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question_answer1) A gas present in a cylinder fitted with a frictionless piston expands against a constant pressure of 1 atm from a volume of 2 litre to a volume of 6 litre. In doing so, it absorbs 800 heat from surroundings. Determine increase in internal energy of process.
question_answer2) The heat of neutralisation of strong base and strong acid is 57.0 kJ. Calculate the heat released when 0.5 mole of \[HN{{O}_{3}}\] is added to 0.20 mole of NaOH solution.
question_answer3) Given Reaction Energy Change \[Li(s)\to Li(g)\] 161 \[Li(g)\to L{{i}^{+}}(g)\] 520 \[\frac{1}{2}{{F}_{2}}(g)\to F(g)\] 77 \[F(g)+{{e}^{-}}\to {{F}^{-}}(g)\] (Electron gain enthapy) \[L{{i}^{+}}(g)+{{F}^{-}}(g)\to Li\,F(s)\] -1047 \[Li(s)+\frac{1}{2}{{F}_{2}}(g)\to Li\,\,F(s)\] -617 Based on data provided, find the value of electron gain enthalpy of fluorine.
question_answer4) The standard enthalpy of formation of \[N{{H}_{3}}\] is \[-\,46.0\text{ kJ}/mol\]. If the enthalpy of formation of \[{{H}_{2}}\] from its atoms is \[-\,436\text{ }kJ/mol\] and that of \[{{N}_{2}}\] is \[-712\text{ }kJ/mol,\] find the average bond enthalpy of \[N-H\] bond in \[N{{H}_{3}}\].
question_answer5) The enthalpy of neutralization of a weak acid in \[1\text{ }M\] solution with a strong base is\[-\,56.1\,kJ\ mo{{l}^{-1}}\]. If enthalpy of ionization of the acid is \[1.5\text{ }kJ\text{ }mo{{l}^{-1}}\] and enthalpy of neutralization of the strong acid with a strong base is \[-\,57.3\text{ }kJ\text{ }equi{{v}^{-1}},\] what is the % ionization of the weak acid in molar solution (assume the acid to be monobasic)?
question_answer6) The heat of sublimation of iodine is \[24\text{ }cal\text{ }{{g}^{-1}}\] at \[50{}^\circ C\]. If specific heat of solid iodine and its vapour are \[0.055\] and \[0.031\text{ }cal\text{ }{{g}^{-1}}\] respectively. Calculate the heat of sublimation of iodine at \[100{}^\circ C\].
question_answer7) When \[0.2\] mole of anhydrous \[CuS{{O}_{4}}\] is dissolved in water, the heat evolved is\[1.451\text{ }kcal\]. If 0.2 of \[CuS{{O}_{4}}.5{{H}_{2}}O\] is dissolved in water, the heat absorbed is 0.264 kcal. Calculate the molar heat of hydration of \[CuS{{O}_{4}}\]
question_answer8) The specific heat of a monoatomic gas at constant pressure is \[~248.2\text{ }J\text{ }k{{g}^{-1}}\text{ }{{K}^{-1}}\] and at constant volume it is \[149.0\text{ }J\text{ }k{{g}^{-1}}\text{ }{{K}^{-1}}\]. Find the mean molar mass of the gas.
question_answer9) The standard entropies of \[C{{O}_{2}}(g),\,\,C\,(s),\,\,C\,(s)\] and \[{{O}_{2}}(g)\] are 213.5, 5.740 and \[205\text{ }J{{K}^{-1}}\] respectively. Calculate the standard entropy of formation of \[C{{O}_{2}}(g)\].
question_answer10) Titanium metal is extensively used in aerospace industry because the metal imparts strength to structures but does not unduly add to their masses. The metal is produced by the reduction of \[TiC{{l}_{4}}(\text{l})\] which in turn is produced from mineral rutile\[Ti{{O}_{2}}(s)\]Calculate the Gibb's free energy for the following reaction \[Ti{{O}_{2}}(s)+2C{{l}_{2}}(g)\to TiC{{l}_{4}}(l)+{{O}_{2}}(g)\] Given that: \[H_{f}^{o}\] for \[Ti{{O}_{2}}(s),\] \[TiC{{l}_{4}}(l),\,C{{l}_{2}}(g)\] and \[{{O}_{2}}\,(g)\] are \[-\,944.7,-\,804.2,0.0,\,\,0.0\text{ }kJ\,mo{{l}^{-1}}\] Also \[S{}^\circ \]for \[Ti{{O}_{2}}(g),TiC{{l}_{4}}(l),\,C{{l}_{2}}(g)\] and \[{{O}_{2}}\,(g)\]are 50.3, 252.3, 233.0, 205.1 J \[mo{{l}^{-1}}{{K}^{-1}}\]respectively.
question_answer11) One mole of \[C{{H}_{3}}COOH\] undergoes dimerization in vapour phase at \[127{}^\circ C\]as: \[2C{{H}_{3}}COOH(g)\rightleftharpoons {{(C{{H}_{3}}COOH)}_{2}}(g)\] if dimer formation is due to two H-bonds involved in dimer, each of 33 kJ strength and the degree of dimerisation of acetic acid 98.2%. Calculate the change in standard entropy during dimerization.
question_answer12) The factor of \[\Delta G\] values is important in metallurgy. The \[\Delta G\] values for the following reactions at \[800{}^\circ C\] are given as: \[{{S}_{2}}(s)+2{{O}_{2}}(g)\xrightarrow{{}}2S{{O}_{2}}(g);\,\,\Delta G=-\,544\,\,kJ\] \[2Zn(s)+{{S}_{2}}\text{(s)}\xrightarrow[{}]{}2ZnS(s);\,\,\Delta G=-\,293\text{ }kJ\] \[2Zn(s)+{{O}_{2}}(g)\xrightarrow{{}}2ZnO(s);\,\,\Delta G=-\,480\,kJ\] Calculate the \[\Delta G\] for the reaction: \[2ZnS(s)+3{{O}_{2}}\text{(}g\text{)}\xrightarrow{{}}2ZnO(s)+2S{{O}_{2}}(g)\]
question_answer13) For vaporization of water at 1 atmospheric pressure, the values of \[\Delta \,H\] and \[\Delta S\] are \[40.63\text{ }kJ\,mo{{l}^{-1}}\] and \[108.8\text{ }J{{K}^{-1}}\text{ }mo{{l}^{-1}}\], respectively. Find the temperature at which Gibbs energy change \[(\Delta G)\] for this transformation will be zero.
question_answer14) An ideal gas is allowed to expand from 1 L to 10 L against a constant external pressure of 1 bar. Calculate the work done in kJ.
question_answer15) During compression of a spring the work done is 10 kJ and 2 kJ escaped to the surroundings as heat. Calculate the change in internal energy, (in kJ).
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