Question 2 : The enthalpy of vapourisation of water from the following two equations is.<br>{tex} \mathrm { H } _ { 2 } ( \mathrm { g } ) + \frac { 1 } { 2 } \mathrm { O } _ { 2 } ( \mathrm { g } ) \longrightarrow \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { l } ) , \Delta \mathrm { H } = - 286 \mathrm { kJ } {/tex}<br>{tex} \mathrm { H } _ { 2 } ( \mathrm { g } ) + \frac { 1 } { 2 } \mathrm { O } _ { 2 } ( \mathrm { g } ) , \rightarrow \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { g } ) , \Delta \mathrm { H } = - 245.5 \mathrm { kJ } {/tex}

Question 3 : A container has hydrogen and oxygen mixture in ratio of <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d1b56f3020298ca13bf2"> by weight, then:

Question 4 : 48 g of C (diamond) on complete combustion evolves 1584 kJ of heat. The standard heat of formation of gaseous carbon is 725 kJ/mol. The energies required for the process<br> (i)C (graphite) <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d1746f3020298ca13b95"> C(gas)<br> (ii)C (diamond) <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d1746f3020298ca13b95"> C(gas)are:

Question 5 : A given mass of gas expands reversibly from the state {tex}A{/tex} to the state {tex}B{/tex} by three paths {tex}1 , 2{/tex} and {tex}3{/tex} as shown in the figure. If {tex}w_1 , w_ 2{/tex} and {tex}w_3{/tex} respectively be the work done by the gas along three paths then:<br> <img style='object-fit:contain' src='https://storage.googleapis.com/teachmint/question_assets/NEET/5efadb7a2cb6ea3d580629d4' class="uploaded-image" />

Question 7 : It is impossible to attain the lowest temperature known as zero degree absolute. This is a simple statement of:

Question 8 : The standard enthalpy of formation (DHf°) at 398 K for methane, CH₄(g) is 74.8 kJ mol^–1. The additional information required to determine the average energy for C – H bond formation would be.

Question 9 : Enthalpy of solution of <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d1a6ab3481716f4b74d1"> (solid) in water is <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d2d4c2a2ae2953d94896"> , when <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d1a6ab3481716f4b74d1"> is dissolved in water, the temperature of water

Question 10 : The heat of neutralisation of a strong acid and a strong alkali is 5 <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d2b5c2a2ae2953d94840"> . The heat released when 0.5 mole of <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d1db399925718ac6afe8"> solution is mixed with 0.2 mole of KOH is

Question 11 : The heat of combustion of methane is <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d1b56f3020298ca13bf3"> If 3.2 g of methane is burnt:

Question 13 : For the reaction of one mole of zinc dust with one mole of sulphuric acid in a bomb calorimeter, {tex} \Delta \mathrm { U } {/tex} and {tex} \mathrm { w } {/tex} corresponds to

Question 14 : When water is added to quick lime, the reaction is :

Question 16 : All the naturally occurring processes, <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d29fab3481716f4b76e7"> spontaneous proceed spontaneously in a direction which leads to:

Question 17 : What is the entropy change (in {tex} \mathrm { JK } ^ { - 1 } \mathrm { mol } ^ { - 1 } {/tex} ) when one mole of ice is converted into water at {tex} 0 ^ { \circ } \mathrm { C } {/tex} ? (The enthalpy change for the conversion of ice to liquid water is {tex} 6.0 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex} at {tex} 0 ^ { \circ } \mathrm { C } {/tex} )

Question 21 : The Gibbs energy change for a reversible reaction at equilibrium is:

Question 23 : One mole of a non-ideal gas undergoes a change of state {tex} ( 2.0 \text { atm, } 3.0 \mathrm { L } , 95 \mathrm { K } ) \rightarrow ( 4.0 \mathrm { atm } , {/tex} {tex} 5.0 \mathrm { L } , 245 \mathrm { K } ) {/tex} with a change in internal energy, {tex} \Delta \mathrm { U } = 30.0 \mathrm { L } \mathrm { atm } . {/tex} The change in enthalpy {tex} \Delta \mathrm { H } {/tex} of the process in {tex} \mathrm { L } {/tex} atm is.

Question 24 : One mole of solid iron was vaporized in an oven at its boiling point of {tex} 3433 \mathrm { K } {/tex} and enthalpy of vaporization of iron is {tex} 344.3 \mathrm { kJ } \mathrm { mol } ^ { - 1 } . {/tex} The value of entropy vaporization (in {tex} \left. \mathrm { J } \mathrm { mol } ^ { - 1 } \right) {/tex} of iron is

Question 26 : The enthalpy of vaporisation of a substance is <b>840 J/mol</b> and its boiling point is <b>-173&deg;C</b> . Its entropy of vaporisation is

Question 28 : At 25°C, when 1 mole of {tex} \mathrm {MgSO}_4{/tex} was dissolved in water, the heat evolved was found to be {tex}91.2 \mathrm {kJ}{/tex}. One mole of {tex} \mathrm {MgSO_4 . 7H_20}{/tex} on dissolution gives a solution of the same composition accompanied by an absorption of {tex}13.8 \mathrm {kJ}{/tex} . The enthalpy of hydration, i.e., {tex}\mathrm { \Delta H _h}{/tex} for the reaction <br>{tex} \mathrm { MgSO } _ { 4 } ( \mathrm { s } ) + 7 \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { l } ) \longrightarrow \mathrm { MgSO } _ { 4 } .7 \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { s } ) {/tex} is<br>

Question 30 : Combustion of glucose takes place according to the equation <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d1436f3020298ca13b08"> kcal. How much energy will be required for the production of 1.6 g of glucose (Molecular mass of glucose = 180)?

Question 35 : The enthalpies of the elements in their standard states are assumed to be

Question 36 : A gaseous reaction was carried out, first keeping the volume constant and next keeping the pressure constant. In the second experiment, there was an increase in volume. The heats of reaction were different, because :

Question 38 : Under the same conditions how many mL of <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d13ac2a2ae2953d94643"> and <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d13a6f3020298ca13af1"> solutions, respectively when mixed for a total volume of 100 mL produce the highest rise in temperature?

Question 39 : The latent heat of vapourization of a liquid at {tex} 500 \mathrm { K } {/tex} and {tex}1{/tex} atm pressure is {tex} 10.0 \mathrm { kcal } / \mathrm { mol } {/tex}. What will be the change in internal energy {tex} ( \Delta \mathrm { U } ) {/tex} of {tex}3{/tex} moles of liquid at the same temperature

Question 41 : The heat change for the reaction, <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d1afab3481716f4b74ec"> is called:

Question 43 : A well stoppered thermos flask containing some ice cubes is an example of:

Question 44 : Warming ammonium chloride with sodium hydroxide in a test tube is an example of:

Question 46 : At absolute zero, the entropy of a perfect crystal is zero. This is of thermodynamics.

Question 47 : A container has hydrogen and oxygen mixture in ratio of 1 : 1 by weight, then

Question 49 : If a reaction involves only solids and liquids which of the following is true?

Question 50 : Enthalpy of neutralisation of {tex} \mathrm {HCl}{/tex} with {tex} \mathrm { NaOH }{/tex} is {tex}x{/tex}. The heat evolved when {tex} 500 \mathrm { mL } {/tex} of {tex} 2 \mathrm { NCl } {/tex} are mixed with {tex}250 \mathrm { mL } {/tex} of {tex} 4 \ \mathrm { {N} \ \mathrm { NaOH }}{/tex} will be.

Question 51 : A heat engine carries one mole of an ideal mono-atomic gas around the cycle as shown in the figure. Select the correct option:<br><img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5dfc68498701466b65e5eb13"><br>

Question 53 : What is the normal boiling point of mercury? Given : <br>{tex}\Delta H^{\circ}_f{/tex}{tex}\mathrm { (Hg, I)} {/tex} = 0; {tex}\mathrm {S°(Hg, I)}{/tex} = {tex}77.4 \mathrm {J/K—mol}{/tex} {tex}\Delta H^{\circ}_f{/tex}{tex}\mathrm { (Hg, g)}= 60.8 \mathrm{kJ/mol};{/tex}{tex}\mathrm {S°(Hg, I)}{/tex} = {tex}174.4 \mathrm {J/K—mol}{/tex}

Question 54 : Combustion of sucrose is used by aerobic organisms for providing energy for the life sustaining processes. If all the capturing of energy from the reaction is done through electrical process (non {tex} \mathrm { P-V } {/tex} work) then calculate maximum available energy which can be captured by combustion of {tex}34.2 g{/tex} of sucrose Given: {tex}\mathrm {\Delta H_{combustion}(sucrose)} = 6000 \mathrm { kJ mol}^{-1} {/tex} Given : {tex}\mathrm {\Delta S_{combustion}} = \mathrm {180 J/K mol }{/tex} and body temperature is 300 K.

Question 55 : For a given reaction, {tex} \Delta H = 35.5 \ \mathrm { kJ }\ \mathrm { mol } ^ { - 1 } {/tex} and {tex} \Delta S = 83.6\ \mathrm { J }\ \mathrm { K } ^ { - 1 }\ \mathrm { mol } ^ { - 1 } {/tex} . The reaction is so spontaneous at (Assume that {tex} \Delta H {/tex} and {tex} \Delta S {/tex} do not vary with temperature.)

Question 56 : One mole of an ideal gas at 300{tex} \mathrm { K } {/tex} is expanded isothermally from an initial volume of 1 litre to 10 litres. The {tex} \Delta E {/tex} for this process is

Question 57 : Given :<br>(I){tex} { \mathrm { H } _ { 2 } ( \mathrm { g } ) + \frac { 1 } { 2 } \mathrm { O } _ { 2 } ( \mathrm { g } ) \rightarrow \mathrm { H } _ { 2 } \mathrm { O } ( l ) } \\ { \Delta \mathrm { H } ^ { \circ } _ { 298 \mathrm { K } } = - 285.9 \mathrm { kJ } \mathrm { mol } ^ { - 1 } } {/tex}<br>(II) {tex} \mathrm { H } _ { 2 } ( \mathrm { g } ) + \frac { 1 } { 2 } \mathrm { O } _ { 2 } ( \mathrm { g } ) \rightarrow \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { g } ) {/tex} <br>{tex} \Delta \mathrm { H } ^ { \circ } _ { 298 \mathrm { K } } = - 241.8 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex} <br>The molar enthalpy of vapourisation of water will be:<br>

Question 58 : Consider the following liquid -vapour equillibrium. Liquid {tex}\rightleftharpoons{/tex}Vapour<br>which of the following relations is correct?

Question 59 : Substance {tex} \mathrm { A } _ { 2 } \mathrm { B } ( \mathrm { g } ) {/tex} can undergoes decomposition to form two set of products:<br><img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5dfc68918701466b65e5eb85"><br>If the molar ratio of {tex} \mathrm {A_2(g)}{/tex} to {tex} \mathrm {A(g)}{/tex} is {tex}5 : 3{/tex} in a set of product gases, then the energy involved in the decomposition of 1 mole of {tex} \mathrm{ {A_2 B} (g)} {/tex} is :

Question 60 : When one mole of an ideal gas is compressed to half its initial volume and simultaneously heated to twice in initial temperature, the change in entropy {tex} ( \Delta \mathrm { S } ) {/tex} is

Question 61 : If the enthalpy change for the transition of liquid water to steam is 30kJ {tex}mol^{-1}{/tex} at {tex}27^\circ{/tex} C, the entropy change for the proces would be

Question 62 : Which of the following are not state functions?<br> {tex} \mathrm{(I)}\ q+w{/tex}<br> {tex} \mathrm{(II)}\ q{/tex}<br> {tex} \mathrm{(III)}\ w{/tex}<br>{tex} \mathrm{(IV)}\ H-TS {/tex}

Question 63 : Following reaction occurring in an automobile <br>{tex} 2 \mathrm { C } _ { 8 } \mathrm { H } _ { 18 ( g ) } + 25 \mathrm { O } _ { 2 ( g ) } \rightarrow 16 \mathrm { CO } _ { 2 ( g ) } + 18 \mathrm { H } _ { 2 } \mathrm { O } _ { ( g ) } {/tex}<br> The sign of {tex} \Delta H , \Delta S {/tex} and {tex} \Delta G {/tex} would be

Question 64 : The work done during the expansion of a gas from a volume of 4{tex}\ \mathrm { dm } ^ { 3 } {/tex} to 6{tex}\ \mathrm { dm } ^ { 3 } {/tex} against a constant external pressure of 3{tex}\ \mathrm { atm } {/tex} is {tex} ( 1\ \mathrm { L }\ \mathrm { atm } = 101.32\ \mathrm { J } ) {/tex}

Question 65 : Heat of neutralization of a strong acid {tex} \mathrm {HA } {/tex} and a weaker acid {tex} \mathrm {HB} {/tex} with {tex} \mathrm { KOH } {/tex} are {tex}- 13.7{/tex} and - {tex} 12.7 \mathrm{ \ { k } \ cal \ mol^{- 1}} {/tex} . When {tex}1{/tex} mole of {tex} \mathrm { KOH } {/tex} was added to a mixture containing {tex}{/tex} mole each of {tex} \mathrm {HA} {/tex} and {tex} \mathrm { HB } {/tex}, the heat change was {tex} - 13.5 \ \mathrm { kcal } {/tex}. In what ratio is the base distributed between {tex} \mathrm {HA } {/tex} and {tex} \mathrm {HB} {/tex}.

Question 66 : One mole of an ideal gas is expanded isothermally and reversibly to half of its initial pressure. {tex} \Delta \mathrm S {/tex} for the process in {tex} \mathrm { JK } ^ { - 1 } \mathrm { mol } ^ { - 1 } {/tex} is {tex} [ \ell \mathrm { n } 2 = 0.693 \text { and } R = 8.314 , \mathrm { J } / ( \mathrm { mol } \mathrm { K } ) ] {/tex}

Question 67 : Enthalpy of {tex} \mathrm { CH } _ { 4 } + 1 / 2 \mathrm { O } _ { 2 } \rightarrow \mathrm { CH } _ { 3 } \mathrm { OH } {/tex} is negative. If enthalpy of combustion of {tex} \mathrm { CH } _ { 4 } {/tex} and {tex} \mathrm { CH } _ { 3 } \mathrm { OH } {/tex} are {tex} x {/tex} and {tex} y {/tex} respectively. Then which relation is correct?

Question 68 : The molar enthalpies of combustion of isobutane and n-butane are {tex} - 2870 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex} and {tex} - 2878 \mathrm { kJ } {/tex} {tex} \mathrm { mol } ^ { - 1 } {/tex} respectively at {tex} 298 \mathrm { K } {/tex} and {tex} 1 \mathrm { atm } {/tex}. Calculate {tex} \Delta \mathrm { H } ^ { \circ } {/tex} for the conversion of {tex} 1 \ \mathrm { mole } {/tex} of n-butane to {tex} 1 \ \mathrm { mole } {/tex} of isobutane

Question 69 : Standard enthalpy and standard entropy changes for the oxidation of ammonia at {tex}298{/tex}{tex} \mathrm { K } {/tex} are {tex} - 382.64\ \mathrm { kJ }\ \mathrm { mol } ^ { - 1 } {/tex} and {tex} - 145.6\ \mathrm { kJ }\ \mathrm { mol } ^ { - 1 } , {/tex}respectively. Standard Gibb's energy change for the same reaction at {tex}298{/tex}{tex} \mathrm { K } {/tex} is

Question 70 : Given that {tex} C + O _ { 2 } \rightarrow C O _ { 2 } , \Delta H ^ { \circ } = - x\ \mathrm { kJ } {/tex} {tex} 2 \mathrm { CO } + \mathrm { O } _ { 2 } \rightarrow 2 \mathrm { CO } _ { 2 } , \Delta H ^ { \circ } = - y\ \mathrm { kJ } {/tex}. The enthalpy of formation of carbon monoxide will be

Question 71 : Standard enthalpy of combustion of {tex} \mathrm { CH } _ { 4 } {/tex} is {tex} - 890 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex} and standard enthalpy of vaporisation of water is {tex} 40.5 \mathrm { kJ } \mathrm { mol } ^ { - 1 } . {/tex} The enthalpy change of the reaction<br>{tex} \mathrm { CH } _ { 4 } ( \mathrm { g } ) + 2 \mathrm { O } _ { 2 } ( \mathrm { g } ) \longrightarrow \mathrm { CO } _ { 2 } ( \mathrm { g } ) + \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { g } ) {/tex}<br>

Question 72 : {tex}\mathrm{2Zn\ +\ O_2\ \rightarrow\ 2ZnO;\ \Delta}G^\circ = -616 \ \mathrm J {/tex}<br>{tex}\mathrm{2Zn\ +\ S_2\ \rightarrow\ 2ZnS;\ \Delta}G^\circ = -293 \ \mathrm J {/tex}<br>{tex}\mathrm{S_2\ +\ 2O_2\ \rightarrow\ 2SO_2;\ \Delta}G^\circ = -408 \ \mathrm J {/tex}<br>{tex}\Delta G^\circ {/tex} for the following reaction<br>{tex}\mathrm{2ZnS\ +\ 3O_2\ \rightarrow\ 2ZnO\ +\ 2SO_2} {/tex} is

Question 73 : For a particular reversible reaction at temperature T, ∆H and ∆S were found to be both +ve. If Te is the temperature at equilibrium, the reaction would be spontaneous when.

Question 74 : A gas expands adiabatically at constant pressure such that {tex} \mathrm { T } \propto \mathrm { V } ^ { - 1 / 2 } . {/tex} The value of {tex} \gamma \left( \mathrm { C } _ { \mathrm { p } , \mathrm { m } } / \mathrm { C } _ { \mathrm { v } , \mathrm { m } } \right) {/tex} of the gas will be:

Question 75 : Heat of combustion {tex} \Delta H {/tex} for {tex} C _ { ( s ) } , H _ { 2 ( g ) } {/tex} and {tex} C H _ { 4 ( g ) } {/tex} are {tex} - 94 , - 68 {/tex} and {tex} - 213 {/tex} kcal/mol, then {tex} \Delta H {/tex} for {tex} C _ { ( s ) } + 2 H _ { 2 ( g ) } \rightarrow C H _ { 4 ( g ) } {/tex} is

Question 76 : In a closed insulated container a liquid is stirred with a paddle to increase the temperature which of the following is true?

Question 77 : The enthalpy of neutralisation of a weak acid in {tex} 1 \mathrm { M } {/tex} solution with a strong base is {tex} - 56.1 \mathrm { kcal } {/tex} {tex} \mathrm { mol } ^ { - 1 } {/tex}. If the enthalpy of ionisation of acid is {tex} 1.5 \mathrm { kcal } \mathrm { mol } ^ { - 1 } {/tex} and enthalpy of neutralisation of the strong acid with a strong base is {tex} - {/tex} {tex} 57.3 \mathrm { kJ } \ \mathrm { eq } ^ { - 1 } . {/tex} What is the % ionisation of the weak acid in molar solution (assume the acid is monobasic)

Question 78 : The enthalpy of atomisation of {tex} \mathrm { CH } _ { 4 } {/tex} and {tex} \mathrm { C } _ { 2 } \mathrm { H } _ { 6 } {/tex} are {tex}360{/tex} and {tex} 620 \ \mathrm { kcal } \mathrm { mol } ^ { - 1 } {/tex} respectively. The {tex} \mathrm { C } - \mathrm { C } - \mathrm { C } {/tex} bond energy is expected to be

Question 79 : Enthalpy change for the reaction, {tex}4H(g) \rightarrow 2H_2 (g){/tex} is {tex}-869.6kJ{/tex} The dissociation energy of H-H bond is

Question 80 : Calculate the heat produced (in {tex} \mathrm {k J } ) {/tex} when {tex} 224 \mathrm { g } {/tex} of {tex} \mathrm { CaO } {/tex} is completely converted to {tex} \mathrm { CaCO } _ { 3 } \mathrm { by } {/tex} reaction with {tex} \mathrm { CO } _ { 2 } {/tex} at {tex} 27 ^ { \circ } \mathrm { C } {/tex} in a container of fixed volume.<br>Given {tex} : \Delta \mathrm { H } _ { f } ^ { \circ } \left( \mathrm { CaCO } _ { 3 } , \mathrm { s } \right) = - 1207 \mathrm { kJ } / \mathrm { mol } {/tex} {tex} \Delta \mathrm { H } _ { f } ^ { \circ } ( \mathrm { CaO } , \mathrm { s } ) = - 635 \mathrm { kJ } / \mathrm { mol } , \Delta \mathrm { H } _ { f } ^ { \circ } \left( \mathrm { CO } _ { 2 } , \mathrm { g } \right) = {/tex} {tex} \left. - 394 \mathrm { kJ } / \mathrm { mol } ; \quad \text { [Use } \mathrm { R } = 8.3 \mathrm { JK } ^ { - 1 } \mathrm { mol } ^ { - 1 } \right] {/tex}

Question 81 : 50 mL of water takes 5 min to evaporate from a vessel on a heater connected to an electric source which delivers 400 W. The enthalpy of vaporisation of water is

Question 82 : The heat of combustion of {tex} \mathrm { CH } _ { 4 } ( \mathrm { g } ) , \mathrm { C } {/tex} (graphite), {tex} \mathrm { H } _ { 2 } ( \mathrm { g } ) {/tex} are {tex} -20 \mathrm { kcal } , - 40 \mathrm { kcal } - 10 \mathrm { kcal } {/tex} respectively. The heat of formation of methane is

Question 83 : The heats of neutralisation of {tex} \mathrm { CH } _ { 3 } \mathrm { COOH } , \mathrm { HCOOH } , \mathrm { HCN } {/tex} and {tex} \mathrm { H } _ { 2 } \mathrm { S } {/tex} are {tex} - 13.2 , - 13.4 , - 2.9 {/tex} and {tex} - 3.8 \mathrm { kcal } {/tex} per equivalent respectively. Arrange the acids in increasing order of strength

Question 84 : The heat of atomization of {tex} \mathrm { PH } _ { 3 } ( \mathrm { g } ) {/tex} is {tex} 228 \mathrm { kcal } {/tex} {tex} \mathrm { mol } ^ { - 1 } {/tex} and that of {tex} \mathrm { P } _ { 2 } \mathrm { H } _ { 4 } ( \mathrm { g } ) {/tex} is {tex} 335 \mathrm { kcal } \mathrm { mol } ^ { - 1 } . {/tex} The energy of the {tex} \mathrm { P } - \mathrm { P } {/tex} bond is

Question 86 : If enthalpies of formation for C{tex}_2{/tex}H{tex}_{4(g)}{/tex},CO{tex}_{2(g)}{/tex} and H{tex}_2{/tex}O{tex}_{(\ell)}{/tex} at 25{tex}^\circ{/tex}C and 1 atm pressure are 52, -394 and -286 kJ/mol respectively, then enthalpy of combustion of C{tex}_2{/tex}H{tex}_{4(g)}{/tex} will be

Question 87 : In an irreversible process taking place at constant {tex} \mathrm {T } {/tex} and {tex} \mathrm { P } {/tex} and in which only pressure-volume work is being done, the change in Gibbs free energy {tex} \mathrm { (dG) } {/tex} and change in entropy {tex} \mathrm { (dS) } {/tex}, satisfy the criteria

Question 88 : The enthalpy of hydrogenation of cyclohexene is {tex} - 119.5 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex}. If resonance energy of benzene is {tex} - 150.4 \mathrm { kJ } \mathrm { mol } ^ { - 1 } , {/tex} its enthalpy of hydrogenation would be

Question 89 : The absolute enthalpy of neutralisation of the reaction: <br>{tex} \mathrm { MgO } _ { ( s ) } + 2 \mathrm { HCl } _ { ( a q ) } \rightarrow \mathrm { MgCl } _ { 2 ( a q ) } + \mathrm { H } _ { 2 } \mathrm { O } _ { ( \mathrm { l } ) } {/tex} will be

Question 90 : One mole of a non-ideal gas undergoes a change of state {tex} ( 2.0 \text { atm, } 3.0 \mathrm { L } , 95 \mathrm { K } ) \rightarrow ( 4.0 \mathrm { atm } , 5.0 \mathrm { L } , 245 \mathrm { K } ) {/tex} with a change in internal energy, {tex} \Delta \mathrm { U } = 30.0 \mathrm { Latm } . {/tex} The change in enthalpy {tex} \Delta \mathrm { H } {/tex} of the process in {tex} \mathrm { L } {/tex} atm is.

Question 91 : Hydrogen has an ionisation energy of {tex} 1311 \mathrm { kJ } {/tex} {tex} \mathrm { mol } ^ { - 1 } {/tex} and for chlorine it is {tex} 1256 \mathrm { kJ } \mathrm { mol } ^ { - 1 } . {/tex} Hydrogen forms {tex} \mathrm { H } ^ { + } ( \mathrm { aq } ) {/tex} ions but chlorine does not form {tex} \mathrm { Cl } ^ { + } ( \mathrm { aq } ) {/tex} ions because

Question 93 : For a particular reversible reaction at temperature {tex} T , \Delta H {/tex} and {tex} \Delta S {/tex} were found to be both + ve. If {tex} T _ { e } {/tex} is the temperature at equilibrium, the reaction would be spontaneous when

Question 94 : The free energy change for the following reactions are given below,<br> {tex} \mathrm { C } _ { 2 } \mathrm { H } _ { 2 } ( \mathrm { g } ) + \frac { 5 } { 2 } \mathrm { O } _ { 2 } ( \mathrm { g } ) \rightarrow {/tex}{tex} 2 \mathrm { CO } _ { 2 } ( \mathrm { g } ) \rightarrow \mathrm { CO } _ { 2 } ( \mathrm { g } ) ; \Delta \mathrm { G } ^ { \circ } = - 1234 \mathrm { kJ }{/tex} <br> {tex} \mathrm { C } ( \mathrm { g } ) + \mathrm { O } _ { 2 } ( \mathrm { g } ) \rightarrow \mathrm { CO } _ { 2 } ( \mathrm { g } ) ; \Delta \mathrm { G } ^ { \circ } = - 394 \mathrm { kJ } {/tex}<br> {tex} \mathrm { H } _ { 2 } ( \mathrm { g } ) + \frac { 1 } { 2 } \mathrm { O } _ { 2 } ( \mathrm { g } ) \rightarrow \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { l } ) ; \Delta \mathrm { G } ^ { \circ } = - 237 \mathrm { kJ } {/tex} <br>What is the standard free energy change for the reaction<br> {tex} \mathrm { H } _ { 2 } ( \mathrm { g } ) + 2 \mathrm { C } ( \mathrm { s } ) \longrightarrow \mathrm { C } _ { 2 } \mathrm { H } _ { 2 } ( \mathrm { g } ) {/tex}

Question 95 : Standard entropies of {tex}\mathrm X_2, \mathrm Y_2{/tex} and {tex} \mathrm {XY_3 } {/tex} are {tex}60, 40{/tex} and {tex}50{/tex} {tex}\mathrm{J K}{/tex} {tex}^{-1} {/tex} {tex}\mathrm {mol^{-1}} {/tex} respectively. For the reaction {tex}1/2\mathrm X_2 + 3/2\mathrm Y_2 \rightleftharpoons \mathrm {XY}_3, \Delta H = -\mathrm {30\ kJ} {/tex} to be at equilibrium, the temperature should be

Question 96 : The bond dissociation energies of {tex} \mathrm { CH } _ { 4 } {/tex} and {tex} \mathrm { C } _ { 2 } \mathrm { H } _ { 6 } {/tex} respectively are 360 and 620 {tex} \mathrm { kcal mol } ^ { - 1 } {/tex}. The C-C bond energy would be :- -

Question 97 : Three thermochemical equations are given below<br>(i) C{tex}_{(graphite)} + O{tex}_{2(g)}{/tex} {tex} \rightarrow {/tex}CO{tex}_{2(g)}{/tex};{tex}\Delta{/tex},{tex}H^\circ{/tex} = {tex}x{/tex} kJ mol{tex}^{-1}{/tex} <br>(ii) C{tex}_{(graphite)} +1/2\ O{tex}_{2(g)}{/tex} {tex} \rightarrow {/tex}CO{tex}_{(g)}{/tex};{tex}\Delta{/tex},{tex}H^\circ{/tex} = {tex}y{/tex} kJ mol{tex}^{-1}{/tex} <br>(iii) CO{tex}_{(g)} +1/2\ O{tex}_{2(g)}{/tex} {tex} \rightarrow {/tex}CO{tex}_{2(g)}{/tex};{tex}\Delta{/tex},{tex}H^\circ{/tex} = {tex}z{/tex} kJ mol{tex}^{-1}{/tex}<br>Based on the above equations, find out which of the relationship given below is correct.<br>

Question 98 : Consider the following processes:<br>{tex} 1 / 2 \mathrm { A } \rightarrow \mathrm { B } \quad + 150 {/tex}<br> {tex} 3 \mathrm { B } \rightarrow 2 \mathrm { C } + \mathrm { D } - 125 {/tex}<br> {tex} \mathrm { E } + \mathrm { A } \rightarrow 2 \mathrm { D } \quad + 350 {/tex}<br> For {tex} \mathrm { B } + \mathrm { D } \rightarrow \mathrm { E } + 2 \mathrm { C } , \Delta \mathrm { H } {/tex} will be:<br>

Question 99 : Consider the following reactions:<br> {tex}\mathrm {(i)}\ \mathrm{ H^+}_{(aq)} + \mathrm{ OH^-}_{(aq)} = \mathrm{ H_2O_{(l)}}, \ \Delta H = -X_1\ \mathrm {{kJ}\ mol^{-1}} {/tex}<br> {tex}\mathrm {(ii)}\ \mathrm{ H}_{2(g)} + \mathrm{ 1/2 O}_{2(g)} = \mathrm{ H_2O_{(l)}}, \ \Delta H = -X_2\ \mathrm {{kJ}\ mol^{-1}} {/tex} <br>{tex}\mathrm {(iii)}\ \mathrm{ CO}_{2(g)} + \mathrm{ H}_{2(g)} = \mathrm{ CO_{(g)} + \mathrm{ H_2O_{(l)}}}, \ \Delta H = -X_3\ \mathrm {{kJ}\ mol^{-1}} {/tex} <br>{tex}\mathrm {(iv)}\ \mathrm{C_2 H}_{2(g)} + \mathrm{ 5/2O}_{2(g)} = \mathrm{2CO_{2(g)} + \mathrm{ H_2O_{(l)}}}, \ \Delta H = +X_4\ \mathrm {{kJ}\ mol^{-1}} {/tex} <br> Enthalpy of formation of {tex}\mathrm {H_2O}_{(l)}{/tex} is

Question 100 : Standard enthalpy of vaporisation {tex} \Delta _ { \mathrm { vap } } H ^ { \circ } {/tex} for water at {tex} 100 ^ { \circ } \mathrm { C } {/tex} is {tex} 40.66\ \mathrm { kJ }\ \mathrm { mol } ^ { - 1 } . {/tex} The internal energy of vaporisation of water at {tex} 100 ^ { \circ } \mathrm { C } {/tex} {tex} \left. \text {(in } \mathrm { kJ }\ \mathrm { mol } ^ { - 1 } \right) {/tex} is <br> (Assume water vapour to behave like an ideal gas)

Question 102 : What is the value of change in internal energy at 1 atm in the process?<br>{tex} \mathrm { H } _ { 2 } \mathrm { O } ( 1,323 \mathrm { K } ) \longrightarrow \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { g } , 423 \mathrm { K } ) {/tex} <br>Given : {tex} \mathrm { C } _ { \mathrm { v } , \mathrm { m } } \left( \mathrm { H } _ { 2 } \mathrm { O } , \mathrm { l } \right) = 75.0 \mathrm { JK } ^ { - 1 } \mathrm { mol } ^ { - 1 } {/tex}<br> {tex} \mathrm { C } _ { \mathrm { p } , \mathrm { m } } \left( \mathrm { H } _ { 2 } \mathrm { O } , \mathrm { g } \right) = 33.314 \mathrm { JK } ^ { - 1 } \mathrm { mol } ^ { - 1 } {/tex}<br> {tex} \Delta \mathrm { H } _ { \mathrm { vap } } {/tex} at {tex} 373 \mathrm { K } = 40.7 \mathrm { kJ } / \mathrm { mol } {/tex}<br>

Question 103 : Bond dissociation enthalpy of {tex} \mathrm { H } _ { 2 } , \mathrm { Cl } _ { 2 } {/tex} and {tex} \mathrm { HCl } {/tex} are {tex} 434,242 {/tex} and {tex}431\ \mathrm { mol } ^ { - 1 } {/tex}respectively. Enthalpy of formation of {tex} \mathrm { HCl } {/tex} is

Question 104 : For the reaction taking place at certain temperature {tex} \mathrm { NH } _ { 2 } \mathrm { COONH } _ { 4 } ( \mathrm { s } ) \rightleftharpoons 2 \mathrm { NH } _ { 3 } ( \mathrm { g } ) + \mathrm { CO } _ { 2 } ( \mathrm { g } ) {/tex} if equilibrium pressure is {tex} 3 \mathrm { X } {/tex} bar then {tex} \Delta _ { \mathrm { r } } \mathrm { G } ^ { \circ } {/tex} would be

Question 105 : {tex} \Delta \mathrm { H } _ { \mathrm { f } } ^ { \mathrm { o } } {/tex} of water is {tex} - 285.8 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex}. If enthalpy of neutralisation of monoacidic strong base is {tex} - 57.3 \mathrm { kJmol } ^ { - 1 } . \Delta \mathrm { H } _ { \mathrm { f } } ^ { \circ } {/tex} of {tex} \mathrm { OH } ^ { - } {/tex} ion will be

Question 106 : The following two reactions are known:<br>{tex} \mathrm { Fe } _ { 2 } \mathrm { O } _ { 3 } ( s ) + 3 \mathrm { CO } ( g ) \longrightarrow 2 \mathrm { Fe } ( s ) + 3 \mathrm { CO } _ { 2 } ( g ) ; \Delta \mathrm { H } = - 26.8 \mathrm { kJ } {/tex} {tex} \mathrm { FeO } ( s ) + \mathrm { CO } ( g ) \longrightarrow \mathrm { Fe } ( s ) + \mathrm { CO } _ { 2 } ( g ) ; \Delta \mathrm { H } = - 16.5 \mathrm { kJ } {/tex}<br>The value of {tex} \Delta \mathrm { H } {/tex} for the following reaction {tex} \mathrm { Fe } _ { 2 } \mathrm { O } _ { 3 } ( s ) + \mathrm { CO } ( g ) \longrightarrow 2 \mathrm { FeO } ( s ) + \mathrm { CO } _ { 2 } ( g ) \mathrm { is } {/tex}

Question 107 : A sample of an ideal gas in a cyclinder is compressed adiabatically to {tex}\frac13{/tex}rd of its volume. Will final pressure be more or less than {tex}3\times{/tex} the initial pressure?

Question 108 : The heat of combustion of carbon to {tex} \mathrm { CO } _ { 2 } {/tex} is {tex} - 393.5 \mathrm { kJ } / \mathrm { mol } . {/tex} The heat released upon formation of {tex} \mathrm { 35.2 g } {/tex} of {tex} \mathrm { CO } _ { 2 } {/tex} from carbon and oxygen gas is

Question 109 : The standard enthalpies of formation of {tex} \mathrm { CO } _ { 2 } ( \mathrm { g } ) , \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { I } ) {/tex} and glucose(s) at {tex} 25 ^ { \circ } \mathrm { C } {/tex} are {tex} - 400 \mathrm { kJ } / \mathrm { mol } , - 300 \mathrm { kJ } / \mathrm { mol } {/tex} and {tex} - 1300 {/tex} {tex} \mathrm { kJ } / \mathrm { mol } , {/tex} respectively. The standard enthalpy of combustion of glucose at {tex} 25 ^ { \circ } \mathrm { C } {/tex} is

Question 110 : The enthalpy of neutralisation of {tex} \mathrm { NH } _ { 4 } \mathrm { OH } {/tex} and {tex} \mathrm { CH } _ { 3 } \mathrm { COOH } {/tex} is {tex} - 10.5 \mathrm { kcal } \mathrm { mol } ^ { - 1 } {/tex} and enthalpy of neutralisation of {tex} \mathrm { CH } _ { 3 } \mathrm { COOH } {/tex} with strong base is {tex} - 12.5 \mathrm { kcal } \mathrm { mol } ^ { - 1 } . {/tex} The enthalpy of ionisation of {tex} \mathrm { NH } _ { 4 } \mathrm { OH } {/tex} will be

Question 111 : Using the data provided, calculate the multiple bond energy {tex} \left( \mathrm { k } \mathrm { J } \mathrm { mol } ^ { - 1 } \right) {/tex} of a {tex} \mathrm { C } \equiv \mathrm { C } {/tex} bond in {tex} \mathrm { C } _ { 2 } \mathrm { H } _ { 2 } . {/tex} That energy is (take the bond energy of a {tex}\mathrm { C } - \mathrm { H } {/tex} bond as {tex} 350 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex} )<br>{tex} 2 \mathrm { C } ( s ) + \mathrm { H } _ { 2 } ( g ) \longrightarrow \mathrm { HC } \equiv \mathrm { CH } ( g ) ;\ \Delta \mathrm { H } = 225 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex}<br> {tex} 2 \mathrm { C } ( s ) \longrightarrow 2 \mathrm { C } ( g ) ;\ \Delta \mathrm { H } = 1410 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex}<br> {tex} \mathrm { H } _ { 2 } ( g ) \longrightarrow 2 \mathrm { H } ( g ) ;\ \Delta \mathrm { H } = 330 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex}<br>

Question 112 : When 5 litres of a gas mixture of methane and propane is perfectly combusted at 0{tex}^{\circ}{/tex}C and 1 atmosphere, 16 litres of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion in kJ ({tex}\Delta H_{comb.}{/tex}(CH{tex}_4{/tex}) = 890 kJ mol{tex}^{-1}{/tex}, {tex}\Delta H_{comb.}{/tex}(C{tex}_3{/tex}H{tex}_8{/tex})= 2220 kJ mol{tex}^{-1}{/tex} is

Question 113 : {tex} \Delta \mathrm { H } _ { \mathrm { f } } ^ { \circ } {/tex} of {tex} \mathrm { NF } _ { 3 } {/tex} is {tex} - 113 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex} and {tex} \mathrm { N } - \mathrm { F } {/tex} bond energy is {tex} 273.0 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex}. If {tex} \mathrm { N } \equiv \mathrm { N } {/tex} and {tex} \mathrm { F } - \mathrm { F } {/tex} bond energies are in the rates {tex} 6: 1 , {/tex} their magnitudes will be

Question 114 : The process, in which no heat enters or leaves the system is termed as

Question 115 : The standard enthalpy of formation of {tex} \mathrm { NH } _ { 3 } {/tex} is {tex} - 46.0 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex}. If the enthalpy of formation of {tex} \mathrm { H } _ { 2 } {/tex} from its atoms is {tex} - 436 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex} and that of {tex} \mathrm { N } _ { 2 }{/tex} is {tex}- 712 \mathrm { kJ } \mathrm { mol } ^ { - 1 } , {/tex} the average bond enthalpy of {tex} \mathrm { N } - \mathrm { H } {/tex} bond in {tex} \mathrm { NH } _ { 3 } {/tex} is

Question 116 : For the combustion reaction at {tex} 298 \mathrm { K } {/tex} {tex} 2 \mathrm { Ag } ( \mathrm { s } ) + 1 / 2 \mathrm { O } _ { 2 } ( \mathrm { g } ) \longrightarrow 2 \mathrm { Ag } _ { 2 } \mathrm { O } ( \mathrm { s } ) {/tex}<br> Which of the following alternatives is correct?

Question 117 : The enthalpy change of formation of {tex} \mathrm { CO } _ { 2 } ( \mathrm { g } ) {/tex} is {tex} - 393 \mathrm { kJmol } ^ { - 1 } {/tex} and that of {tex} \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { l } ) {/tex} is {tex} - 286 \mathrm { kJmol } ^ { - 1 } . {/tex} The enthalpy of combustion of one mole of ethanol {tex} \left( \mathrm { C } _ { 2 } \mathrm { H } _ { 5 } \mathrm { OH } \right) {/tex} is {tex} - 1360 . {/tex} The enthalpy change for the formation of one mole of ethanol form its constituent elements is

Question 118 : For which of the following process, {tex} \Delta \mathrm S {/tex} is negative?

Question 119 : Which of the following assumption of kinetic molecular theory states that gases do not have fixed shape?

Question 120 : The densities of graphite and diamond at 298{tex}\ \mathrm { K } {/tex} are 2.25 and 3.31{tex}\ \mathrm { g }\ \mathrm { cm } ^ { - 3 } , {/tex}respectively. If the standard free energy difference {tex} \left( \Delta G ^ { \circ } \right) {/tex} is equal to 1895{tex}\ \mathrm { J }\ \mathrm { mol } ^ { - 1 } {/tex}, the pressure at which graphite will be transformed into diamond at 298{tex}\ \mathrm { K } {/tex} is

Question 121 : The difference between heats of reaction at constant pressure and constant volume for the reaction :<br>{tex} 2 \mathrm { C } _ { 6 } \mathrm { H } _ { 6 } ( \mathrm { l } ) + 15 \mathrm { O } _ { 2 } ( \mathrm { g } ) \rightarrow 12 \mathrm { CO } _ { 2 } ( \mathrm { g } ) + 6 \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { l } ) {/tex} at {tex} 25 ^ { \circ } \mathrm { C } {/tex} in {tex} \mathrm { kJ } {/tex} is<br>

Question 122 : Assuming that water vapour is an ideal gas, the internal energy change ( {tex} \Delta \mathrm { U } ) {/tex} when {tex} 1 \mathrm { mol } {/tex} of water is vapourised at {tex} 1 \mathrm { bar } {/tex} pressure and {tex} 100 ^ { \circ } \mathrm { C } {/tex}, (given : molar enthalpy of vapourisation of wa- ter at {tex} 1 \mathrm { bar } {/tex} and {tex} 373 \mathrm { K } = 41 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex} and {tex} \mathrm { R } = 8.3 \mathrm { J } \mathrm { mol } ^ { - 1 } \mathrm { K } ^ { - 1 } {/tex} ) will be

Question 123 : The {tex} \Delta \mathrm { H } {/tex} at {tex} 358 \mathrm { K } {/tex} for the reaction {tex} \mathrm { Fe } _ { 2 } \mathrm { O } _ { 3 } ( \mathrm { s } ) + 3 \mathrm { H } _ { 2 } ( \mathrm { g } ) \longrightarrow 2 \mathrm { Fe } ( \mathrm { s } ) + 3 \mathrm { H } _ { 2 } \mathrm { O } ( l ) {/tex} given that {tex} \Delta \mathrm { H } _ { 298 } = - 33.29 \mathrm { kJmol } ^ { - 1 } {/tex} and {tex} \mathrm { C } _ { \mathrm { p } } {/tex} for {tex} \mathrm { Fe } _ { 2 } \mathrm { O } _ { 3 } ( \mathrm { s } ) {/tex} {tex} \mathrm { Fe } ( \mathrm { s } ) , \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { l } ) {/tex} and {tex} \mathrm { H } _ { 2 } ( \mathrm { g } ) {/tex} and {tex} 103.8,25.1,75.3 {/tex} and {tex} 28.8 \mathrm { J } / \mathrm { Kmol } {/tex}

Question 124 : Equal volumes of methanoic acid and sodium hydroxide are mixed. If {tex}\mathrm x {/tex} is the heat of formation of water, then heat evolved on neutralization is

Question 125 : The amount of energy released when {tex} 20 \mathrm { mL } {/tex} of {tex} 0.5 \mathrm { M } {/tex} {tex} \mathrm {NaOH}{/tex} are mixed with {tex} 100 \mathrm { mL } {/tex} of {tex} 0.1 \mathrm { M } {/tex} {tex} \mathrm { HCl } {/tex} is {tex} { x } {/tex} kJ. The heat of neutralisation (in {tex} \left. \mathrm {kJ\ mol } ^ { - 1 } \right) {/tex} is

Question 126 : The lattice energy of solid {tex} \mathrm { NaCl } {/tex} is {tex} 180 \mathrm { kcal } \mathrm {\ mol } ^ { - 1 } {/tex} and enthalpy of solution is {tex}1\mathrm{ kcal}{/tex} {tex} \mathrm {\ mol } ^ { - 1 } {/tex}. If the hydration energies of {tex} \mathrm { Na } ^ { + } {/tex} and {tex} \mathrm { Cl } ^ { - } {/tex} ions are in the ratio {tex} 3: 2 , {/tex} what is the enthalpy of hydration of sodium ion?

Question 127 : Match the columns<br> <table> <tr><th>Column I </th> <th>Column II </th> </tr> <tr><td>A. {tex}\mathrm {C_4H_{10}+\frac{13}{2}O_2\rightarrow4CO_2+5H_2O};\Delta H=-w {/tex}</td> <td>I.Enthalpy of atomisation</td> </tr> <tr><td>B.{tex}\mathrm {CH_4\rightarrow C+4H}; \Delta H= x{/tex}</td> <td>II.Enthalpy of formation</td> </tr> <tr><td>C. {tex}\mathrm {H_2+Br_2\rightarrow 2HBr};\Delta H= y{/tex}</td> <td>III.Enthalpy of combustion</td> </tr> <tr><td>D. {tex}\mathrm {Na^-(s)\rightarrow Na(g); \Delta H= z}{/tex}</td> <td>IV. Enthalpy of sublimation</td> </tr> </table>

Question 128 : The enthalpy of neutralisation of a weak acid in {tex} 1 \mathrm { M } {/tex} solution with a strong base is {tex} - 56.1 \mathrm { kcal } \mathrm { mol } ^ { - 1 } {/tex}. If the enthalpy of ionisation of acid is {tex} 1.5 \mathrm { kcal } \mathrm { mol } ^ { - 1 } {/tex} and enthalpy of neutralisation of the strong acid with a strong base is {tex} - 57.3 {/tex} {tex} \mathrm { kJeq } ^ { - 1 } . {/tex} What is the % ionisation of the weak acid in molar solution (assume the acid is monobasic)

Question 130 : Given that:<br> (i) {tex} \Delta _ { \mathrm { f } } \mathrm { H } ^ { \circ } {/tex} of {tex} \mathrm { N } _ { 2 } \mathrm { O } {/tex} is {tex} 82 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex}<br> (ii) Bond energies of {tex} \mathrm { N } \equiv \mathrm { N } , \mathrm { N } = \mathrm { N } , \mathrm { O } = \mathrm { O } {/tex} and {tex} \mathrm { N } = \mathrm { O } {/tex} are {tex} 946,418,498 {/tex} and {tex} 607 \mathrm { kJ } {/tex} {tex} \mathrm { mol } ^ { - 1 } {/tex} respectively, <br>The resonance energy of {tex} \mathrm { N } _ { 2 } \mathrm { O } {/tex} is:

Question 131 : {tex} \mathrm { PbO } _ { 2 } \rightarrow \mathrm { PbO } ; \Delta G _ { 298 } < 0 {/tex}<br> {tex} \mathrm { SnO } _ { 2 } \rightarrow \operatorname { SnO } ; \Delta G _ { 228 } > 0 {/tex}<br> Most probable oxidation state of {tex} \mathrm { Pb } {/tex} and {tex} \mathrm { Sn } {/tex} will be

Question 132 : The enthalpy of neutralisation of {tex} \mathrm { NH } _ { 4 } \mathrm { OH } {/tex} with {tex} \mathrm { HCl } {/tex} is {tex} - 51.46 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex} and the enthalpy of neutralisation of {tex} \mathrm { NaOH } {/tex} with {tex} \mathrm { HCl } {/tex} is {tex} - 55.90 {/tex} {tex} \mathrm { kJ } \mathrm { mol } ^ { - 1 } . {/tex} The enthalpy of ionisation of {tex} \mathrm { NH } _ { 4 } \mathrm { OH } {/tex} is

Question 133 : A certain reaction is non spontaneous at {tex} 298 \mathrm { K } {/tex}. The entropy change during the reaction is {tex} 121 \mathrm { JK } ^ { - 1 } {/tex}. If the reaction is endothermic or exothermic, the minimum value of {tex} \Delta \mathrm { H } {/tex} for the reaction is

Question 134 : Boron can undergo the following reactions with the given enthalpy changes:<br>{tex} 2 \mathrm { B } ( \mathrm { s } ) + \frac { 3 } { 2 } \mathrm { O } _ { 2 } ( \mathrm { g } ) \longrightarrow \mathrm { B } _ { 2 } \mathrm { O } _ { 3 } ( \mathrm { s } ) , \Delta \mathrm { H } = - 1260 \mathrm { kJ } {/tex} <br>{tex} 2 \mathrm { B } ( \mathrm { s } ) + 3 \mathrm { H } _ { 2 } ( \mathrm { g } ) \longrightarrow \mathrm { B } _ { 2 } \mathrm { H } _ { 6 } ( \mathrm { g } ) ; \Delta \mathrm { H } = 30 \mathrm { kJ } {/tex} <br>Assume no other reactions are occurring.<br>If in a container (operating at constant pressure) which is isolated from the surrounding, mixture of {tex} \mathrm { H } _ { 2 } ( \text { gas) and } \mathrm { O } _ { 2 } {/tex} (gas) are passed over excess of {tex} \mathrm { B } ( \mathrm { s } ) {/tex}, then calculate the molar ratio {tex} \left( \mathrm { O } _ { 2 }: \mathrm { H } _ { 2 } \right) {/tex} so that temperature of the container do not change:

Question 135 : Diborane is a potential rocket fuel which undergoes combustion according to the equation {tex} \mathrm { B } _ { 2 } \mathrm { H } _ { 6 } ( \mathrm { g } ) + 3 \mathrm { O } _ { 2 } ( \mathrm { s } ) \longrightarrow \mathrm { B } _ { 2 } \mathrm { O } _ { 3 } ( \mathrm { s } ) + 3 \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { g } ) {/tex} Calculate the enthalpy change for the combustion of diborane. Given<br><img style='object-fit:contain' src="https://data-screenshots.sgp1.digitaloceanspaces.com/5dfc98bbee7a9376db8896b7.jpg" /><br><img style='object-fit:contain' src="https://data-screenshots.sgp1.digitaloceanspaces.com/5dfc98a894c4c577246c5072.jpg" />

Question 136 : When {tex}1{/tex} mole of oxalic acid is treated with excess of {tex} \mathrm { NaOH } {/tex} in dilute aqueous solution, {tex} 106 \mathrm { kJ } {/tex} of heat is liberated. Predict the enthalpy of ionisation of the acid

Question 137 : From the following bond energies: <br>{tex} \mathrm { H } - \mathrm { H } {/tex} bond energy: {tex} 431.37 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex}<br> {tex} \mathrm { C } = \mathrm { C } {/tex} bond energy. {tex} 606.10 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex} <br>{tex} \mathrm { C } - \mathrm { C } {/tex} bond energy: {tex} 336.49 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex}<br> {tex} \mathrm { C } - \mathrm { H } {/tex} bond energy. {tex} 410.50 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex} <br>Enthalpy for the reaction,<br> <img style='object-fit:contain' src='https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7d94f399925718ac6b238' class="uploaded-image" /> <br> will be

Question 138 : {tex}2{/tex} mole of ideal gas at {tex} 27 ^ { \circ } \mathrm { C } {/tex} temperature is expanded reversibly from {tex}2{/tex} lit. to {tex}20{/tex} lit. Find entropy change. {tex} ( \mathrm R = 2\ \mathrm { cal } / \mathrm { mol }\ \mathrm { K } ) {/tex}