If (i) \[\Delta H_{f}^{o}\] (benzene)\[=-358.5\,\,kJ\,\,mo{{l}^{-1}}\].
(ii) Heat of atomization of graphite\[=716.8\,\,kJ\,mo{{l}^{-1}}\].
(iii) Bond energy of \[C-H,\,\,C-C,\,\,C=C\] and \[H-H\] bonds are 490, 340, 620 and\[436.9\,\,kJ\,\,mo{{l}^{-1}}\] respectively. The resonance energy (in \[kJ\,\,mo{{l}^{-1}}\]) of \[{{C}_{6}}{{H}_{6}}\] using Kekule formula is
A 1 g sample of octane \[{{C}_{8}}{{H}_{18}}\] is burned in excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rises from 294 K to 300 K. If heat capacity of the calorimeter is 8 kJ/K, the enthalpy of combustion of octane is
The polymerization of ethylene to linear polyethylene is represented by the reaction \[nC{{H}_{2}}=C{{H}_{2}}\xrightarrow{\,}\,{{(-C{{H}_{2}}-C{{H}_{2}}-)}_{n}}\] when 'n' has a large integral value. Given that average enthalpies of bond dissociation for \[C=C\] and \[C-C\] at 298 K are + 590 and \[+331\,\,kJ\,\,mo{{l}^{-1}}\] respectively. Then the enthalpy of polymerization/mol of ethylene at298 K is
The standard heat of combustion of Al is \[-\,837.8\,kJ\,mo{{l}^{-1}}\] at \[{{25}^{o}}C\]. If Al reacts with \[{{O}_{2}}\] at \[{{25}^{o}}C,\] which of the following releases 250 kcal of heat?
A)
The reaction of 0.624 mole of Al
doneclear
B)
The formation of 0.624 mole of \[A{{l}_{2}}{{O}_{3}}\]
doneclear
C)
The reaction of 0.312 mole of Al
doneclear
D)
The formation of 0.150 mole of \[A{{l}_{2}}{{O}_{3}}\]
The heat of hydration of solution anhydrous \[CuS{{O}_{4}}\] and hydrated \[CuS{{O}_{4}}\cdot 5{{H}_{2}}O\] are - 66.5 and 11.7 kJ \[mo{{l}^{-1}}\]respectively. Calculate the heat of hydration of \[CuS{{O}_{4}}\] to \[CuS{{O}_{4}}\cdot 5{{H}_{2}}O\]
In an adiabatic process non-transfer of heat takes place between system and surroundings. Choose the correct option for free expansion of an ideal gas under adiabatic condition from the following.
\[2{{A}_{2}}(g)+5{{B}_{2}}(g)\to 2{{A}_{2}}{{B}_{5}}(g)\] at \[{{27}^{o}}C\]
the heat change at constant pressure is found to be \[-\,50160\,J\]. Calculate the value of internal energy change \[(\Delta E)\]. Given that R = 8.314 J/K mol.
The difference between the heats of reaction at constant pressure and a constant volume for the reaction \[2{{C}_{6}}{{H}_{6\left( 1 \right)}}+15{{O}_{2(g)}}\xrightarrow{{}}12C{{O}_{2(g)}}+6{{H}_{2}}{{O}_{(I)}}\] in Kj is :
The enthalpy of combustion of \[{{H}_{2}}(g),\] to give\[{{H}_{2}}(g)\] is \[-249\text{ }kJ\text{ }mo{{l}^{-1}}\] and bond enthalpies of \[H-H\] and \[O=O\] are \[433\text{ }kJ\text{ }mo{{l}^{-1}}\] and \[492\text{ }kJ\text{ }mo{{l}^{-1}}\] respectively. The bond enthalpy of \[O-H\] is
Use the bond enthalpies in the table to determine \[\Delta H{}^\circ \] for the formation of hydrazine, \[{{N}_{2}}{{H}_{4}}(g)\] from nitrogen and hydrogen in standard state according to the equation : \[{{N}_{2}}(g)+2{{H}_{2}}(g)\xrightarrow{{}}{{N}_{2}}{{H}_{4}}(g)\]
For this reaction \[\Delta {{H}^{o}}=129.2\,kJ/mol,\] \[\Delta {{S}^{o}}=334.2\,J/mol-K\]. From this information, the minimum temperature at which this reaction becomes spontaneous is:
Consider the following reaction occuring in an automobile engine : \[2{{C}_{8}}{{H}_{18}}(l)+25\,{{O}_{2}}(g)\to 16\,C{{O}_{2}}(g)+18\,{{H}_{2}}O(g)\] of \[\Delta H,\,\Delta S\] and \[\Delta G\] would be:
A coffee cup calorimeter initially contains 125 g of water, at a temperature of \[24.2{}^\circ C\]. 8 g of ammonium nitrate \[(N{{H}_{4}}N{{O}_{3}}),\] also at \[24.2{}^\circ C,\] is added to the water, and the final temperature is \[18.2{}^\circ C\] what is the heat of solution of ammonium nitrate in kJ/mol? The specific heat capacity of the solution is \[4.2\text{ }J/{}^\circ Cg\].
Calculate the heat change in the reaction \[4\,N{{H}_{3}}(g)+3{{O}_{2}}(g)\to 2{{N}_{2}}(g)+6{{H}_{2}}O(\ell )\] at 298 K, given that the heats of formation at 298 K for \[N{{H}_{3}}(g)\] and \[{{H}_{2}}O(\ell )\] are - 46.0 and - 28.60 kJ \[mo{{l}^{-1}}\] respectively.
If heat of dissociation of \[CHC{{l}_{2}}COOH\] is 0.7 kcal/mol, then \[\Delta H\] for the reaction: \[CHC{{l}_{2}}COOH+KOH\to CHC{{l}_{2}}COOK+{{H}_{2}}O\]
The \[\Delta H_{F}^{O}\] for \[C{{O}_{2}}(g),\,\,CO(g)\] and \[{{H}_{2}}O(g)\] are \[-\,393.5,\,-110.5\] and \[-\,241.8\text{ }kJ\text{ }mol\], respectively. The standard enthalpy change (in kJ) for the reaction \[C{{O}_{2(g)}}+{{H}_{2}}_{(g)}\xrightarrow{{}}C{{O}_{(g)}}+{{H}_{2}}{{O}_{(g)}}\] is:
The enthalpies of formation of \[A{{l}_{2}}{{O}_{3}}\] and \[C{{r}_{2}}{{O}_{3}}\] 1596 kJ and - 1134 kJ respectively. \[\Delta H\] for the reaction \[2Al+C{{r}_{2}}{{O}_{3}}\to 2Cr+A{{l}_{2}}{{O}_{3}}\]
The heat of neutralization of four acids A, B, C, D are -13.7, -9.4, - 11.2 and - 12.4 kcal, respectively, when they are neutralized by a common base. The acidic character obeys the order: