Question 1 :
$ \Delta U^{ \ominus } $ of combustion of methane is $ -X kJ mol^{-1} $ The value of $ \Delta H^{ \ominus } $ is
Question 3 :
When hydrochloric acid is added to cobalt nitrate solution at room temperature, the following reaction takes place and the reaction mixture becomes blue. On cooling the mixture, it becomes pink. On the basis of this information mark the correct answer.<br>$[Co(H_{2}O)_{6}]^{3+}(aq)(pink)+4Cl^{-}(aq)\leftrightharpoons [CoCl_{4}]^{2-}(aq)(blue)+6H_{2}O(l)$<br>
Question 4 :
For the reaction of one mole zinc dust with one mole sulphuric acid in a bomb calorimeter, $\triangle U$ and w correspond to?<br/>
Question 5 :
For the reaction: <br/>${ C }_{ 2 }{ H }_{ 4 }(g)+3{ O }_{ 2 }(g)\rightarrow 2C{ O }_{ 2 }(g)+2{ H }_{ 2 }O(l)$<br/>$\Delta E=-1415KJ$. The $\Delta H$ at $27C$ is:
Question 7 :
For the reaction of one-mole zinc dust with one more sulphuric acid in a bomb calorimeter, $\Delta U$ and $w$ correspond to:<br/>[Hint: In bomb calorimeter, $w=0, \Delta U=q$ ($-ve$)]
Question 8 :
For the reaction of one mole of zinc dust with one mole of sulphuric acid in a bomb calorimeter, $\triangle U$ and $w$ corresponds to:
Question 10 :
How much energy is needed to melt $100g$ of water?<br/>$\Delta {H}_{v}=540\ cal/g$<br/>$\Delta {H}_{f}=80\ cal/g$<br/>${C}_{water}=1\ cal/{g}^{o}C$
Question 11 :
Given:<br/>$C(s)+{O}_{2}(g)\rightarrow {CO}_{2}(g)+94.2kcal$<br/>${H}_{2}(g)+\cfrac{1}{2}{O}_{2}(g)\rightarrow {H}_{2}O(l)+68.3kcal$<br/>${CH}_{4}+2{O}_{2}(g)\rightarrow {CO}_{2}(g)+2{H}_{2}O(l)+210.8kcal$<br/>The heat of formation of methane in $kcal$ will be:
Question 12 :
For the reaction of one mole of zinc dust with one mole of sulphuric acid in a bomb calorimeter $\Delta U$ and w correspond to
Question 14 :
A diatomic ideal gas is expanded at constant at pressure. If work done by the system is $10 \,J$ then calculate heat absorbed.
Question 15 :
Which of the following relationships is not correct for the reaction between $\Delta H$ and $\Delta U$?
Question 17 :
<span>$\Delta H_{f}=$ -98.2 K.Cal/mole<br/>$S_{Na} =$ 36 K.Cal/mole<br/>$I_{Na} =$ 118.5 K.Cal/mole<br/>$\dfrac{1}{2}D_{Cl_{2}}=$ 29 K.Cal/mole<br/>$U_{NaCl}=$ -184.2 K.Cal/mole<br/></span><span>From the data given below for $NaCl$, the electron </span><span>affinity of chlorine $[-E_{a}]$ is:</span><span><br/></span>
Question 18 :
"The change of enthalpy of a chemical reaction is the same whether the reaction takes place in one step or in several steps". This law was presented by:
Question 20 :
Metabolism is the stepwise breakdown of the food we eat to provide energy for growth<br/>and function. A general overall equation for this complex process represents the<br/>degradation of glucose $(C_{6}H_{12}O_{6})$   to   $CO_{2}$    and   $H_{2}O$. This metabolic process involves many<br/>steps and its enthalpy $(\Delta H)$ is called the enthalpy of combustion. This is because the same<br/>quantity of heat is evolved whether we burn 1 mole of glucose in air or let the metabolic<br/>process break it down. Which of the following equations can be used to calculate the<br/>standard enthalpy of the metabolic process correctly?<br/>
Question 22 :
Calculate the heat of formation of methane, given that<br>heat of formation of water $=-286kJ\quad { mol }^{ -1 }$<br>heat of combustion of methane $=-890kJ\quad { mol }^{ -1 }$<br>heat of combustion of carbon $=-393.5kJ\quad { mol }^{ -1 }$
Question 24 :
Calorific value of ${ H }_{ 2 }$ gas is x kJ/gm. What is heat of formation of ${ H }_{ 2 }O$ ?
Question 25 :
Consider the reaction at $300$K.<br>$H_2(g)+Cl_2(g)\rightarrow 2HCl(g);$ $\Delta H^o=-185$kJ<br>If $2$ mole of $H_2$ completely react with $2$ mole of $Cl_2$ to form HCl. What is $\Delta U^o$ for the reaction?<br>
Question 26 :
Given that:<br/>$2Fe(s)+\cfrac { 3 }{ 2 } { O }_{ 2 }(g)\longrightarrow { Fe }_{ 2 }{ O }_{ 3 }(s);\Delta H=-193.4kJ...(i)$<br/>$Mg(s)+\cfrac { 1 }{ 2 } { O }_{ 2 }(g)\longrightarrow MgO(s);\Delta H=-140.2kJ....(ii)$<br/>What is $\Delta H$ of the reaction?<br/>$3Mg+{ Fe }_{ 2 }{ O }_{ 3 }\longrightarrow 3MgO+2Fe$
Question 27 :
If melting one mole of ice to water requires $6 $ kJ of enthalpy, then freezing of water to two mole of ice will require ________ kJ of energy.
Question 28 :
Hess' Law and bond energy data can be used to calculate the enthalpy change of a reaction. Bromoethane, $CH_2CH_2Br$, can be made by reacting ethene with hydrogen bromide.<br>$CH_2=CH_2+HBr\rightarrow CH_3CH_2Br$<br>What is the enthalpy change for this reaction?<br>
Question 29 :
If $\triangle H_{vaporisation}$ of substance $X(l)$ (molar mass: $30\ g/mol)$ is $300\ J/g$ at it's boiling point $300\ K$, then molar entropy change for reversible condensation process is____________.
Question 30 :
For which one of the following system $\Delta E < \Delta H$?
Question 31 : <div><span>Chemical reaction is invariably associated with the transfer of energy either in the form of heat or light. In the laboratory, </span><span>heat changes in physical and chemical processes are measured with an instrument called Calorimeter. Heat change </span><span>in the process is calculated as :</span></div><div><br/><blockquote>$q = ms\Delta T$ ........ $s= specific\quad heat$<br/>  $= c\Delta T$ ....... $c= heat\quad capacity$</blockquote><blockquote><br/>Heat of reaction at constant volume is measured using bomb Calorimeter.<br/>$q_V = \Delta U = $internal energy change</blockquote><blockquote><br/>Heat of reaction at constant pressure is measured using bomb Calorimeter.<br/>$q_P = \Delta H$<br/>$q_P = q_V + P\Delta V$<br/>$\Delta H = \Delta U + \Delta nRT$</blockquote></div>The heat capacity of a bomb calorimeter is $500  J  K^{ -1 }$. When $0.1  g$ of Methane was burnt in this calorimeter, the temperature rose by $2^{ \circ }C$. The value of $\Delta U$ per mole will be :<br/>
Question 32 :
$\Delta { U }^{ o }$ of combustion of methane is $-X$ $kJ$ ${ mol }^{ -1 }$. The value of $\Delta { H }^{ o }$ is:
Question 33 : The energy of an electron in the ground state of $H$ atom is $-13.6eV$.<div><br/>The negative sign indicates that:</div>
Question 34 :
The equilibrium constant of a reaction at $298K$ is $5\times {10}^{-3}$ and at $1000K$ is $2\times {10}^{-5}$. What is the sign of $\Delta H$ for the reaction?
Question 35 :
The value of $\Delta E$ for combustion of 16 g of $CH_4$ is -885389 J at 298 K. The $\Delta H$ combustion for $CH_4$ in J $mol^{-1}$ at this temperature will be: $(Given that, R \, = \, 8.314 \, JK^{-1} \, mol^{-1})$
Question 36 :
Hess's law is applicable for the determination of heat of ________.
Question 37 :
The enthalpy changes for two reactions are given by the equations:<br>$2Cr(s)+1\cfrac { 1 }{ 2 } { O }_{ 2 }(g)\longrightarrow { Cr }_{ 2 }{ O }_{ 3 }(s);\Delta H=-1130kJ$<br>$C(s)+\cfrac { 1 }{ 2 } { O }_{ 2 }(g)\longrightarrow CO(g);\Delta H=-110kJ$<br>What is the enthalpy change, in $kJ$, for the reaction?<br>$3C(s)+{ Cr }_{ 2 }{ O }_{ 3 }(s)\longrightarrow 2Cr(s)+3CO(g)$
Question 38 :
<span>Based on the first law of thermodynamics, which one of the following is correct ?</span>
Question 39 :  For the reactions,<br/><div><span>(i) ${H}_{2}(g)+{Cl}_{2}(g)=2HCl(g)+x$ $kJ$</span><br/></div><div><br/></div><div>(ii) ${H}_{2}(g)+{Cl}_{2}(g)=2HCl(l)+y$ $kJ$<br/><br/></div><div>which one of the following statements is correct?</div>
Question 40 :
A bomb calorimeter is used to measure the value of heat of reaction at a constant <br>
Question 41 : Consider the reaction at $300\ K$, <span>$H_{2}(g) + Cl_{2}(g)\rightarrow 2HCl(g), \ \ \ \Delta H^{\circ} = -185\ kJ$</span><div>If $3$ mole of $H_{2}$ completely reacts with $3$ mole of $Cl_{2}$ to form $HCl$, What is $\Delta U^{\circ}$ for this reaction?</div>
Question 42 :
If $\Delta {H}_{f}^{o}$ for ${H}_{2}{O}_{2}(l)$ and ${H}_{2}O(l)$ are $-188kJ$ ${mol}^{-1}$ and $-286kJ$ ${mol}^{-1}$, what will be the enthalpy change of the reaction?<br/>$2{H}_{2}{O}_{2}(l)\rightarrow 2{H}_{2}O(l)+{O}_{2}(g)$
Question 43 :
Two mole of an ideal gas is heated at constant pressure of one atomosphere from $27^\circ$C to $127^\circ$C. If $C_{v,m}\, =\, 20\, +\, 10^{-2}\, T\, JK^{-1}\, mol^{-1}$, then $q$ and $\Delta U$ for the process are respectively.
Question 44 :
In an isobaric process ratio of heat supplied to the system, to workdone by the system for diatomic gas is:
Question 45 :
Heat of formation of $H_2O$ (g) at $25^0C$ is -243 KJ. $\Delta U$ for the reaction $H_2 (g) + \frac{1}{2} O_2  (g) \rightarrow H_2O (g) $ at $25^0C$ is:
Question 46 :
Heat of combustion $\Delta H^o$ for $C(s), H_2(g)$ and $CH_4(g)$ are $-94,-68$ and $-213 kcal/mol$ respectively. Then $\Delta H^o$  for $C(s) + 2H_2(g) \rightarrow CH_4$ is:
Question 47 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">Hess's law of constant heat summation is based on</p></span></span>
Question 49 : <div>$C(s) + O_2(g) \to CO_2(g); \quad \Delta H = -94kcal$</div><div><br/></div><div>$2CO(g) + O_2(g) \to 2CO_2(g); \quad \Delta H = -135.2 kcal$</div><div><br/></div><div>The heat of formation of $CO(g)$ is :</div>
Question 50 :
Specific heat capacity of lead is $120\space J\space kg^{-1}\space K^{-1}$. When $7200J$ of heat is supplied to $5kg$ of lead, the rise in temperature is
Question 51 :
The heat of combustion of ethanol determined in a bomb calorimeter is $-670.48kcal$ ${mol}^{-1}$ at $298K$. What is the $\Delta U$ at $298K$ for the reaction?
Question 52 : Calculate enthalpy for formation of ethylene from the following data:<div><br/>(I) $C(graphite) + O_2 (g) \rightarrow CO_2 (g); \ \ \ \Delta H = -393.5 kJ$<br/>(II) $H_2(g) + \dfrac{1}{2} O_2 (g) \rightarrow H_2O(l); \ \ \ \ \Delta H = - 286.2 kJ$<br/>(III) $C_2H_4(g) + 3O_2(g) \rightarrow 2CO_2(g)  + 2H_2 O(l); \ \ \ \   \Delta H = - 1410.8 kJ$</div>
Question 53 : 4 grams of sodium hydroxide pellets were dissolved in $100  {cm}^{3}$ of water. The temperature before adding the sodium hydroxide pellets was 25 degrees C, and after adding the pellets it was 35 degrees C. Calculate the enthalpy change in ${kJ}/{mole}$ of the reaction.<div><span>[Specific heat capacity of water $= 4.2  {J}/{k}/{g}]$</span><br/></div>
Question 55 :
<span>How many joules of heat are absorbed when 70.0 g of water is completely vaporised at its boiling point ?</span><br/><span>[Take : L</span><span>V</span><span> = 2260 kJ / kg]</span>
Question 56 : Given that:<br/>(i) $C$ (graphite)$+O_2(g)\rightarrow CO_2(g)$; $\quad \Delta _rH^o=x\ kJ mol^{-1}$.<br/>(ii) $C$ (graphite)$+\dfrac{1}{2}O_2(g)\rightarrow CO(g)$; $\quad \Delta _rH^o=y\ kJ mol^{-1}$<br/>(iii) $CO(g)+\dfrac{1}{2}O_2(g)\rightarrow CO_2(g)$; $\quad \Delta _rH^o=z\ kJ mol^{-1}$<br/><br/><div>Based on the given thermochemical equations, find out which one of the following algebraic relationships is correct?<br/></div>
Question 57 : Following are the thermochemical reactions:<br/>$C$ (graphite) $+ \dfrac{1}{2}O_2  \rightarrow CO \ ;  \Delta H = - 110.5$ kJ/mol<br/>$CO + \dfrac{1}{2} O_2  \rightarrow CO_2 \ ;  \Delta H = - 283.2$ kJ/mol<div>The heat of reaction (in kJ/mol) for the following reaction is:</div><div><span>$C (\text{graphite})  + O_2  \rightarrow CO_2$</span></div>
Question 59 : Using the data provided, calculate the multiple bond energy (kJ / mol) of a $C=C$ bond in $C_{2}H_{2}$.  (Take the bond energy of a C-H bond as 350 kJ / mol)<br/><br/>$2C(s) + H_{2}(g) \rightarrow C_{2}H_{2}(g)$ $\Delta H = 225 kJ / mol$ <div>$2C(s)\rightarrow 2C(g);\Delta H= 1410kJ mol^{-1}$</div><div>$H_2(g)\rightarrow 2H(g);\Delta H= 330kJ mol^{-1}$</div>
Question 60 :
The heat energy of $743J$ is needed to raise the temperature of $5$ moles of an ideal gas by $2K$ at constant pressure. How much heat energy is needed to raise the temperature of the same mass of the gas by $2K$ at constant volume?
Question 61 :
In conversion of line-stone to lime,<br>$Ca{CO}_{3}(s)\rightarrow CaO(s)+{CO}_{2}(g)$<br>the values of $\Delta {H}^{o}$ and $\Delta {S}^{o}$ are $+179.1kJ{mol}^{-1}$ and $160.2J/K$ respectively at $298K$ and $1$ bar. Assuming that $\Delta {H}^{o}$ and $\Delta {S}^{o}$ do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is:
Question 62 :
The reaction $NH_{2}CN(s) + \dfrac {3}{2}O_{2}(g) \rightarrow N_{2}(g) + CO_{2}(g) + H_{2}O(l)$ was carried out at $300\ k$ in a bomb calorimeter. The heat released was $742\ kJ\ mol^{-1}$. The value of $\triangle H_{300K}$ for this reaction would be_________.
Question 63 :
What can be used in combination with a calorimeter to compare the specific heats of two substances?
Question 64 :
In an ice calorimeter, a chemical reaction is allowed to occur in thermal contact with an ice-water mixture at $0^{o}C$. Any heat liberated by the reaction is used to melt some ice; the volume change of the ice-water mixture indicates the amount of melting. When solutions containing $1.0$ millimole each of $AgNO_{3}$ and $NaCl$ were mixed in such a calorimeter, both solution having been pre-cooled to $0^{o}C$, $0.20\ g$ of ice-melted. Assuming complete reaction in this experiment, what is $\Delta H$ for the reactions: $Ag^{+}(aq)+Cl^{-}(aq)\rightarrow AgCl(s)$ ? Latent heat of fusion of ice at $0^{o}C$ is $80\ cal/g$.
Question 65 : Calculate ${ \Delta H }/{ kJ }$ for the following reaction using the listed standard enthalpy of reaction data.<br/>$2{ N }_{ 2 }\left( g \right) +5{ O }_{ 2 }\left( g \right) \longrightarrow 2{ N }_{ 2 }{ O }_{ 5 }\left( s \right) $<div><br/>${ N }_{ 2 }\left( g \right) +3{ O }_{ 2 }\left( g \right) +{ H }_{ 2 }\left( g \right) \longrightarrow 2HN{ O }_{ 3 }\left( aq \right)    ;        \           { \Delta H }/{ kJ }=-414.0$<br/><br/></div><div>${ N }_{ 2 }{ O }_{ 5 }\left( s \right) +{ H }_{ 2 }O\left( l \right) \longrightarrow 2HN{ O }_{ 3 }\left( aq \right)                  ;    \       { \Delta H }/{ kJ }=-86.0$<br/><br/></div><div>$2{ H }_{ 2 }\left( g \right) +{ O }_{ 2 }\left( g \right) \longrightarrow 2{ H }_{ 2 }O\left( l \right)                     ;      \    { \Delta H }/{ kJ }=-571.6$</div>
Question 66 :
If the bond dissociation energy of $XY,\ X_2,\ Y_2$ (all are gaseous diatomic molecules) are in the ratio of 1:1:0.5 and enthalpy for the formation of $XY$ is -200kJ/mol. The bond dissociation energy of $X_2$ will be:
Question 67 : Given, <div>$C(s)+{O}_{2}(g)\rightarrow {CO}_{2}(g); \Delta H=-395\ kJ$<br/>$S(s)+{O}_{2}(g)\rightarrow {SO}_{2}(g);\Delta H=-295\ kJ$<br/>$C{S}_{2}(l)+3{O}_{2}(g)\rightarrow {CO}_{2}(g)+2{SO}_{2}(g);\Delta H=-1110\ kJ$<br/><br/></div><div>The heat of formation of $C{S}_{2}(l)$ is:</div>
Question 68 : Determine ${ \Delta H }/{ kJ }$ for the following reaction using the listed enthalpies of reaction:<br/>$4CO\left( g \right) +8{ H }_{ 2 }\left( g \right) \longrightarrow 3C{ H }_{ 4 }\left( g \right) +C{ O }_{ 2 }\left( g \right) +2{ H }_{ 2 }O\left( l \right) $<div><br/>$C\left( graphite \right) +{ 1 }/{ 2 }{ O }_{ 2 }\left( g \right) \longrightarrow CO\left( g \right) ;                           { \Delta H }/{ kJ }=-110.5kJ$</div><div><br/>$CO\left( g \right) +{ 1 }/{ 2 }{ O }_{ 2 }\left( g \right) \longrightarrow C{ O }_{ 2 }\left( g \right)         ;                 { \Delta H }/{ kJ }=-282.9kJ$</div><div><br/>${ H }_{ 2 }\left( g \right) +{ 1 }/{ 2 }{ O }_{ 2 }\left( g \right) \longrightarrow { H }_{ 2 }O\left( l \right)        ;                   { \Delta H }/{ kJ }=-285.8kJ$</div><div><br/>$C\left( graphite \right) +2{ H }_{ 2 }\left( g \right) \longrightarrow C{ H }_{ 4 }\left( g \right)           ;                       { \Delta H }/{ kJ }=-74.8kJ$</div>
Question 69 :
Statement 1: The $\Delta H_{reaction}$ of a particular reaction can be arrived at by the summation of the $\Delta H_{reaction}$ values of two or more reactions that, added together, will give the $\Delta H_{reaction}$ of the particular reaction.<br/>Statement 2: Hess's Law conforms to the First Law of Thermodynamics, which states that the total energy of the universe is a constant.
Question 70 : For the reaction  : <div><br/><div>$3N_{2} + H_{2} \rightarrow 2NH_{3}$,   </div><div><br/></div><div>$\triangle H = - 24 kcal$ at $427^{0}C$ and $200 atm$</div><div><br/></div><div>Calculate magnitude of internal enerrgy change in $Kcal$ ($\triangle U$), if 168 g $N_{2}$ gas and 30 g $H_{2}$ gas are allowed to react completely (100% reaction yield) to form $NH_{3}$ gas at $427^{0}C$ and 200 atm. </div></div>
Question 71 :
For gas $'A'$ in a calorimeter heat evolved is $250\ kJ. mol^{-1}$. For $0.2$ mol of $A$, temperature rise from $298 K$ to $ 300 K$. Find out capacity of calorimeter.
Question 72 :
The enthalpy of combustion of methane, graphite and dihydrogen at $298K$ are $-890.3$ $kJ{ mol }^{ -1 },-393.5$ $kJ{ mol }^{ -1 },-285.8$ $kJ { mol }^{ -1 }$ respectively. Enthalpy of formation of ${CH}_{4(g)}$ will be:
Question 73 :
Based on the following thermochemical equations<br>${H}_{2}(g)+C(s)\longrightarrow CO(g)+{H}_{2}(g)$; $\Delta H=133kJ {mol}^{-1}$<br>$CO(g)+\cfrac{1}{2}{O}_{2}(g)\longrightarrow {CO}_{2}(g)$; $\Delta H=-282kJ{mol}^{-1}$<br>${H}_{2}(g)+\cfrac{1}{2}{O}_{2}(g)\longrightarrow {H}_{2}O(g)$; $\Delta H=-242kJ{mol}^{-1}$<br>$C(s)+{O}_{2}(g)\longrightarrow {CO}_{2}(g)$; $\Delta H=xkJ{mol}^{-1}$<br>The value of $x$ will be:
Question 74 : <span>Determine ${ \Delta H }/{ kJ }$ for the following reaction using the listed enthalpies of reaction:</span><br/><span>$4CO\left( g \right) +8{ H }_{ 2 }\left( g \right) \longrightarrow 3C{ H }_{ 4 }\left( g \right) +C{ O }_{ 2 }\left( g \right) +2{ H }_{ 2 }O\left( l \right) $</span><br/><span><br/></span><div><span>Given that</span></div><div><span>$C\left( graphite \right) +{ 1 }/{ 2 }{ O }_{ 2 }\left( g \right) \longrightarrow CO\left( g \right)    ;        \                { \Delta H }/{ kJ }=-110.5kJ$</span><br/><span><br/></span></div><div><span>$CO\left( g \right) +{ 1 }/{ 2 }{ O }_{ 2 }\left( g \right) \longrightarrow C{ O }_{ 2 }\left( g \right)      ;\                    { \Delta H }/{ kJ }=-282.9kJ$</span><br/><span><br/></span></div><div><span>${ H }_{ 2 }\left( g \right) +{ 1 }/{ 2 }{ O }_{ 2 }\left( g \right) \longrightarrow { H }_{ 2 }O\left( l \right)     ;\                      { \Delta H }/{ kJ }=-285.8kJ$</span><br/><span><br/></span></div><div><span>$C\left( graphite \right) +2{ H }_{ 2 }\left( g \right) \longrightarrow C{ H }_{ 4 }\left( g \right)       ;\                           { \Delta H }/{ kJ }=-74.8kJ$</span><br/></div>
Question 75 :
$(CH_3)_2CH + Cl_2 \longrightarrow (CH_3)_2CHCl + Cl$<br>$CH_3CH_2CH_2 - H$ $98$<br>$(CH_3)_2CH - H$ $95$<br>$Cl - Cl$ $58$<br>$H - Cl$ $103$<br>$CH_3CH_2CH_2 - Cl$ $81$<br>$(CH_3)_2CH -Cl$ $80$<br>Given the bond dissociation energies below (in $kcal/mole$), estimate the ${ \Delta H }^{ o }$ for the propagation step:<br>
Question 76 :
The heat of reaction for $A + \frac{1}{2} O_2  \rightarrow AO$ is $-50$ kcal/mol and $AO + \frac{1}{2} O_2  \rightarrow AO_2$ is $100$ kcal/mol.<br/>The heat of reaction (in kcal/mol) for $A + O_2  \rightarrow AO_2$ will be:
Question 77 :
1 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/g-deg. What is the molar heat of decomposition for $NH_4NO_3$?<br>
Question 78 : $C+O_{2}\rightarrow CO_{2}+94.2 kcal$<br/>$H_{2}+1/2O_{2}\rightarrow H_{2}O+68.3 kcal$<br/><p>$CH_{4}+2O_{2}\rightarrow CO_{2}+2H_{2}O\left ( g \right<br/>)+210.8kcal$</p><p>Then the possible heat of formation of methane will be </p>
Question 79 :
When $0.2$ mole of ethane is burnt completely in a bomb calorimeter, the temperature of calorimeter system increased by $2\ K$. What should be the increase in temperature of the same calorimeter system, when $0.4$ mole of ${CH}_{4}$ is burnt?<br>Given: ${ \Delta }_{ C }{ U_{ { C }_{ 2 }{ H }_{ 6 }(g) } }=-400\ Kcal/mol$ and ${ \Delta }_{ c }U_{ CH_{ 4 }\left( g \right) }=-200\ Kcal/mol$.<br>
Question 80 :
If $\Delta {H}_{vaporisation}$ of substance $X(l)$ (molar mass :$30g/mol$) is $300J/g$ at its boiling point $300K$, then molar entropy change for reversible condensation process is:
Question 81 :
When we take acetone in a test tube it feels cold. Which reaction occurs in the process?
Question 82 :
What will be the heat formation of methane; if the heat of combustion of carbon is '$-x$' $kJ$, heat of formation of water is '$-y$' $kJ$ and heat of combustion of methane is '$-z$' $kJ$?
Question 83 : Calculate ${ \Delta H }/{ kJ }$ for the following reaction using the listed standard enthalpy of reaction data:<div>                       $2{ N }_{ 2 }\left( g \right) +5{ O }_{ 2 }\left( g \right) \longrightarrow 2{ N }_{ 2 }{ O }_{ 5 }\left( s \right) $</div><div><br/>${ N }_{ 2 }\left( g \right) +3{ O }_{ 2 }\left( g \right) +{ H }_{ 2 }\left( g \right) \longrightarrow 2HN{ O }_{ 3 }\left( aq \right)                       { \Delta H }/{ kJ }=-414.0$</div><div><br/></div><div>${ N }_{ 2 }{ O }_{ 5 }\left( s \right) +{ H }_{ 2 }O\left( I \right) \longrightarrow 2HN{ O }_{ 3 }\left( aq \right)                             { \Delta H }/{ kJ }=-86.0$</div><div><br/></div><div>$2{ H }_{ 2 }\left( g \right) +{ O }_{ 2 }\left( g \right) \longrightarrow 2{ H }_{ 2 }O\left( I \right)                               { \Delta H }/{ kJ }=-571.6$</div>
Question 84 : Assuming that water vapour is an ideal gas, the internal energy change ($\Delta U$) when $1mol$ of water is vaporised at $1$ bar pressure and ${100}^{o}C$ will be:<div>(Given: Molar enthalpy of vapourisation of water at $1$ bar and $373K=41\ kJ.{mol}^{-1}$ and $R=8.3J{mol}^{-1}$ ${K}^{-1}$)</div>
Question 86 :
The statement "The change of enthalpy of a chemical reaction is same whether the reaction takes place in one or several steps" is
Question 87 :
$\Delta U^{0}$ of  combustion of $CH_{4(g)}$ at certain temperature is $-393\ kJ mol ^{-1}$. The value $\Delta H^{o}$ is 
Question 88 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">Match the list -I with list - II.</p></span></span><b><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">List-I List - II</p></span></span></b><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">A) Hess law is not applicable for 1) is not a state function</p><p class="wysiwyg-text-align-left">B) All combustion reactions are 2) Heat of dilution</p><p class="wysiwyg-text-align-left">C) Work 3) Exothermic</p><p class="wysiwyg-text-align-left">D) Difference between two integral 4) Nuclear reaction</p><p class="wysiwyg-text-align-left"> heats of solutions</p></span></span>
Question 89 :
The enthaply change on freezing of $1\ mol$ of water at $10^ {o}C$ to ice at $-10^ {o}C$ is:
Question 92 :
The enthalpy of hydrogenation of benzene is $-49.8\ kcal/mol$ while its resonance energy is $36.0\ kcal/mol$. The enthalpy of formation of benzene is:<br>
Question 93 : $NX$ is produced by the following step of reactions:<br/><div>$M+{ X }_{ 2 }\longrightarrow M{ X }_{ 2 }$<br/></div><div>$3M{ X }_{ 2 }+{ X }_{ 2 }\longrightarrow { M }_{ 3 }{ X }_{ 8 }$<br/></div><div>${ M }_{ 3 }{ X }_{ 8 }+{ N }_{ 2 }{ CO }_{ 3 }\longrightarrow NX+{ CO }_{ 2 }+{ M }_{ 3 }{ O }_{ 4 }$<br/></div><div>How much $M$ (metal) is consumed to produce $206gm$ of $NX$?<div>(Take atomic weight of $M=56,N=23,X=80$)</div></div>
Question 94 :
For a reaction. $A(g)\rightarrow A(l);\Delta {H}=-3RT$. The correct statement for the reaction is:
Question 95 : Given: $S+\dfrac { 3 }{ 2 } { O }_{ 2 }\longrightarrow S{ O }_{ 3 }+2x$ $kcal$<br/>           $S{ O }_{ 2 }+\dfrac { 1 }{ 2 } { O }_{ 2 }\longrightarrow S{ O }_{ 3 }+y$ $kcal$<div><br/>With the help of the above reactions, find out the heat of formation of $S{ O }_{ 2 }$.</div>
Question 96 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">A coffee cup calorimeter initially contains 125g of water at a temperature of $24.2^{0}C$. After 10.5gm solute is added to the water at the same temperature, the final temperature becomes $21.1^{0}C$. The heat of solution is:<br/></p>
Question 97 :
Consider the following reactions. In which case the formation of product is favoured by decrease in pressure?<br/>(1) $CO_2(g)+C(s) \rightarrow  2CO(g)$; $\Delta H=+172.5$ kJ<br/>(2) $N_2(g)+3H_2(g) \rightarrow  2NH_3(g)$; $\Delta H=-91.8$ kJ<br/>(3) $N_2(g)+O_2(g) \rightarrow  2NO(g)$; $\Delta H=+181$ kJ<br/>(4) $2H_2O(g) \rightarrow 2H_2(g)+O_2(g); \Delta H=484.6$ kJ
Question 98 :
Given that the bond energies of $:N\equiv N$ is $946$ kJ $mol^{-1}$ $H-H$ is $435 $ kJ $mol^{-1}$, $N-N$ is $159$ kJ $mol^{-1}$, and $N-H$ is $389$ kJ $mol^{-1}$, the heat of formation of hydrazine in the gas phase in kJ $mol^{-1}$ is:<br/>
Question 99 :
If ${H}_{2}+\cfrac{1}{2}{O}_{2}\rightarrow {H}_{2}O;\Delta H=-68.09kcal$<br>$K+{H}_{2}O+water \rightarrow KOH(aq.)+\cfrac{1}{2}{H}_{2};\Delta H=-48.0kcal$<br>$KOH+water\rightarrow KOH(aq); \Delta H=-14.0kcal$<br>the heat of formation of $KOH$ is:
Question 100 :
Standard heats of formation for $C{Cl}_{4},{H}_{2}O,{CO}_{2}$ and $HCl$ at $298K$ are $-25.5,-57.8,-94.1$ and $-22.1kJ/mol$ respectively.<br/>For the reaction, what will be $\Delta H$?<br/>$C{Cl}_{4}+2{H}_{2}O\rightarrow {CO}_{2}+4HCl$
Question 101 : Consider the following processes.<br/><table class="wysiwyg-table"><tbody><tr><td></td><td>$\Delta H (kJ/mol)$</td></tr><tr><td>$1/2A\rightarrow B$</td><td>+150</td></tr><tr><td>$3B\rightarrow 2C+D$</td><td>-125</td></tr><tr><td>$E+A\rightarrow 2D$</td><td>+350</td></tr></tbody></table>For $B+D\rightarrow E+2C, \Delta H$ will be:
