Question 8 : Assertion: $Bi{Cl}_{5}$ does not exist.
Reason: In $Bi$ inert pair effect is predominant.<div><br/></div><div>Read the above assertion and reason and choose the correct option regarding it.</div>
Question 9 :
In which of the following arrangements, the sequence is not strictly according to the property written against it?<br>
Question 10 :
An element X combines with hydrogen to form a compound $XH_3$. The element X is placed on the right side ofthe periodic table. What is true about the element X?<br>A. Has 3 valence electrons.<br>B. Is a metal and is solid.<br>C. Is a non-metal and is a gas.<br>D. Has 5 valence electrons.<br>E. $XH_3$ reacts with water to form a basic compound?<br>
Question 11 :
The mole fraction of solute in 10% (w/w) aqueous NaOH solution is:
Question 12 :
If we take 44g of ${ CO }_{ 2 }$ and 14g of ${ N }_{ 2 }$ , what will be the mole fraction of ${ CO }_{ 2 }$ in the mixture?
Question 13 :
The sum of mole fractions of solute and solvent of a solution is equal to:
Question 14 :
One kilogram of sea water sample contains $6\ mg$ of dissolved $O_{2}$. The concentration of $O_{2}$ in the sample in ppm is:
Question 15 :
The sum of mole fractions of solute and solvent of a solution is equal to:
Question 16 :
Which of the following are homogenous in nature ?<br>(i) Ice<br>(ii) Wood<br>(iii) Soil <br>(iv) Air
Question 17 :
The mole fraction of solute in a solution is 0.3 . The mole percent of solvent is:
Question 18 :
If 3.65 g of $HCl$ is dissolved in 16.2 g of water then the mole fraction of $HCl$ is 0.9.
Question 19 :
$Y$ molal solution of a compound in benzene has mole fraction of solute equal to $0.2$. The value of ?
Question 20 :
Assertion: The solubility of a solid in a liquid increases with increase of pressure.
Reason: Solubility of gas in a liquid is directly proportional to the pressure of the gas.
Question 21 :
At $300 \,K$, when a solute is added to a solvent its vapour pressure over the mercury reduces from $50 \,mm$ to $45 \,mm.$ The value of mole fraction of solute will be
Question 22 :
The number of moles of $KCl$ in $1000\ ml$ water of $3$ molar solution is :
Question 23 :
A sample of $H_2O_2$ solution labelled as $28$ volume has density of $265$ g/L. Mark the correct option(s) representing concentration of same solution in other units.<br>
Question 25 :
A solution contains 1 mole of water and 4 moles of ethanol. The mole fraction of water and ethanol will be:
Question 26 :
When an ideal binary solution is in equilibrium with its vapour, molar ratio of the two components in the solution and in the vapour phases is
Question 27 : Oleum is considered as a solution of $SO_3$ in $H_2SO_4$. Which is obtained by passing $SO_3$ in solution of $H_2SO_4$.When 100 g sample of oleum is diluted with desired weight of $H_2O$ then the total mass of $H_2SO_4$.obtained after dilution is known as labelling of oleum. <br/><br/><div>For example , a oleum is diluted by 9 g of $H_2O$ which combined with all the free $SO_3$ to form $H_2SO_4$ as:<br/>$SO_3 +H_2O \rightarrow H_2SO_4$.<br/><br/>What is the % of free $SO_3$ in an oleum that is labelled as 104.5 % $H_2SO_4$?</div>
Question 28 :
Assertion: A solution is a homogeneous mixture of two or more chemically non-reacting substances
Reason: Solution is prepared by the combination of two same phases of matter.
Question 29 :
What is the mass percentage of carbon tetrachloride if $22 g$ of benzene is dissolved in $122$ $g$ of carbon tetrachloride? 
Question 30 :
$10$ g of NaCl is dissolved in $250$ g water. The correct way to express concentration of NaCl in solution are<span> :</span>
Question 31 :
$10$ L of hard water required $0.56$ g of lime (CaO) for removing hardness. Hence, the temporary hardness in ppm (part per million) of $CaCO_3$ is :
Question 33 :
$2.0\ g$ mixture of sodium carbonate and sodium bicarbonate on heating to constant weight gave $224\ mL$ of $CO_{2}$ at N.T.P.<br>The $\%$ weight of sodium bicarbonate in the mixture is:
Question 34 :
An amount of $1$ mole of $N_2$ and $4$ moles of $H_2$ are allowed to react in a vessel and after reaction, water is added. Aqueous solution required $1$ mole of $HCl$ for complete reaction. Mole fraction of $H_2$ in the gas mixture after reaction is
Question 35 :
The hardness of water sample which contains $0.001$ mol $ MgSO_{4}$ per litre of water is:<br/>
Question 36 :
Mole fraction of $I_2$ in $C_6H_6$ is 0.2. The molality of $I_2$ in  $C_6H_6$<span> is:</span>
Question 37 :
What is the mole fraction of the solute in a $1.00$ m aqueous solution?
Question 38 :
Solution of $100ml$ water contains $0.73g$ of $Mg(HCO_3)_2$ and $0.81g$ of $Ca(HCO_3)_2$. Calculate the hardness in terms of ppm of $CaCO_3$.
Question 39 :
Assuming that concentration of ${Ca}^{2+}$ ions in solution is in equal equivalence ratio to chloride ions, the hardness of water is<span> :</span>
Question 40 :
The mole fraction of water in 98% (w/w) $H_2SO_4$ solution is :
Question 41 :
The IUPAC name of haloalkane is always written as a ______ word. 
Question 46 :
The starting material for the manufacture of polyvinyl chloride is obtained by reacting $HCl$ with:
Question 47 :
Which major product is formed in the free-radical bromination of methane by limited supply of bromine?
Question 48 :
The organic compound obtained during the addition of $HBr$ to propene in the presence of peroxide catalyst is:
Question 51 :
$HBr$ reacts with $CH_{2} = CH - OCH_{3}$ under anhydrous conditions at room temperature to give:
Question 54 :
$2$-methyl butane on reaction with $Br_{2}$ in the presence of sunlight mainly gives:<br>
Question 55 :
Assertion: Statement-I : free radical chlorination of $n$-butane gives $72\%$ of $2$-chlorobutane and $28\%$ of $1$-chlorobutane though it has six primary and four secondary hydrogens. <br> Because
Reason: Statement-II : A secondary hydrogen is abstracted more easily than the primary hydrogen.
Question 56 :
In which of the following cases $C-C$ bond length will be the longest?
Question 57 :
Action hydrogen chloride on $CH_3 - \underset{CH_3}{\underset{|}{C}} = CH_2$ and $CH \equiv CH$ will predominantly give the compounds, respectively
Question 58 :
Ethyl alcohol reacts at a faster rate with $HI$ than with $HCl$ in forming the corresponding ethyl halides under identical conditions mainly because:
Question 59 :
Anisole can be prepared by the action of methyl iodide on sodium phenate. The reaction is called:
Question 60 :
Haloalkanes contain halogen atom (s) attached to the $ sp^{3} $ hybridised carbon atom of an alkyl group. Identify haloalkane from the following compounds.
Question 62 :
Which of the followin are used as free radical chain initiators?
Question 63 :
A solution of $(R)-2-$iodobutane, $[\alpha]= 15.9^{\circ}$ in acetone is treated with radioactive iodied, until $1.0$% of iodobutane contain radioactive iodine, the specific rotation of recovered iodobutane is found to be $-15.58^{\circ},$ which statement is correct about above information?
Question 65 : Assertion: Addition of one equivalent of $HCl$ to 1,3-butadiene at ${80}^{o}C$ gives 3-chloro-1-butene as major product.
Reason: 3-chloro-1-butene is a kinetically controlled product.<div><br/></div><div>Read the above assertion and reason and choose the correct option regarding it.</div>
Question 67 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">Which one of the following cells can convert chemical energy of $O_{2}$ and $H_{2}$ directly into electrical energy:</p>
Question 68 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">Which of the following statements is true for fuel cells ?</p></span></span>
Question 69 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">Which of the following reaction is used to make a fuel cell ?</p></span></span>
Question 71 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">Which of the following energy changes occur in galvanic cell?</p></span></span>
Question 73 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">Hydrogen -Oxygen fuel cells are used in space craft to supply:</p>
Question 74 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">The potential across the metal and the aqueous solution of its ions of unit activity at 298K is known as:</p>
Question 75 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">Lithium is generally used as an electrode in high energy density batteries. This is because:</p>
Question 77 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">Following are some of the facts about dry cell</p><p class="wysiwyg-text-align-left">i) It is also called Leclanche cell</p><p class="wysiwyg-text-align-left">ii) It is also called Daniel cell</p><p class="wysiwyg-text-align-left"><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">iii) Electrolyte is a moist paste of NH$_{4}$Cl</span></span><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">and ZnCl$_{2}$</span></span><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">in starch</span></span></p><p class="wysiwyg-text-align-left">iv) Cathodic reaction is</p><p class="wysiwyg-text-align-left"><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">MnO<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">$_{2}$</span></span></span></span><span class="wysiwyg-font-size-xx-small"><span class="wysiwyg-font-size-xx-small"> </span></span><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">(s) + NH$_{4}^{+}$</span></span><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"> + e$^{-}\rightarrow $</span></span><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">MnO(OH)+NH$_{3}$</span></span></p><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p>Select correct facts :</p>
Question 78 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">In which reactants are not contained within the cell but are continuously supplied from external source?</p></span></span>
Question 79 :
In a cell, the following reaction takes place: $Fe + CuSO_{4} \rightarrow FeSO_{4} + Cu$. The cell can be represented as:
Question 80 :
Assertion: Dry cell is a primary cell and lead storage cell is a secondary cell.<br/>Reason: A primary cell can only be used once while secondary cells are rechargeable.<br/>
Question 81 :
When the electric current is passed through a cell having an electrolyte, the positive ions move towards cathode and negative ions towards the anode. If the cathode is pulled out of the solution then____________.
Question 83 :
KCl can be used in salt bridge as electrolyte in which of the following cells?
Question 84 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">In a galvanic cell, the reactions taking place in the anodic half cell and the cathodic half cell will be:</p>
Question 86 :
Electrolysis of a dilute solution of aqueous sodium chloride results in the cathode product:
Question 87 : Which of the following will increase the voltage of the cell? <br/><br/><div>$Sn(s) + 2 \text{Ag}^+ (aq) \rightarrow 2Ag(s) + Sn^{2+}$</div>
Question 89 : <p class="wysiwyg-text-align-left"><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">The reaction $ \frac{1}{2}\times H_{2}(g) + AgCl(aq) \rightarrow H^{+}(aq) + Ag(s)$</span></span></p><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p> can be represented in the galvanic cell as:</p>
Question 90 :
The reaction<br/>$1/2H_2(g)\, +\, AgCl(s)\, \rightarrow\, H^{\bigoplus}(aq)\, +\, Cl^{\circleddash}(aq)\, +\, Ag(s)$ occurs in the galvanic cell:
Question 91 : Consider a spontaneous electrochemical cell containing $Cd, Cd^{2+}, Ag^{+}$, and $Ag$.<br/>The reduction potential of $Cd$ is $-0.403\ V$ and $Ag$ is $0.799\ V$.<br/><br/><div>What is the balanced equation for the reaction that is occurring, and what is the electrochemical cell voltage?</div>
Question 92 :
Assertion: When an electric current is passed through an aqueous solution of sodium chloride, sodium ions move towards cathode and chloride ions move towards anode.
Reason: Cathode is a negatively charged electrode and therefore attracts Na$^+$ ions. Anode is a positively charged electrode and therefore attracts Cl$^-$ ions.
Question 93 :
Assertion: For the Daniell cell, $Zn|Zn^{2+} | | Cu^{2+}|Cu$ with $E_{cell} = 1.1\ volt$, the application of opposite potential greater than $1.1\ V$ results into flow of electrons from cathode to anode.
Reason: $Zn$ is deposited at anode and $Cu$ is dissolved at cathode.
Question 96 :
The standard EMF of quantity electrode is $0.699 V$. The EMF of the quinhydrone electrode dipped in a solution with pH = 10 is:
Question 98 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">During the discharge of a lead storage battery, the density of sulphuric acid fell from $1.294$ to $1.139$ gm$L^{-1}$. Sulphuric acid of density $1.294$ gm $L^{-1}$ is $39$% by weight and that of density 1.139 gm $L^{-1}$ is $20$% by weight. The battery holds $3.5$ litres of acid and the column practically remained constant during the discharge. </p><p class="wysiwyg-text-align-left">Calculate the number of ampere-hours for which the battery must have been used. The charging and discharging reactions are : </p><p class="wysiwyg-text-align-left">$Pb+SO{_{4}}^{2-}\rightarrow PbSO_{4}+2e^{-}$ (charging)</p><p class="wysiwyg-text-align-left">$PbO_{2}+4H^{+}+SO{_{4}}^{2-}+2e^{-}\rightarrow PbSO_{4}+2H_{2}O$ (discharging)</p><span class="wysiwyg-font-size-xx-small"><span class="wysiwyg-font-size-xx-small"></span></span><p></p>
Question 99 : <b><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span></b><p class="wysiwyg-text-align-left">List I                                                   List II</p><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">A) Salt bridge                                 1) Reduction</p><p class="wysiwyg-text-align-left">B) Standard hydrogen electrode    2) Oxidation</p><p class="wysiwyg-text-align-left"><span>C) Cathode                                    3) Reference electrode</span><br/></p><p class="wysiwyg-text-align-left"><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"> D) Anode                                      4) KCl,KNO$_{3},$</span></span></p><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left"><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">                                                       (or) NH$_{4}$NO$_{3}.$</span></span><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">.</span></span></p><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">The correct match is<span> </span><span>:</span></p>
Question 100 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">The negative Zn pole of Daniel cell, sending a constant current through a circuit, decreases in mass by 0.13 g in 30 minutes. If the chemical equivalent of Zn and Cu and 32.5 and 31.5 respectively, the increase in the mass of the positive Cu pole in this time is : <br/></p>
