ $B$. Process with $\Delta P = 0; \Delta T = 0$ $II$. $\Delta G_{T, P} < 0$ $C$. $\Delta H_{reaction}$ $III$. Isothermal and isobaric process $D$. Exothermic process $IV$. [Bond energies of molecules in reactants] - [Bond energies of product molecules]
Choose the correct answer from the options given below:
| List-$I$ | List-$II$ |
| $A$. Spontaneous process | $I$. $\Delta H < 0$ |
| $B$. Process with $\Delta P = 0; \Delta T = 0$ | $II$. $\Delta G_{T, P} < 0$ |
| $C$. $\Delta H_{reaction}$ | $III$. Isothermal and isobaric process |
| $D$. Exothermic process | $IV$. [Bond energies of molecules in reactants] - [Bond energies of product molecules] |
Choose the correct answer from the options given below:
Consider the following data for the reaction $X_2(g) + Y_2(g) \rightleftharpoons 2XY(g)$ at $600 \ K$. The $\Delta_r G^\circ$ (in $kJ \ mol^{-1}$) for the reaction is:
Compound
$\Delta_f H^\circ$ $(kJ \ mol^{-1})$
$S^\circ$ $(J \ mol^{-1} \ K^{-1})$
$XY(g)$
$42$
$200$
$X_2(g)$
$8$
$140$
$Y_2(g)$
$80$
$250$
| Compound | $\Delta_f H^\circ$ $(kJ \ mol^{-1})$ | $S^\circ$ $(J \ mol^{-1} \ K^{-1})$ |
|---|---|---|
| $XY(g)$ | $42$ | $200$ |
| $X_2(g)$ | $8$ | $140$ |
| $Y_2(g)$ | $80$ | $250$ |
DifficultJEE MAIN 2026
View SolutionWhich graph represents an exothermic reaction?
Medium
View SolutionFor the hypothetical reaction
$A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$
$\Delta_r G^o$ and $\Delta_r S^o$ are $20 \ kJ/mol$ and $-20 \ J K^{-1} mol^{-1}$ respectively at $200 \ K$.
If $\Delta_r C_P$ is $20 \ J K^{-1} mol^{-1}$ then $\Delta_r H^o$ at $400 \ K$ is.....$kJ/mol$
$A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$
$\Delta_r G^o$ and $\Delta_r S^o$ are $20 \ kJ/mol$ and $-20 \ J K^{-1} mol^{-1}$ respectively at $200 \ K$.
If $\Delta_r C_P$ is $20 \ J K^{-1} mol^{-1}$ then $\Delta_r H^o$ at $400 \ K$ is.....$kJ/mol$
Medium
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