Question 1 :
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 2 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">Lithium is generally used as an electrode in high energy density batteries. This is because:</p>

Question 3 :
<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>

Question 5 :
<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>

Question 6 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><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 7 :
In a cell, the following reaction takes place: $Fe + CuSO_{4} \rightarrow FeSO_{4} + Cu$. The cell can be represented as:

Question 10 :
KCl can be used in salt bridge as electrolyte in which of the following cells?

Question 11 :
Assertion:&#160;Dry cell is a primary&#160;cell and lead storage cell is a&#160;secondary&#160;cell.<br/>Reason: A primary cell can only be used once while secondary cells are rechargeable.<br/>

Question 13 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><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 class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">and ZnCl$_{2}$<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">in starch</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 class="wysiwyg-font-size-xx-small"><span class="wysiwyg-font-size-xx-small"> <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">(s) + NH$_{4}^{+}$<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">&#160;+ e$^{-}\rightarrow $<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">MnO(OH)+NH$_{3}$</p><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p>Select correct facts :</p>

Question 14 :
<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>

Question 15 :
<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>

Question 17 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><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 19 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><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 22 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">Hydrogen -Oxygen fuel cells are used in space craft to supply:</p>

Question 23 :
Which of the following is always true regarding the spontaneity of reaction occuring in a galvanic cell?

Question 24 :
In a fuel cell ${H}_{2}$ and&#160;${O}_{2}$ react to produce electricity. In the process&#160;${H}_{2}$ gas is oxidized&#160;at anode and&#160;${O}_{2}$ at cathode. If 67.2 litre of&#160;${H}_{2}$&#160;at&#160;STP reacts in&#160;&#160;15 minutes. The average current produced is:<br/>

Question 25 :
Which of the following statements about the spontaneous reaction occurring in a galvanic cell is always true?

Question 27 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">List A&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160; List B</p>&#10;<p class="wysiwyg-text-align-left">A. Dry Cell&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160; &#160;(P) Primary cell</p>&#10;<p class="wysiwyg-text-align-left">B. Lead storage&#160;</p>&#10;<p class="wysiwyg-text-align-left"><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">battery&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160; &#160;(Q) 38%$H_{2}SO_{4}$</p><i>&#10;</i><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left"><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">C. Ni-Cd cell&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160; &#160;&#160;&#160; &#160;(R) $MnO_{2}+C$</p><i>&#10;</i><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">D.<i> </i>$H_{2}-O_{2}$ <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">fuel cell&#160;&#160;&#160;&#160;&#160;&#160;&#160;&#160; (S) Secondary cell</p>

Question 28 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">What is the approximate quantity of electricity(in coulombs) required to deposit all the silver from 250 ml of 1 M AgNO$_{3}$ aqueous solution?&#160;<br/></p>

Question 32 :
Which of the following statements are correct about voltaic cell?<br>(I) Chemical energy isconverted into electrical energy.<br>(II) Electrons flow from anode to cathode.<br>(III) Oxidation occurs at anode.<br>(IV) Anode is negative and cathode is positive.

Question 33 :
For cell reaction : $Zn+ Cu^{2+} \rightarrow Zn^2 + Cu$ cell representation is:

Question 34 :
The weights of various ions liberated by passing the same current through different electrolytes are in the ratio of their:

Question 35 :
Which one is correct about a hypothetical electrochemical cell shown below?<br/>$\underset{A}{\ominus } | A^+ (XM) || B^+ (YM) |&#160;\underset{B}{\oplus} &#160; &#160; &#160; &#160; &#160; E_{cell} &#160;= + 0.20 V$<br/>

Question 36 :
Following are some of the facts about a dry cell<br/>I : It is also called Leclanche cell<br/>II : It is also called Daniel cell<br/>III : Electrolyte is a moist paste of 4 $NH_4Cl$ and 2 $ZnCl_2$ in starch<br/>IV : Cathodic reaction is<br/><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">$2MnO_{2}(s)+2NH_{4}^{+}(aq)+2e^{-}\rightarrow Mn_{2}O_{3}(s)+2NH_{3}(g)+H_{2}O(l)$<br/>Select the correct facts.

Question 37 :
Which of the following reactions is correct for a given electrochemical cell at ${ 25 }^{ o }C$?<br/>$Pt\left| { Br }_{ 2 }\left( g \right) &#160;\right| { Br }^{ - }\left( aq \right) ||{ Cl }^{ - }\left( aq \right) \left| { Cl }_{ 2 }\left( g \right) &#160;\right| Pt$

Question 38 :
Assertion: The Daniell cell becomes dead after some time. Reason: Oxidation potential of zinc anode decreases and that of copper increases.

Question 39 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">In an electro chemical process, a salt bridge is used</p><p class="wysiwyg-text-align-left">a) to maintain electro neutrality in each solution.</p><p class="wysiwyg-text-align-left">b) to complete the circuit so that current can flow</p><p>c) as an oxidising agent</p><p>d) as a colour indicator</p>

Question 40 :
Read the passage given below and answer the question:<br/>Chemical reactions involve the interactions of atoms and molecules. A&#160;large&#160;number of atoms/molecules (approximately $6.023 \times 10^{23}$) are present in few grams of any chemical compound varying with their atomic/molecular masses. To handle such large numbers conveniently, the mole concept was introduced. This concept has implications in diverse areas such as analytical chemistry,&#160; biochemistry, electrochemistry, and radiochemistry. the following example illustrates&#160;a typical case, involving chemical/electrochemical reaction, which requires a clear understanding of the mole concept.<br/>A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolyzed. This leads to the evolution of chlorine gas at one of the electrodes (atomic&#160;mass:&#160;Na = 23, Hg = 200; 1 faraday =96500 coulombs).&#160;<br/>The total charge (coulombs) required for complete electrolysis is:

Question 41 :
The&#160;potential of a hydrogen electrode in a solution with pH = 5 at $25^{\circ}C$&#160;is:

Question 42 :
Assertion: In a galvanic cell, the half-cell with higher reduction potential provides a reducing agent.Reason: Easily reducible substances are good oxidants.<br/>

Question 44 :
Electrolysis of a dilute solution of aqueous sodium chloride results in the cathode product:

Question 45 :
Calculate the EMF of a Daniel cell when the concentration of $ZnSO_{4}$ and $CuSO_{4}$ are $0.001$ M and $0.1$ M&#160;respectively. The standard potential of the cell is $1.1$ V.<br/>

Question 46 :
Saturated solution of $KNO_{3}$ is used to make salt bridge because:

Question 47 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">The chemical used in salt bridge in a galvanic cell is:</p>

Question 49 :
An electrolytic cell is constructed for preparing hydrogen. For an average current of 1 ampere in the circuit, the time required to produced $450mL$ of hydrogen at NTP is approximately.

Question 52 :
<p>In an experiment set up for the measurement of EMF of a half&#160;cell using a reference electrode and a salt bridge, when the salt bridge is&#160;removed, the voltage:</p>

Question 53 :
Foe the electrochemical cell:<br/>$Zn\left( s \right) |{ Zn }^{ 2+ }\left( aq \right) \parallel { Cl }^{ - }\left( aq \right) |{ Cl }_{ 2 }\left( g \right) |Pt\left( s \right)&#160;$<br/>Given : ${ E }_{ { Zn }^{ 2+ }/Zn }^{ o }=-0.76\ Volt$<br/>&#160; &#160; &#160; &#160; &#160; &#160; &#160;${ E }_{ { Cl }^{ - }/{ Cl }_{ 2 }\left( g \right)&#160; }^{ o }=-1.36\ Volt$<br/>From these data one can deduce that:

Question 54 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">The electrochemical cell stops working after some time because:</p>

Question 55 :
Splitting up of the water molecule by an electric current is an example of electrolysis.<br/>

Question 57 :
Which of the following will increase the voltage of the cell?&#160;<br/><br/>$Sn(s) + 2 \text{Ag}^+ (aq) \rightarrow 2Ag(s) + Sn^{2+}$

Question 58 :
The value of equilibrium constant for a feasible cell reaction is:

Question 59 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">Some of the batteries are rechargeable :</p><p class="wysiwyg-text-align-left">I : Dry cell battery</p><p class="wysiwyg-text-align-left">II : Lead-storage (acid) battery</p><p class="wysiwyg-text-align-left">III : Nickel-cadmium battery</p><p class="wysiwyg-text-align-left">IV : Lithium battery</p><p class="wysiwyg-text-align-left">V : Fuel cell</p><p>Select correct alternates :</p>

Question 60 :
During the electrolysis of the aqueous solution of copper sulphate using&#160;Pt electrodes, the reaction taking place at anode electrode is:

Question 61 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">In a galvanic cell, the positive ions of salt bridge migrate towards:</p>

Question 62 :
Which of the following statement (s) differentiate between electrochemical cell and electrolytic cell?

Question 63 :
Which of the following statements is true forthe electrochemical Daniel cell?

Question 64 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">For the galvanic cell :</p>$Al{(s)}|Al{^{3+}}{(aq)}(0.1M)|Ag{^{+}}{(aq)}(0.1M)|Ag{(s)},$<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p>which of the following is/are correct?</p>

Question 66 :
State True or False.<br/>The effect of a change in the concentration of a reactant or product on the cell voltage can be predicted by applying Le-chateliers principle.

Question 67 :
Two&#160;platinum electrodes were immersed in a solution of $CuSO_4$ and electric&#160;current was passed through the solution. After some time, it was found that&#160;colour of $CuSO_4$ disappeared with evolution of gas at the electrode. The&#160;colorless solution contains:<br/>

Question 68 :
Which of the following reactions is used to make a fuel cell?

Question 70 :
In producing chlorine through electrolysis $100$ watt power at 125 V is being consumed. How&#160;much chlorine per minute is liberated ? Electrochemical Equivalent of&#160;chlorine is $0.367$ $\times$ 10$^{-6}$ kg/coulomb:

Question 71 :
<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"><p class="wysiwyg-text-align-left">A lead storage battery containing 5.0 L of (1N)&#160;$H_{2}SO_{4}$ solution is operated for $9.65\times 10^{5}$ s&#160;with a steady current of 100 mA. Assuming volume&#160;of the solution remaining constant, normality of $H_{2}SO_{4}$ will:<span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small">&#160;</p>

Question 72 :
At $25^oC$, the standard oxidation potential of $Zn$ and $Ag$ in water are:<br/>&#160;$Zn(s)\rightarrow Zn^{+2}(aq)+2e^{-},\: E^{0}=0.76V$&#160;<br/>and $Ag(s)\rightarrow Ag^{+}(aq)+e^{-},\: E^{0}=-0.80V$.&#160;<br/>Which of the following reaction actually takes place?