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Electrical cells - class-X

electrical cells

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Questions

Question 1 Multiple Choice (Single Answer)

Which of the following statement is incorrect about electrochemical cell?

  1. Electrons are released at anode
  2. Chemical energy is converted into electrical energy
  3. Salt bridge maintains the electrical neutrality of the electrilytes
  4. Cell can work indefinitely
Question 2 Multiple Choice (Single Answer)

The following electrochemical cell is taken $Cu| Cu^{2+}(aq)|| Ag^{+}(aq))| Ag$ and has emf $E _{r}>0$ by which of the following actions $E _{1}$ increases?

  1. Adding $NH _{3}$ to the cathodic chamber
  2. Adding $HCl$ to the cathodic chamber
  3. Adding $AgNO _{3}$ to the anodic chamber
  4. Adding $NH _{3}$ to the anodic chamber
Question 3 Multiple Choice (Single Answer)

Find out ${E} _{cell}$ of following electrochemical cell (${E} _{{Br} _{2}/{Br}^{-}}=1.09V$)
$Pt(s)\mid {Br} _{2}(l)\mid{Br}^{-}(0.01M)\mid\mid{H}^{+}(0.01M)\mid{H} _{2}(g)(1bar)\mid Pt(s)$

  1. $-1.32V$
  2. $+1.09V$
  3. $-2.15V$
  4. $-1.92V$
Question 4 Multiple Choice (Single Answer)

The following electrochemical cell has been set up: $Pt(s)|Fe^{3+}, Fe^{2+}(a=1)||Ce^{4+}, Ce^{3+}(a=1)|Pt(s); E^{\circ}(Fe^{3+}|Fe^{2+})= 0.77V$; $E^{\circ}(Ce^{4+}|Ce^{3+})= 1.61V$. If an ammeter is connected between the two platinum electrodes, predict the direction of flow of current. Will the current increase or decrease with time?

  1. Ce electrode to Fe electrode, decrease
  2. Ce electrode to Fe electrode, increase
  3. Fe electrode to Ce electrode, decrease
  4. Fe electrode to Ce electrode, increase
Question 5 Multiple Choice (Single Answer)

After some time, the voltage of an electrochemical cell becomes zero. This is because ____________________.

  1. their electrode potential becomes zero.
  2. their reduction potential become equal but have opposite sign
  3. their reduction potential become equal and have the same sign.
  4. the ions of the electrolyte in the salt bridge stop moving.
Question 6 Multiple Choice (Single Answer)

Which one of the following statements is incorrect regarding an electrochemical cell?

  1. The electrode on which oxidation takes place is called anode.
  2. Anode is the negative pole.
  3. The direction of the current is same as that of the direction of flow of electrons.
  4. The flow of current is partly due to flow of electrons and partly due to flow of ions.
Question 7 Multiple Choice (Single Answer)

The first electro-chemical was invented by:

  1. Luigi Galvani.
  2. Alessandro Volta.
  3. Deniel.
  4. Lechanche
Question 8 Multiple Choice (Single Answer)

Statement $1$: In an electrolytic cell, the anode becomes positive and the cathode becomes negative.
Statement $2$: Anions migrate to the anode and cations migrate to the cathode.

  1. Statement $1$ and Statement $2$ are correct and Statement 2 is the correct explanation of Statement $1$.
  2. Both the Statement $1$ and Statement $2$ are correct, but Statement $2$ is NOT the correct explanation of Statement $1$.
  3. Statement $1$ is correct, but Statement $2$ is not correct.
  4. Statement $1$ is not correct, but Statement $2$ is correct.
Question 9 Multiple Choice (Single Answer)

The apparatus in which electrical energy is converted into chemical energy is known as:

  1. voltameter
  2. coulometer
  3. both (A) and (B)
  4. none of these
Question 10 Multiple Choice (Single Answer)

Consider a spontaneous electrochemical cell containing $Cd, Cd^{2+}, Ag^{+}$, and $Ag$.
The reduction potential of $Cd$ is $-0.403\ V$ and $Ag$ is $0.799\ V$.

What is the balanced equation for the reaction that is occurring, and what is the electrochemical cell voltage?

  1. $Ag^{+} + Cd \rightarrow Cd^{2+} + Ag; 1.19\ V$
  2. $2Ag^{+} + Cd \rightarrow Cd^{2+} + 2Ag; 1.20\ V$
  3. $Ag^{+} + Cd \rightarrow Cd^{2+} + Ag^{+}; 0.40\ V$
  4. $2Ag^{+} + Cd \rightarrow Cd^{2+} + 2Ag; 2,30\ V$
Question 11 Multiple Choice (Single Answer)

Which of the following is true of an electrolytic cell?

  1. An electric current causes an otherwise non-spontaneous chemical reaction to occur.
  2. Reduction occurs at the anode
  3. A spontaneous electrochemical reaction produces an electric current
  4. The electrode to which the electrons flow is where oxidation occurs
  5. None of the above
Question 12 Multiple Choice (Single Answer)

The chemical change in an electrolytic cell is non-spontaneous. 

  1. True
  2. False
Question 13 Multiple Choice (Single Answer)

What is a voltaic cell?

  1. A cell in which a spontaneous redox reaction produces electricity.
  2. A cell in which an oxidation reaction produces electricity.
  3. A cell that produces voltage.
  4. A cell full of volts.
  5. Any cell that undergoes a spontaneous reaction.
Question 14 Multiple Choice (Single Answer)

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

  1. $< 1$
  2. $= 1$
  3. $> 1$
  4. zero
Question 15 Multiple Choice (Single Answer)

An electrochemical cell consists of?

  1. A cathode, anode, electrolyte, wire and two compartments.
  2. Cathode, anode, and wire
  3. Two compartments that conduct electricity.
  4. A positive and negative side.
  5. A cathode and an anode.
Question 16 Multiple Choice (Single Answer)

Consider the reaction;
$Cl _2(g)+2Br^-(aq)\rightarrow 2Cl^-(aq)+Br _2$
The emf of the cell when
$[Cl^-]=[Br _2]=[Br]=0.01 M$ and $Cl _2$ gas at 1 atm pressure will be: ($E^0$ for the above reaction is = 0.29 volt)

  1. 0.54 volt
  2. 0.35 volt
  3. 0.24 volt
  4. -0.29 volt
Question 17 Multiple Choice (Single Answer)

In an electrochemical cell, anode and cathode are__________.

  1. Positively and negatively charges ions
  2. Positively and negatively charges electrodes
  3. Negatively and positively charged electrodes
  4. Negatively and positively charged ions
Question 18 Multiple Choice (Multiple Answers)

Electrochemical cells are also called:

  1. electrolytic cells
  2. galvanic cells
  3. fuel cells
  4. voltaic cells
Question 19 Multiple Choice (Single Answer)

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

  1. $Zn + Cl _{2} \rightleftharpoons Zn^{2+} + 2Cl^{-}$ is a non-spontaneous reaction at standard conditions.
  2. $Zn^{2+} + 2Cl^{-} \rightleftharpoons Cl _{2} + Zn$ is a spontaneous reaction at standard conditions with ${ E } _{ cell }^{ o } = 2.12\ volt.$
  3. $Zn + Cl _{2} \longrightarrow Zn^{2+} + 2 Cl^{-}$ is a spontaneous reaction at standard conditions with ${ E } _{ cell }^{ o } = 2.12\ volt.$
  4. $Zn + Cl _{2} \longrightarrow Zn^{2+} + 2 Cl^{-}$ is a spontaneous reaction at standard conditions with ${ E } _{ cell }^{ o } = 0.60\ volt.$
Question 20 Multiple Choice (Multiple Answers)

In an electrolytic cell:

  1. anode is positively charged
  2. cathode is negatively charged
  3. oxidation takes place at anode
  4. reduction takes place at cathode
Question 21 Multiple Choice (Single Answer)

The electrochemical cell shown below is a concentration cell.
$M|{ M }^{ 2+ }$ (saturated solution of a sparingly soluble salt, $M{X} _{2})\parallel {M}^{2+}(0.001 mol{dm}^{-3})| M$. 
The emf of the cell depends on the difference in concentrations of ${M}^{2+}$ ions at the two electrodes.
The emf of the cell at $298K$ is $0.099V$
The solubility product (${K} _{sp}:{mol}^{3}{dm}^{-9}$) of ${MX} _{2}$ at $298K$ based on the information available for the given concentration cell is: (take $2.303\times R\times 298/F=0.059V$)

  1. $1\times {10}^{-15}$
  2. $4\times {10}^{-15}$
  3. $1\times {10}^{-12}$
  4. $4\times {10}^{-12}$
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