Question 2 : <p class="wysiwyg-text-align-left"><span class="wysiwyg-font-size-small">$ Cu(S) + 2Ag^{+}(aq) \rightarrow Cu^{2+}(aq)+2Ag(S) $</span></p><span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">In the given reaction, the reduction half cell reaction is:</p>
Question 3 :
The electric conduction of a salt solution in water depends on the:
Question 4 :
$Zn(s)|ZnCl_2(aq)| |Cl^-(aq)|Cl_2(g)|C(s)$<br/>In the electrochemical cell described by the cell diagram above, what reaction occurs at the anode?<br/>
Question 6 :
Among $Na, Hg, S, Pt$ and graphite, which can be used as electrodes in electrolytic cells having aqueous solutions?
Question 7 :
An electrode connected to the positive terminal of a battery is called anode.
Question 8 :
In a cell, the following reaction takes place: $Fe + CuSO_{4} \rightarrow FeSO_{4} + Cu$. The cell can be represented as:
Question 9 :
KCl can be used in salt bridge as electrolyte in which of the following cells?
Question 10 :
In the silver plating of copper, K[Ag(CN)$_{2}$] is used instead of AgNO$_{3}$. The reason is:
Question 12 :
Which of the following statements are correct about voltaic cell?<br>(I) Chemical energy is converted 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 13 : <span class="wysiwyg-font-size-small"><span class="wysiwyg-font-size-small"></span></span><p class="wysiwyg-text-align-left">The chemical used in salt bridge in a galvanic cell is:</p>
Question 14 :
The U shaped vessel used in Nelson cell is lined inside with asbestos which:<br/>
Question 15 :
For the cell<br/>$Cu(10\ g)|\underset { (C_{1}) }{ CuSO_{4} }$ solution $||\underset { (C_{2}) }{ZnSO_{4} }$ solution $|Zn(10\ g), E_{cell}=E\ V$<br/>$E_{cell}$ for the cell $Cu(20\ g)|\underset{ (C_{1}) } { CuSO_{4} }$ solution $||\underset { (C_{2}) }{ ZnSO_{4} }$ solution $|Zn(20\ g)$, is<br/>
Question 16 :
In an electro-chemical cell, the purpose of the salt bridge is:
Question 17 :
A current being passed for two hour through a solution of an acid liberating $11.2$ litre of oxygen at NTP at anode. What will be the amount of copper deposited at the cathode by the same current when passed through a solution of copper sulphate for the same time?
Question 18 :
Assertion: The anions migrate to the cathode in an electrochemical reaction
Reason: Positively charged ions are attracted to the negatively charged electrode
Question 19 :
Two half-cells have potentials $-0.44$ and $0.799$ volt respectively. These two are coupled to make a galvanic cell. Which of the following will be true?
Question 21 :
Examine the following statement sand select the correct option.<br/>A : Electrolytic conduction is a physical change.<br/>B : In Electrolytic conduction, positive as well as negative ions conduct electricity.
Question 22 :
The standard electrode potential of the half cells is given below:<br/>$Zn^{2+}+2e^{-}\rightarrow Zn; E=-0.76 V$<br/>$Fe^{2+}+2e^{-}\rightarrow Fe; E=-0.44 V$<br/>The emf of the cell $Fe^{2+}=Zn^{-}\rightarrow Zn^{2+}+Fe $
Question 23 :
Assertion: In an electrochemical cell, the electrode that is the site of reduction is called the anode.<br/>
Reason: Oxidation always occurs at the cathode.
Question 24 :
At infinite dilution equivalent conductances of $B{ a }^{ +2 }$ & $C{ 1 }^{ - }$ ions are $127$ & $76\ oh{ m }^{ -1 }c{ m }^{ -1 }\ e{ q }^{ -1 }$ respectively. Equivalent conductance of $BaCl_{ 2 }$ at infinite dilution is:
Question 27 :
Saturated solution $K{ NO }_{ 3 }$ is used to make salt bridge because:
Question 28 :
A steady current of $10.0$ Amps is passed through a nickel production cell of $15$ minutes.<br>Which of the following is the correct expression for calculating the number of grams of nickel produced?<br>Note:<br>$\bullet 1\ faraday = 96,500\ Coulombs$<br>$\bullet$ The electroytic cell involves the following half-reaction:<br>$Ni_{(aq)}^{2+} + 2e^{-} \rightarrow Ni_{(s)}$<br>
Question 29 :
The correct order of the stoichiometries of $AgCl$ formed when $AgNO_{3}$ in excess is treated with the complexes: $CoCl_{3}.6NH_{3}, CoCl_{3}.5NH_{3}, CoCl_{3}.4NH_{3}$ respectively is:
Question 32 :
Given that the standard reduction potentials for ${ { M }^{ + } }/{ M }$ and ${ { N }^{ + } }/{ N }$ electrodes at $298 K$ are $0.52 V$ and $0.25 V$ respectively. Which of the following is correct in respect of the following electrochemical cell?<br>$M | { M }^{ + } || { N }^{ + } | N$
Question 33 :
Consider the half-cell reduction reactions :<br> ${ Mn }^{ 2+ }+{ 2e }^{ - }\rightarrow Mn,{ E }^{ o }=-1.18\ V$<br> ${ Mn }^{ 2+ }\rightarrow { 2n }^{ 3+ }+{ e }^{ - },{ E }^{ o }=-1.51\ V$<br>The ${ E }^{ o }$ for the reaction ${ 3Mn }^{ 2+ }\rightarrow { Mn }^{ 0 }+{ 2Mn }^{ 3+ }$ and possibility of the forward reaction are respectively:<br>
Question 34 :
Assertion: The conductivity of electrolytic solutions increases with increase of temperature.
Reason: Electronic conductance decreases with increase of temperature.
Question 35 :
In an electrochemical cell, reduction takes place at anode BECAUSE oxidation always takes place at the cathode.
