Question 1 :
Among cellulose, polyvinyl chloride, nylon and natural rubber, in which of the polymer intermolecular force of attraction is weakest?

Question 2 :
The valency of Cr in the complex $\left[ \mathrm { Cr } \left( \mathrm { H } _ { 2 } \mathrm { O } \right) _ { 4 } \mathrm { Cl } _ { 2 } \right] ^ { + }$

Question 3 :
Assertion: Transition metals show variable valence. Reason: Due to a large energy difference between the $ ns^2 $ and $ ( n - 1)d $ electrons.

Question 4 :
The oxidation state of Barium in $Ba({ H }_{ 2 }{ PO }_{ 2 }{ ) }_{ 2 }$  is:

Question 5 :
$0.7\ g$ of $Na_{2}CO_{3}. xH_{2}O$ is dissolved in $100\ ml, 20\ ml$ of which required $19.8\ ml$ of $0.1\ N\ HCl$. The value of $x$ is:

Question 7 :
Which of the following is not a property of an ionic compound?

Question 8 :
$KF$ combines with $HF$ to form $KHF_2$. The compound contains the species:

Question 9 :
In which of the following pairs, the two species are isostructural?

Question 10 :
The bond dissociation energy of {tex} \mathrm { B } - \mathrm { F } {/tex} in {tex} \mathrm { BF } _ { 1 } {/tex} is {tex} 646 \mathrm { kJ } \mathrm { mol } ^ { - 1 } {/tex} whereas that of {tex} \mathrm { C } - \mathrm { F } {/tex} in {tex} \mathrm { CF } _ { 4 } {/tex} is {tex} 515 {/tex} {tex} \mathrm { kJ } \mathrm { mol } ^ { - 1 } . {/tex} The correct reason for higher {tex} \mathrm { B } - \mathrm { F } {/tex} bond dissociation energy as compared to that of {tex} \mathrm { C } - \mathrm { F } {/tex} is

Question 11 :
Assertion: Ionic bonds are directional in nature whereas covalent bonds are non-directional. Reason: According to orbital overlap concept, the formation of a covalent bond between two atoms results by pairing of electrons present in the valence shell having same spins.

Question 12 :
Which of the following family form negative ions in an ionic bond?

Question 14 :
Which of the following sets of characteristics leads to the increase in solubility of ionic substances?

Question 21 :
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 22 :
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 23 :
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 24 :
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 25 :
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 26 :
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 27 :
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 28 :
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 29 :
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 30 :
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 31 :
When $2$ g of gas A is introduced into an evacuated flask kept at $25^oC$, the pressure was found to be $1$ atmosphere. If $3$ g of another gas B is then added to the same flask, the pressure becomes $1.5$ atm. Assuming ideal behaviour, the ratio of molecular weights $(M_B:M_A)$ is :

Question 32 :
When a drop of liquid splits up into a number of drops.

Question 33 :
At STP, determine the amount of oxygen in liters that can be prepared from the decomposition of $212$ grams of sodium chlorate($1$ mol$=106$g).

Question 34 :
Consider a vessel filled with carbodioxide at $27^{\circ}C$ and $5$ atmospheric pressure. A part of the gas is removed at $27^{\circ}C$ and it fills a $3L$ container at $1\ atm$ and the pressure drops to $3.5\ atm$ in the vessel. The volume of the vessel is:

Question 35 :
A gaseous mixture of ethene, ethane and methane having total volume $150\ ml$&#160;is subjected to combustion in excess of oxygen. If percentage of methane in the original mixture is $20\%$&#160;then calculate volume (in ml) of $C{ O }_{ 2 }\left( g \right)$&#160;which will be obtained at same temperature and pressure.

Question 36 :
The volume of $HCl$ passed through the solution at ${25}^{o}C$ and $1$ atm is:

Question 37 :
An open vessel containing air at 27$^o$C is heated to 127$^o$C. The fraction of air originally present in the bottle that is expelled is:

Question 38 :
The gaseous reaction $A_{(g)} \rightarrow 2B_{(g)} + C_{(g)}$ is found to be first order with respect to $A$. If the reaction is started with $p_{A} = 90\ mmHg$, the pressure after $10$ minutes found to be $180\ mmHg$. The rate constant of the reaction is?

Question 39 :
At STP, a gas that contains $6.02\times 10^{23}$ atoms and it forms diatomic molecules will occupy&#160;:

Question 40 :
When $2$ g of gas A is introduced into an evacuated flask kept at $25^oC$, the pressure was found to be $1$ atm. If $3$ g of another gas B is then added to the same flask containing A, the pressure becomes $1.5$ atm. Assuming ideal behaviour, the ratio of molecular weights $(M_A:M_B)$ is&#160;:

Question 41 :
$0.303$ g of the organic compound in Duma's method on combustion gave $32.27$ ml of moist nitrogen at $27^{\circ}$C and at P mm of Hg pressure. The vapour pressure at $ 27^{\circ}$C is $21$ mm of Hg. Find the value of P.

Question 43 :
The force which exists between particle of same kind of substance called cohesion force.

Question 44 :
$0.40\ g$ of helium in a bulb at a temperature of $T\ K$ had a pressure of $p$ atm. When the bulb was immersed in water bath at temperature $50\ K$ more than the first one, $0.08\ g$ of gas had to be removed to restore the original pressure. The temperature $T$ is:

Question 45 :
The relative strength of interionic/ intermolecular forces in decreasing order is :