Question Bank for NEET Chemistry Electrochemistry / विद्युत् रसायन Self Evaluation Test - Electrochemistry

1)

Which of the following statement is correct?

A)

Cathode is -ve terminal in both, galvanic and electrolytic cells.

B)

Anode is +ve terminal in both, galvanic and electrolytic cells.

C)

Cathode and anode are -ve terminal in electrolytic and galvanic cell.

D)

Cathode and anode are +ve terminal in electrolytic and galvanic cell.

View Solution

2)

Based on the cell notation for a spontaneous reaction, at the anode: \[Ag\left( s \right)\left| AgCl\left( s \right) \right|C{{l}^{-}}\left( aq \right)\left| \left| B{{r}^{-}}\left( aq \right) \right|B{{r}_{2}}\left( l \right) \right|C\left( s \right)\]

A)

\[AgCl\] gets reduced

B)

Ag gets oxidized

C)

\[B{{r}^{-}}\] gets oxidized

D)

\[B{{r}_{2}}\] gets reduced

View Solution

3)

For the electrochemical cell \[Pt(s)\underset{1\text{ }atm}{\mathop{|{{H}_{2}}(g)|}}\,{{H}^{+}}(1M)|,Cu(s)\] which one of the following statements is true?

A)

\[{{H}^{+}}\] ions are formed at anode and Cu is deposited at cathode.

B)

\[{{H}_{2}}\] is liberated at cathode and Cu is deposited at anode.

C)

Oxidation occurs at cathode.

D)

Reduction occurs at anode.

View Solution

4)

The standard reduction potentials at 298K for the following half reactions are given against each

\[Z{{n}^{2+}}(aq)+2{{e}^{-}}\rightleftharpoons Zn(s);\,\,-0.762\,V\]

\[C{{r}^{3+}}(aq)+3{{e}^{-}}~\rightleftharpoons Cr(s);\,\,-0.740\,V\]

\[2{{H}^{+}}(aq)+2{{e}^{-}}\rightleftharpoons {{H}_{2}}(g);\,\,\,0.00\,V\]

\[F{{e}^{3+}}(aq)+2{{e}^{-}}\rightleftharpoons F{{e}^{2+}}(aq);\,\,0.770\,V\]

Which is the strongest reducing agent?

A)

\[Zn\left( s \right)\]

B)

\[Cr\left( s \right)\]

C)

\[{{H}_{2}}\left( g \right)\]

D)

\[F{{e}^{3+}}(aq)\]

View Solution

5)

Zn gives \[{{H}_{2}}\] gas with \[{{H}_{2}}S{{O}_{4}}\] and \[HCl\] but not with \[HN{{O}_{3}}\] because

A)

Zn acts as oxidizing when reacts with \[HN{{O}_{3}}\].

B)

\[HN{{O}_{3}}\] is weaker acid than \[{{H}_{2}}S{{O}_{4}}\] and \[HCl\].

C)

In electrochemical series Zn is above hydrogen.

D)

\[N{{O}_{3}}^{-}\] is reduced in preference to hydronium.

View Solution

6)

A smuggler could not carry gold by depositing iron on the gold surface since

A)

gold is denser

B)

iron rusts

C)

gold has higher reduction potential than iron

D)

gold has lower reduction potential than iron

View Solution

7)

Standard electrode potential for \[S{{n}^{4+}}/S{{n}^{2+}}\] couple is + 0.15 V and that for the \[C{{r}^{3+}}/Cr\] couple is\[-0.74V\]. These two couples in their standard state are connected to make a cell. The cell potential will be:

A)

+1.19 V

B)

+0.89 V

C)

+0.18 V

D)

+1.83 V

View Solution

8)

A solution contains \[F{{e}^{2+}},F{{e}^{3+}}\] and \[{{I}^{-}}\] ions. This solution was treated with iodine at\[35{}^\circ C\]. \[E{}^\circ \] for \[F{{e}^{3+}}/F{{e}^{2+}}\] is + 0.77 V and \[E{}^\circ \] for \[{{I}_{2}}/2{{I}^{-}}=0.536V.\] he favourable redox reaction is:

A)

\[{{I}_{2}}\] will be reduced to \[{{I}^{-}}\]

B)

There will be no redox reaction

C)

\[{{I}^{-}}\] will be oxidised to \[{{I}_{2}}\]

D)

\[F{{e}^{2+}}\] will be oxidised to \[F{{e}^{3+}}\]

View Solution

9)

Consider the following four electrodes:

\[P=C{{u}^{2+}}(0.0001M)/Cu(s)\]

\[Q=C{{u}^{2+}}\left( 0.1\text{ }M)/Cu(s \right)\]

\[R=C{{u}^{2+}}(0.01M/)Cu(s)\]

\[S=C{{u}^{2+}}(0.001M/)Cu(s)\]

If the standard reduction potential of \[C{{u}^{2+}}/Cu\] is +0.34 V, the reduction potentials in volts of the above electrodes follow the order.

A)

\[P>S>R>Q\]

B)

\[S>R>Q>P\]

C)

\[R>S>Q>P\]

D)

\[Q>R>S>P\]

View Solution

10)

Following cell has EMF 0.7995V. \[Pt|{{H}_{2}}(1\,atm)|HN{{O}_{3}}(1M)||AgN{{O}_{3}}(1M)|Ag\] If we add enough \[KCl\] to the Ag cell so that the final \[C{{l}^{-}}\] is 1M. Now the measured emf of the cell is 0.222V. The \[{{K}_{sp}}\] of \[AgCl\] would be -

A)

\[1\times {{10}^{-9.8}}\]

B)

\[1\times {{10}^{-19.6}}\]

C)

\[2\times {{10}^{-10}}\]

D)

\[2.64\times {{10}^{-14}}\]

View Solution

11)

Standard cell voltage for the cell \[Pb|P{{b}^{2+}}||S{{n}^{2+}}\] is - 0.01 V. If the cell is to exhibit \[{{E}_{cell}}=0\], the value of \[[S{{n}^{2+}}]/[P{{b}^{2+}}]\] should be antilog of-

A)

+0.3

B)

0.5

C)

1.5

D)

\[-0.5\]

View Solution

12)

An electrochemical cell is set up as: \[Pt;{{H}_{2}}(1\,atm)|HCl(0.1M)||C{{H}_{3}}COOH(0.1M)|{{H}_{2}}\](1atm); Pt. The e.m.f of this cell will not be zero, because

A)

the temperature is constant

B)

e.m.f depends on molarities of acids used

C)

acids used in two compartments are different

D)

pH of \[0.1\text{ }M\text{ }HCl\] and \[0.1\,M\,C{{H}_{3}}COOH\] is not same

View Solution

13)

A variable, opposite external potential \[({{E}_{ext}})\] is applied to the cell \[Zn|Z{{n}^{2+}}(1M)||C{{u}^{2+}}(1\,M)|Cu,\] of potential 1.1 V. When \[{{E}_{ext}}<1.1V\] and \[{{E}_{ext}}>1.1V\], respectively electrons flow from:

A)

anode to cathode in both cases

B)

cathode to anode and anode to cathode

C)

anode to cathode and cathode to anode

D)

cathode to anode in both cases

View Solution

14)

The standard electrode potentials \[\left( E{{{}^\circ }_{{{M}^{+}}/M}} \right)\] of four metals A, B, C and D are\[-1.2V,\text{ }0.6V,\text{ }0.85V\] and \[-0.76\text{ }V,\] respectively. The sequence of deposition of metals on applying potential is:

A)

A, C, B, D

B)

B, D, C, A

C)

C, B, D, A

D)

D, A, B, C

View Solution

15)

A current of 10.0 A flows for 2.00 h through an electrolytic cell containing a molten salt of metal X. This results in the decomposition of \[0.250\text{ }mol\] of metal X at the cathode. The oxidation state of X in the molten salt is: \[\left( F=96,500C \right)\]

A)

\[{{1}^{+}}\]

B)

\[{{2}^{+}}\]

C)

\[{{3}^{+}}\]

D)

\[{{4}^{+}}\]

View Solution

16)

Which of the following will form a cell with the highest voltage?

A)

\[1\,MA{{g}^{+}},1\,MC{{o}^{2+}}\]

B)

\[2M\,A{{g}^{+}},2\,MC{{o}^{2+}}\]

C)

\[0.1\,M\,A{{g}^{+}},2\,MC{{o}^{2+}}\]

D)

\[2\,M\,A{{g}^{+}},0.1\,MC{{o}^{2+}}\]

View Solution

17)

The standard EMF for the cell reaction, \[Zn+C{{u}^{2+}}\xrightarrow{{}}Cu+Z{{n}^{2+}}\] is 1.1 volt at \[25{}^\circ C.\] The EMF for the cell reaction, when \[0.1\,MC{{u}^{2+}}\] and \[0.1MZ{{n}^{2+}}\] solutions are used, at \[25{}^\circ C\] is

A)

1.10 V

B)

0.10 V

C)

\[-1.10\text{ }V\]

D)

\[-0.110\text{ }V\]

View Solution

18)

Consider the following reactions

(i) \[C{{d}^{2+}}\left( aq \right)+2{{e}^{-}}\xrightarrow{{}}Cd\left( s \right),E{}^\circ =-0.40V\]

(ii) \[A{{g}^{+}}(aq)+{{e}^{-}}\xrightarrow{{}}Ag(s),E{}^\circ =0.80V\]

For the galvanic cell involving the above reactions. Which of the following is not correct?

A)

Molar concentration of the cation in the cathodic compartment changes faster than that of the cation in the anodic compartment.

B)

\[{{E}_{cell}}\] increase when \[C{{d}^{2+}}\] solution is diluted.

C)

Twice as many electrons pass through the cadmium electrode as through silver electrode.

D)

\[{{E}_{cell}}\] decreases when \[A{{g}^{+}}\] solution is diluted.

View Solution

19)

Given that: \[E{{{}^\circ }_{A{{g}^{+}}/Ag}}~=0.80V\] and \[[A{{g}^{+}}]={{10}^{-3}}M;\] \[E{{{}^\circ }_{Hg_{2}^{2+}/Hg}}=0.785V\] and \[[Hg_{2}^{2+}]={{10}^{-1}}M\] which is true for the cell reaction \[2Hg(l)+2A{{g}^{+}}(aq)\to 2Ag(s)+Hg_{2}^{2+}(aq)?\]

A)

The forward reaction is spontaneous

B)

The backward reaction is spontaneous

C)

\[{{E}_{cell}}=0.163\,\nu \]

D)

\[{{E}_{cell}}=1.585\,\nu \]

View Solution

20)

Use the following standand electrode potentials, calculate \[\Delta G{}^\circ \] in kJ/ mol for the indicated reaction:

\[5C{{e}^{4+}}(aq)+M{{n}^{2+}}(aq)+4{{H}_{2}}O(l)\xrightarrow{{}}\] \[5C{{e}^{3+}}(aq)+MnO_{4}^{-}(aq)+8{{H}^{+}}(aq)\]

\[MnO_{4}^{-}\left( aq \right)+8{{H}^{+}}\left( aq \right)+5{{e}^{-}}\xrightarrow{{}}\] \[M{{n}^{2+}}(aq)+4{{H}_{2}}O(l);E{}^\circ =+1.51V\]

\[C{{e}^{4+}}(aq)+{{e}^{-}}\xrightarrow{{}}C{{e}^{3+}}(aq);E{}^\circ =+1.61\,V\]

A)

\[-9.65\]

B)

\[-24.3\]

C)

\[-48.25\]

D)

\[-35.2\]

View Solution

21)

If 0.01 M solution of an electrolyte has a resistance of 40 ohms in a cell having a cell constant of \[0.4\text{ }c{{m}^{-1}},\] then its molar conductance in \[oh{{m}^{-1}}c{{m}^{2}}mo{{l}^{-1}}\] is

A)

\[{{10}^{2}}\]

B)

\[{{10}^{4}}\]

C)

10

D)

\[{{10}^{3}}\]

View Solution

22)

When a concentrated solution of an electrolyte is diluted

A)

its specific conductance increases.

B)

its equivalent conductivity decreases.

C)

its specific conductivity decreases and equivalent conductivity increases.

D)

both specific and equivalent conductivity increase.

View Solution

23)

The limiting equivalent conductivity of \[NaCl,~KCl\] and \[KBr\] are 126.5, 150.0 and\[151.5\text{ }S\text{ }c{{m}^{2}}e{{q}^{-1}}\], respectively. The limiting equivalent ionic conductivity for \[B{{r}^{-}}\] is\[78\,Sc{{m}^{2}}e{{q}^{-1}}\]. The limiting equivalent ionic conductivity for \[N{{a}^{+}}\] ions would be:

A)

128

B)

125

C)

49

D)

50

View Solution

24)

The ionic conductivity of \[B{{a}^{2+}}\] and \[C{{l}^{-}}\] at infinite dilution are 127 and 76 \[oh{{m}^{-1}}\] \[c{{m}^{2}}e{{q}^{-1}}\] respectively. The equivalent conductivity of \[BaC{{l}_{2}}\] at infinity dilution (in \[oh{{m}^{-1}}\,C{{m}^{2}}e{{q}^{-1}}\]) would be:

A)

203

B)

279

C)

101.5

D)

139.5

View Solution

25)

Aluminium oxide may be electrolysed at \[1000{}^\circ C\] to furnish aluminium metal (At. Mass = 27 amu; 1 Faraday = 96,500 Coulombs). The cathode reaction is - \[A{{l}^{3+}}+3{{e}^{-}}\to Al\] To prepare 5.12 kg of aluminium metal by this method we require electricity of

A)

\[5.49\times {{10}^{1}}C\]

B)

\[5.49\times {{10}^{4}}C\]

C)

\[1.83\times {{10}^{7}}C\]

D)

\[5.49\times {{10}^{7}}C\]

View Solution

26)

When electric current is passed through acidified water, 112 mL of hydrogen gas at STP collected at the cathode in 965 seconds. The current passed in amperes is

A)

1.0

B)

0.5

C)

0.1

D)

2.0

View Solution

27)

On passing current through two cells, connected in series containing solution of \[AgN{{O}_{3}}\] and \[CuS{{O}_{4}}\], 0.18 g of Ag is deposited. The amount of the Cu deposited is:

A)

0.529 g

B)

10.623 g

C)

0.0529 g

D)

1.2708 g

View Solution

28)

If x is the specific resistance of the solution and N is the normality of the solution, the equivalent conductivity of the solution is given by

A)

\[\frac{1000x}{N}\]

B)

\[\frac{1000x}{N}\]

C)

\[\frac{1000N}{x}\]

D)

\[\frac{Nx}{1000}\]

View Solution

29)

For an electrolyte solution of \[0.05\text{ }mol\text{ }{{L}^{-1}}\] the conductivity has been found to be \[0.0110\text{ }S\text{ }c{{m}^{-1}}\] The molar conductivity is

A)

\[0.055\text{ }S\text{ }c{{m}^{2}}mo{{l}^{-1}}\]

B)

\[550\text{ }S\text{ }c{{m}^{2}}mo{{l}^{-1}}\]

C)

\[0.22\text{ }S\text{ }c{{m}^{2}}mo{{l}^{-1}}\]

D)

\[220\text{ }S\text{ }c{{m}^{2}}mo{{l}^{-1}}\]

View Solution

30)

The highest electrical conductivity of the following aqueous solutions is of

A)

0.1 M difluoroacetic acid

B)

0.1 M fluoroacetic acid

C)

0.1 M chloroacetic acid

D)

0.1 M acetic acid

View Solution

31)

A current of 2.0 A passed for 5 hours through a molten metal salt deposits 22.2 g of metal (At wt. = 177). The oxidation state of the metal in the metal salt is

A)

+1

B)

+2

C)

+3

D)

+4

View Solution

32)

The specific conductivity of \[N/10\text{ }KCl\] solution at \[20{}^\circ C\] is \[0.212\text{ }oh{{m}^{-1}}c{{m}^{-1}}\] and the resistance of the cell containing this solution at \[20{}^\circ C\] is 55 ohm. The cell constant is

A)

\[4.616\,c{{m}^{-1}}\]

B)

\[11.66\,\,c{{m}^{-1}}\]

C)

\[2.173\,c{{m}^{-1}}\]

D)

\[3.324\,c{{m}^{-1}}\]

View Solution

33)

The equivalent conductance at infinite dilution of a weak acid such as HF

A)

can be determined by extrapolation of measurements of dilute solutions of \[HCl,HBr\] and HI

B)

can be determined by measurement of very dilute HF solutions

C)

can be determined from measurements of dilute solutions of \[NaF,NaCl\] and \[HCl\]

D)

is an undefined quantity

View Solution

34)

Conductance of \[0.1\text{ }M\text{ }KCl\] (conductivity = \[X\,\,Oh{{m}^{-1}}c{{m}^{-1}}\] filled in a conductivity cell is \[Y\,\,Oh{{m}^{-1}}\]. If the conductance of \[0.1\text{ }M\text{ }NaOH\] filled in the same cell is \[Z\,\,Oh{{m}^{-1}},\] the molar conductance of \[NaOH\] will be

A)

\[{{10}^{3}}\frac{XZ}{Y}\]

B)

\[{{10}^{4}}\frac{XZ}{Y}\]

C)

\[10\frac{XZ}{Y}\]

D)

\[0.1\frac{XZ}{Y}\]

View Solution

35)

In electrolytic reduction of a nitroarene with 50% current efficiency 20.50 g of the compound is reduced by \[2\times 96500\text{ }C\] of electric charge. The molar mass of the compound is

A)

123.0 g

B)

61.5 g

C)

10.2 g

D)

20.5 g

View Solution

36)

Electrolysis of \[NaCl\] solution with inert electrodes for certain period of time gave \[600\text{ }c{{m}^{3}}\] of 1.0 M \[NaOH\] in the electrolytic cell. During the same period 31.80 g of copper was deposited in a copper voltmeter in series with the electrolytic cell. What is the percent current efficiency in the electrolytic cell? (At.wt. of Cu =63.6)

A)

40

B)

25

C)

60

D)

50

View Solution

37)

Given the ionic conductance of

, \[{{K}^{+}}\], and \[N{{a}^{+}}\] are 74, 50, and \[73\text{ }c{{m}^{2}}oh{{m}^{-1}}\] \[e{{q}^{-1}}\] respectively. The equivalent conductance at infinite dilution of the salt

is

A)

\[197\text{ }c{{m}^{2}}oh{{m}^{-1}}e{{q}^{-1}}\]

B)

\[172\,c{{m}^{2}}oh{{m}^{-1}}e{{q}^{-1}}\]

C)

\[135.5\,c{{m}^{2}}oh{{m}^{-1}}e{{q}^{-1}}\]

D)

\[160.5\,c{{m}^{2}}oh{{m}^{-1}}e{{q}^{-1}}\]

View Solution

38)

On passing a current of 1.0 ampere for 16 min and 5 sec through one litre solution of\[CuC{{l}_{2}}\], all copper of the solution was deposited at cathode. The strength of \[CuC{{l}_{2}}\] solution was (Molar mass of Cu= 63.5; Faraday constant\[=96500Cmo{{l}^{-1}}\])

A)

0.01 N

B)

0.01 M

C)

0.02 M

D)

0.2 N

View Solution

39)

Electrode potential of the half cell \[Pt\left( s \right)|Hg\left( l \right)|\]\[H{{g}_{2}}C{{l}_{2}}(s)|C{{l}^{-}}(aq)\] can be increased by:

A)

Increasing \[\left[ C{{l}^{-}} \right]\]

B)

Decreasing \[\left[ C{{l}^{-}} \right]\]

C)

Increasing \[H{{g}_{2}}C{{l}_{2}}(s)\]

D)

Decreasing \[Hg\left( l \right)\]

View Solution

40)

Identify the correct statement:

A)

Corrosion of iron can be minimized by forming a contact with another metal with a higher reduction potential

B)

Iron corrodes in oxygen free water

C)

Corrosion of iron can be minimized by forming an impermeable barrier at its surface

D)

Iron corrodes more rapidly in salt water because its electrochemical potential is higher

View Solution

41)

During the charging of lead storage battery, the reaction at anode is represented by:

A)

\[P{{b}^{2+}}+SO_{4}^{2-}\xrightarrow{{}}PbS{{O}_{4}}\]

B)

\[PbS{{O}_{4}}+2{{H}_{2}}O\xrightarrow{{}}Pb{{O}_{2}}+SO_{4}^{2-}\]\[+4{{H}^{+}}+2{{e}^{-}}\]

C)

\[Pb\xrightarrow{{}}P{{b}^{2+}}+2{{e}^{-}}\]

D)

\[P{{b}^{2+}}+2{{e}^{-}}\xrightarrow{{}}Pb\]

View Solution

42)

Which colourless gas evolves, when \[N{{H}_{4}}Cl\] reacts with zinc in a dry cell battery

A)

\[N{{H}_{4}}\]

B)

\[{{N}_{2}}\]

C)

\[{{H}_{2}}\]

D)

\[C{{l}_{2}}\]

View Solution

43)

Given

\[F{{e}^{3+}}(aq)+{{e}^{-}}\to F{{e}^{2+}}(aq);E{}^\circ =+0.77V\]

\[A{{l}^{3+}}(aq)+3{{e}^{-}}\to Al(s);E{}^\circ =-1.66V\]

\[B{{r}_{2}}(aq)+2{{e}^{-}}\to 2B{{r}^{-}};E{}^\circ =+1.09V\]

Considering the electrode potentials, which of the following represents the correct order of reducing power?

A)

\[F{{e}^{2+}}<Al<B{{r}^{-}}\]

B)

\[B{{r}^{-}}<F{{e}^{2+}}<Al\]

C)

\[Al<B{{r}^{-}}<F{{e}^{2+}}\]

D)

\[Al<F{{e}^{2+}}<B{{r}^{-}}\]

View Solution

44)

How many electrons would be required to deposit 6.35 g of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate? (Atomic mass of copper \[=63.5u,{{N}_{A}}\] = Avogadro's constant):

A)

\[\frac{{{N}_{A}}}{20}\]

B)

\[\frac{{{N}_{A}}}{10}\]

C)

\[\frac{{{N}_{A}}}{5}\]

D)

\[\frac{{{N}_{A}}}{2}\]

View Solution

45)

Given:

\[E{{{}^\circ }_{\frac{1}{2}C{{l}_{2}}/C{{l}^{-}}}}=1.36V,\text{ }E{{{}^\circ }_{C{{r}^{3+}}/Cr}}~=-0.74V,\]

\[E{{{}^\circ }_{C{{r}_{2}}O_{7}^{2-}/C{{l}^{-}}}}=1.33V,\text{ }E{{{}^\circ }_{MnO_{4}^{-}/M{{n}^{2+}}}}~=1.51\,V\]

The correct order of reducing power of the species \[\left( Cr,C{{r}^{3+}},\text{ }M{{n}^{2+}}and\text{ }C{{l}^{-}} \right)\] will be:

A)

\[M{{n}^{2+}}<C{{l}^{-}}<C{{r}^{3+}}<Cr\]

B)

\[M{{n}^{2+}}<C{{r}^{3+}}<C{{l}^{-}}<Cr\]

C)

\[C{{r}^{3+}}<C{{l}^{-}}<M{{n}^{2+}}<Cr\]

D)

\[C{{r}^{3+}}<C{{l}^{-}}<Cr<M{{n}^{2+}}\]

View Solution

46)

The oxidation potential of a hydrogen electrode at pH = 10 and \[{{P}_{H}}_{_{2}}=1\,atm\] is

A)

\[-0.59V\]

B)

\[0.00\text{ }V\]

C)

\[+0.59V\]

D)

0.059 V

View Solution

47)

If the \[E{{{}^\circ }_{cell}}\] for a given reaction has a negative value, then which of the following gives the correct relationships for the values of \[\Delta G{}^\circ \] and \[{{K}_{eq}}\] ?

A)

\[\Delta G{}^\circ >0;{{K}_{eq}}>1\]

B)

\[\Delta G{}^\circ <0;\,\,{{K}_{eq}}>1\]

C)

\[\Delta G{}^\circ <0;\,\,{{K}_{eq}}<1\]

D)

\[\Delta G{}^\circ >0;\,\,{{K}_{eq}}<1\]

View Solution

48)

The EMF of the cell \[Tl/T{{l}^{+}}(0.001M)||C{{u}^{2+}}(0.01M)/Cu\,is\,0.83.\] The cell EMF can be increased by

A)

Increasing the concentration of \[T{{l}^{+}}\] ions.

B)

Increasing the concentration of\[C{{u}^{2+}}\] ions.

C)

Increasing the concentration of \[T{{l}^{+}}\] and \[C{{u}^{2+}}\]ions.

D)

None of these

View Solution

49)

Small quantities of solutions of compounds TX, TY and TZ are put into separate test tubes containing X, Y and Z solution. TX does not react with any of these. TY reacts with both X and Z. TZ reacts with X. The decreasing order of state of oxidation of the anions \[{{X}^{-}},{{Y}^{-}},{{Z}^{-}}\]is

A)

\[{{Y}^{-}},{{Z}^{-}},{{X}^{-}}\]

B)

\[{{Z}^{-}},{{X}^{-}},{{Y}^{-}}\]

C)

\[{{Y}^{-}},{{X}^{-}},{{Z}^{-}}\]

D)

\[{{X}^{-}},{{Z}^{-}},{{Y}^{-}}\]

View Solution

50)

An unknown metal M displaces nickel from nickel (II) sulphate solution but does not displace manganese from manganese sulphate solution. Which order represents the correct order of reducing power?

A)

\[Mn>Ni>M\]

B)

\[Ni>Mn>M\]

C)

\[Mn>M>Ni\]

D)

\[M>Ni>Mn\]

View Solution

51)

What is the e.m.f for the given cell?

\[Cr|C{{r}^{3+}}(1.0M)||C{{o}^{2+}}(1.0M)|Co\]

\[(E{}^\circ for\text{ }C{{r}^{3+}}/Cr=-0.74\] volt and \[E{}^\circ \] for \[C{{o}^{2+}}/Co=-0.28\] volt)

A)

\[-0.46\]volt

B)

\[-1.02\,~volt\]

C)

\[+0.46\] volt

D)

1.66 volt

View Solution

52)

The standard electrode potential \[\left( E{}^\circ \right)\] for \[OC{{l}^{-}}/C{{l}^{-}}\] and \[C{{l}^{-}}/\frac{1}{2}C{{l}_{2}}\] respectively are 0.94 V and \[-1.36\text{ }V\]. The \[E{}^\circ \] value for \[OC{{l}^{-}}/\frac{1}{2}C{{l}_{2}}\] will be

A)

\[-0.42\,\,V\]

B)

\[-2.20\,\,V\]

C)

0.52 V

D)

1.04 V

View Solution

53)

For the reduction of silver ions with copper metal, the standard cell potential was found to be \[+0.46\text{ }V\] at \[25{}^\circ C.\] The value of standard Gibbs energy, \[\Delta G{}^\circ \] will be \[\left( F=96500C\text{ }mo{{l}^{-1}} \right)\]

A)

\[-89.0\,kJ\]

B)

\[-89.0\,J\]

C)

\[-44.5\,kJ\]

D)

\[-98.0\,kJ\]

View Solution

54)

In a cell that utilises the reaction \[Zn(s)+2{{H}^{+}}(aq)\to Z{{n}^{2+}}(aq)+{{H}_{2}}(g)\] addition of \[{{H}_{2}}S{{O}_{4}}\] to cathode compartment, will

A)

increase the E and shift equilibrium to the right

B)

lower the E and shift equilibrium to the right

C)

lower the E and shift equlibrium to the left

D)

increase the E and shift equilibrium to the left

View Solution

55)

For a cell reaction involving two electron change, the standard EMF of the cell is 0.295 V at \[2{}^\circ C\]. The equilibrium constant of the reaction at \[25{}^\circ C\] will be:

A)

\[29.5\times {{10}^{-2}}\]

B)

10

C)

\[1\times {{10}^{10}}\]

D)

\[2.95\times {{10}^{-10}}\]

View Solution

56)

On the basis of the information available from the reaction \[\frac{4}{3}Al+{{O}_{2}}\to \frac{2}{3}A{{l}_{2}}{{O}_{3}},\Delta G\] \[=-827\text{ }kJ\text{ }mo{{l}^{-1}}\] of \[{{O}_{2}}\] the minimum e.m.f required to carry out an electrolysis of \[A{{l}_{2}}{{O}_{3}}\] is \[\left( F=96500C\text{ }mo{{l}^{-1}} \right)\]

A)

8.56 V

B)

2.14 V

C)

4.28 V

D)

6.42 V

View Solution

57)

The e.m.f. of a Daniell cell at 298 K is \[{{E}_{1}}.\]

When the concentration of \[ZnS{{O}_{4}}\] is 1.0 M and that of \[CuS{{O}_{4}}\] is 0.01 M, the e.m.f. changed to \[{{E}_{2}}\]. What is the relationship between \[{{E}_{1}}\] and\[{{E}_{2}}\]?

A)

\[{{E}_{2}}=0\ne {{E}_{1}}\]

B)

\[{{E}_{1}}>{{E}_{2}}\]

C)

\[{{E}_{1}}<{{E}_{2}}\]

D)

\[{{E}_{1}}={{E}_{2}}\]

View Solution

58)

Mark the false statement?

A)

A salt bridge is used to eliminate liquid junction potential

B)

The Gibbs free energy change, \[\Delta G\] is related with electromotive force E as \[\Delta G=-nFE\]

C)

Nernst equation for single electrode potential is \[E=E{}^\circ -\frac{RT}{nF}log{{a}_{{{M}^{n+}}}}\]

D)

The efficiency of a hydrogen-oxygen fuel cell is 23%

View Solution

59)

The electrode potential \[{{E}_{(Z{{n}^{2+}}/Zn)}}\] of a zinc electrode at \[25{}^\circ C\] with an aqueous solution of \[0.1\text{ }M\text{ }ZnS{{O}_{4}}\] is\[[E{{{}^\circ }_{(Z{{n}^{2+}}/Zn)}}~=-0.76\text{ }V\]. Assume \[\frac{2.303RT}{F}=0.06\text{ }at\text{ }298\text{ }K].\]

A)

+0.73

B)

\[-0.79\]

C)

\[-0.82\]

D)

\[-0.70\]

View Solution

60)

The reduction potential (in volt) of a hydrogen electrode set up with a \[2\times {{10}^{-2}}M\] aqueous solution of a weak mono basic acid \[({{K}_{a}}=5\times {{10}^{-5}})\] at one atmosphere and \[25{}^\circ C\] is

A)

+0.09

B)

+0.18

C)

\[-0.09\]

D)

\[-0.18\]

View Solution

61)

A solution of copper sulphate \[\left( CuS{{O}_{4}} \right)\] is electrolysed for 10 minutes with a current of 1.5 amperes. The mass of copper deposited at the cathode (at. mass of\[Cu=63u\]) is:

A)

0.3892 g

B)

0.2938 g

C)

0.2398 g

D)

0.3928 g

View Solution

62)

A battery is constructed of Cr and \[N{{a}_{2}}C{{r}_{2}}{{O}_{7}}\]. The unbalanced chemical equation when such a battery discharges is following \[N{{a}_{2}}C{{r}_{2}}{{O}_{7}}+Cr+{{H}^{+}}\to C{{r}^{3+}}+{{H}_{2}}O+N{{a}^{+}}\] If one Faraday of electricity is passed through the battery during the charging, the number of moles of \[C{{r}^{\text{3+}}}\] removed from the solution is

A)

\[\frac{4}{3}\]

B)

\[\frac{1}{3}\]

C)

\[\frac{3}{3}\]

D)

\[\frac{2}{3}\]

View Solution

63)

The standard potentials of \[A{{g}^{+}}/Ag,H{{g}_{2}}^{2+}/2Hg,C{{u}^{2+}}/Cu\] and \[M{{g}^{2+}}/Mg\] electrodes are 0.80,0.79, 0.34 and\[-2.37\text{ }V\], respectively. An aqueous solution which contains one mole per litre of the salts of each of the four metals is electrolyzed. With increasing voltage, the correct sequence of deposition of the metals at the cathode is

A)

\[Ag,Hg,Cu,Mg\]

B)

\[Cu,Hg,Ag\] only

C)

\[Ag,Hg,Cu\] only

D)

\[Mg,Cu,Hg,Ag\]

View Solution

64)

When electric current is passed through a cell having an electrolytic solution, the cations move towards the cathode and anions towards the anode. If anode is pulled out from the solution

A)

the cations and anions will move towards the cathode

B)

the cations will continue to move towards cathode and anions will stop moving

C)

both the cations and anions will stop moving

D)

the cations and anions will start moving randomly.

View Solution

65)

At 298K the standard free energy of formation of \[{{H}_{2}}O(l)\] is \[-237.20\text{ }kJ/mol\] while that of its ionisation into \[{{H}^{+}}\] ion and hydroxyl ions is 80 kJ/ mol, then the emf of the following cell at 298 K will be [Take Faraday constant F = 96500 C] \[{{H}_{2}}(g,1bar)|{{H}^{+}}(1M)||O{{H}^{-}}(1M)|{{O}_{2}}(g,1\,bar)\]

A)

0.40 V

B)

0.81 V

C)

1.23 V

D)

\[-0.40\text{ }V\]

View Solution

66)

A concentration cell is a galvanic cell in which

A)

decrease in free energy in a spontaneous chemical process appears as electrical energy

B)

decrease in free energy in a spontaneous physical process appears as electrical energy

C)

decrease in free energy in a spontaneous physical or chemical process appears as electrical energy

D)

a non-spontaneous physical or chemical process produces electrical energy.

View Solution

67)

In the silver plating of copper, \[K[Ag{{(CN)}_{2}}]\] is used instead of \[AgN{{O}_{3}}\]. The reason is

A)

a thin layer of Ag is formed on Cu

B)

more voltage is required

C)

\[A{{g}^{+}}\] ions are completely removed from solution

D)

less availability of \[A{{g}^{+}}\] ions, as Cu cannot displace Ag from \[{{[Ag{{\left( CN \right)}_{2}}]}^{-}}\] ion

View Solution

68)

1.0 L each of a buffer containing 1 mole \[N{{H}_{3}}\] and 1 mol of \[NH_{4}^{+}\] were placed in the cathodic and anodic half-cells and 965 C of electricity was passed. If anodic and cathodic half cells reactions involve oxidation and reduction of water only as

\[2{{H}_{2}}O\xrightarrow{{}}4{{H}^{+}}+{{O}_{2}}-4{{e}^{-}};\]

\[2{{H}_{2}}O+2{{e}^{-}}\xrightarrow{{}}{{H}_{2}}+2O{{H}^{-}}\]

Then pH of

A)

cathodic solution will increase

B)

anodic solution will decrease

C)

both the solutions will remain practically constant

D)

both the solutions will increase

View Solution

69)

The emf of a particular voltaic cell with the cell reaction \[Hg_{2}^{2+}+{{H}_{2}}\rightleftharpoons 2Hg+2{{H}^{+}}\] is 0.65 V. The maximum electrical work of this cell when 0.5 g of \[{{H}_{2}}\] is consumed.

A)

\[-3.12\times {{10}^{4}}J\]

B)

\[-1.25\times {{10}^{5}}J\]

C)

\[25.0\times {{10}^{6}}J\]

D)

None of these

View Solution

70)

A cell reaction would be spontaneous if the cell potential and \[{{\Delta }_{r}}G\] are respectively:

A)

positive and negative

B)

negative, negative

C)

zero, zero

D)

positive, zero

View Solution

71)

The Nernst equation \[E=E{}^\circ -RT/nF\] In Q indicates that the Q will be equal to equilibrium constant \[{{K}_{c}}\] when:

A)

\[E=E{}^\circ \]

B)

\[RT/nF=1\]

C)

\[E=zero\]

D)

\[E{}^\circ =1\]

View Solution

72)

Thermodynamic efficiency of a cell is given by:

A)

\[\frac{\Delta H}{\Delta G}\]

B)

\[\frac{nFE}{\Delta G}\]

C)

\[\frac{-nFE}{\Delta H}\]

D)

\[nFE{}^\circ \]

View Solution

73)

A graph was plotted between molar conductivity of various electrolytes \[(NaCl,HCl\,and\,N{{H}_{4}}OH)\] and \[\sqrt{c}(in\,mol\,{{L}^{-1}}).\] Correct set is:

A)

\[I(NaCl),II(HCL),III,(N{{H}_{4}}OH)\]

B)

\[I\left( HCl \right),II\left( NaCl \right),III,\left( N{{H}_{4}}OH \right)\]

C)

\[I\left( N{{H}_{4}}OH \right),II\left( NaCl \right),III,\left( HCl \right)\]

D)

\[I(N{{H}_{4}}OH),II(HCl),III,(NaCl)\]

View Solution

74)

\[HN{{O}_{3}}\] (aq) is titrated with \[NaOH\left( aq \right)\] conductometrically, graphical representation of the titration is:

A)

B)

C)

D)

View Solution

75)

In the electrolysis of water, one faraday of electrical energy would liberate

A)

one mole of oxygen

B)

one gram atom of oxygen

C)

8 g oxygen

D)

22.4 lit. of oxygen

View Solution

76)

Resistance of a conductivity cell filled with a solution of an electrolyte of concentration 0.1 M is \[100\Omega .\]. The conductivity of this solution is \[1.29\text{ }S\text{ }{{m}^{-1}}\]. Resistance of the same cell when filled with 0.02 M of the same solution is \[520\Omega \]. The molar conductivity of 0.02 M solution of electrolyte will be

A)

\[1.24\times {{10}^{-4}}\,S{{m}^{2}}mo{{l}^{-1}}\]

B)

\[12.4\times {{10}^{-4}}\,S{{m}^{2}}mo{{l}^{-1}}\]

C)

\[124\times {{10}^{-4}}\,S{{m}^{2}}mo{{l}^{-1}}\]

D)

\[1240\times {{10}^{-4}}\,S{{m}^{2}}mo{{l}^{-1}}\]

View Solution

77)

\[{{\Lambda }_{ClC{{H}_{2}}COONa}}=224\,oh{{m}^{-1}}c{{m}^{2}}g\,e{{q}^{-1}},\]

\[{{\Lambda }_{NaCl}}=38.2\,oh{{m}^{-1}}c{{m}^{2}}g\,e{{q}^{-1}},\]

\[{{\Lambda }_{HCl}}=203\,oh{{m}^{-1}}c{{m}^{2}}ge{{q}^{-1}},\]

What is the value of \[{{\Lambda }_{CIC{{H}_{2}}COOH}}\]

A)

\[288.5\,oh{{m}^{-1}}c{{m}^{2}}\,g\,e{{q}^{-1}}\]

B)

\[289.5\,oh{{m}^{-1}}c{{m}^{2}}ge{{q}^{-1}}\]

C)

\[388.8\,oh{{m}^{-1}}c{{m}^{2}}g\,e{{q}^{-1}}\]

D)

\[59.5\,oh{{m}^{-1}}c{{m}^{2}}g\,e{{q}^{-1}}\]

View Solution

78)

1.08 g of pure silver was converted into silver nitrate and its solution was taken in a beaker. It was electrolysed using platinum cathode and silver anode. 0.01 Faraday of electricity was passed using 0.15 volt above the decomposition potential of silver. The silver content of the beaker after the above shall be

A)

0 g

B)

0.108 g

C)

1.08 g

D)

None of these

View Solution

79)

Specific conductance of 0.1 M sodium chloride solution is\[1.06\times {{10}^{-2}}oh{{m}^{-1}}c{{m}^{-1}}\]. Its molar conductance in \[oh{{m}^{-1}}c{{m}^{2}}mo{{l}^{-1}}\] is

A)

\[1.06\times {{10}^{2}}\]

B)

\[1.06\times {{10}^{3}}\]

C)

\[1.06\times {{10}^{4}}\]

D)

\[5.3\times {{10}^{2}}\]

View Solution

80)

In the electrolysis of \[CuC{{l}_{2}}\] solution, the mass of the cathode increased by 3.2 g. What occured at the copper anode?

A)

0.12 litre of \[C{{l}_{2}}\] was liberated

B)

0.56 litre of \[{{O}_{2}}\] was liberated

C)

0.1 mol \[C{{u}^{2+}}\] passed into the solution.

D)

0.05 mol of \[C{{u}^{2+}}\] passed into the solution.

View Solution

81)

Given \[E{{{}^\circ }_{C{{u}^{2+}}/Cu}}=0.34V,\,E{{{}^\circ }_{C{{u}^{2+}}/Cu}}=0.15V\] Standard electrode potential for the half cell \[C{{u}^{+}}/Cu\] is

A)

0.38 V

B)

0.53 V

C)

0.19 V

D)

0.49 V

View Solution

82)

At 298 K, the standard reduction potentials are 1.51 V for \[MnO_{4}^{-}|M{{n}^{2+}},1.36V\,\text{for }C{{l}_{2}}|C{{l}^{-}},\,\,1.07\] \[V\,for\,B{{r}_{2}}/B{{r}^{-}}\], and 0.54 V for \[{{I}_{2}}/{{I}^{-}}.\text{ }At\text{ }pH=3,\] permanganate is expected to oxidize: \[\left( \frac{RT}{F}=0.059V \right)\]

A)

\[C{{l}^{-}},B{{r}^{-}}\] and \[{{I}^{-}}\]

B)

\[B{{r}^{-}}\] and \[{{I}^{-}}\]

C)

\[C{{l}^{-}}\] and \[B{{r}^{-}}\]

D)

\[{{I}^{-}}\] only

View Solution

83)

Electrode potentials \[\left( E{}^\circ \right)\] are given below:

\[C{{u}^{+}}/Cu=+0.52V,\]

\[F{{e}^{3+}}/F{{e}^{2+}}=+0.77V,\]

\[\frac{1}{2}{{I}_{2}}(s)/{{I}^{-}}=+0.54V,\]

\[A{{g}^{+}}/Ag=+0.88V\].

Based on the above potentials, strongest oxidizing agent will be:

A)

\[C{{u}^{+}}\]

B)

\[F{{e}^{3+}}\]

C)

\[A{{g}^{+}}\]

D)

\[{{I}_{2}}\]

View Solution

84)

Which of the following is a highly corrosive salt?

A)

\[H{{g}_{2}}C{{l}_{2}}\]

B)

\[HgC{{l}_{2}}\]

C)

\[FeC{{l}_{2}}\]

D)

\[PbC{{l}_{2}}\]

View Solution

85)

The Zn acts as sacrificial or cathodic protection to prevent rusting of iron because:

A)

\[{{E}^{{}^\circ }}_{OP}\,\text{of }Zn<{{E}^{{}^\circ }}_{OP}\text{of}\,Fe\]

B)

\[{{E}^{{}^\circ }}_{OP}\,\text{of}\,Zn>{{E}^{{}^\circ }}_{OP}\,\text{of}\,Fe\]

C)

\[{{E}^{{}^\circ }}_{OP}\text{of}\,Zn={{E}^{{}^\circ }}_{OP}\,\text{of}\,Fe\]

D)

Zn is cheaper than iron

View Solution

86)

Among the following cells:

(I) Leclanche cell

(II) Nickel-Cadmium cell

(III) Lead storage battery

(IV) Mercury cell primary cells are

A)

I and II

B)

I and III

C)

II and III

D)

I and IV

View Solution

87)

How long a current of 3 amperes has to be passed through a solution of \[AgN{{O}_{3}}\] to coat a metal surface of \[80c{{m}^{2}}\] and 0.005 mm thick layer. Density of Ag is \[10.5\text{ }g\,c{{m}^{-3}}\]

A)

125.1 seconds

B)

12.5 seconds

C)

155.2 seconds

D)

200 seconds

View Solution

88)

\[A{{l}_{2}}{{O}_{3}}\] is reduced by electrolysis at low potentials and high currents. If \[4.0\times {{10}^{4}}\] amperes of current is passed through molten \[A{{l}_{2}}{{O}_{3}}\] for 6 hours, what mass of aluminium is produced? (Assume 100% current efficiency. At. mass of\[Al=27g\text{ }mo{{l}^{-1}}\])

A)

\[8.1\times {{10}^{4}}g\]

B)

\[2.4\times {{10}^{5}}g\]

C)

\[1.3\times {{10}^{4}}g\]

D)

\[9.0\times {{10}^{3}}g\]

View Solution

89)

The resistance of 1 N solution of acetic acid is 250 ohm, when measured in a cell of cell constant\[1.15\text{ }c{{m}^{-1}}\]. The equivalent conductance (in \[oh{{m}^{-1}}c{{m}^{2}}equi{{v}^{-1}}\]) of 1 N acetic acid will be

A)

4.6

B)

9.2

C)

18.4

D)

0.023

View Solution

90)

Specific conductance of 0.1 MHA is \[3.75\times {{10}^{-4}}oh{{m}^{-1}}c{{m}^{-1}}\]. If \[{{\lambda }^{\infty }}(HA)=250\,oh{{m}^{-1}}c{{m}^{2}}mo{{l}^{-1}}\], the dissociation constant \[{{K}_{a}}\] of HA is:

A)

\[1.0\times {{10}^{-5}}\]

B)

\[2.25\times {{10}^{-4}}\]

C)

\[2.25\times {{10}^{-5}}\]

D)

\[2.25\times {{10}^{-13}}\]

View Solution

91)

Equivalent conductance at infinite dilution, \[{{\lambda }^{{}^\circ }}\] of \[N{{H}_{4}}Cl,\,NaOH\] and \[NaCl\] are 128.0,217.8 and \[109.3\text{ }oh{{m}^{-1}}c{{m}^{2}}\text{ }e{{q}^{-1}}\] respectively. The equivalent conductance of \[0.01\text{ }N\text{ }N{{H}_{2}}OH\] is \[9.30\text{ }oh{{m}^{-1}}\,c{{m}^{2}}\text{ }e{{q}^{-1}}\] then the degree of ionization of \[N{{H}_{4}}OH\] at this temperature would be

A)

0.04

B)

0.1

C)

0.39

D)

0.62

View Solution

92)

\[{{I}_{2}}(s)|{{I}^{-}}(0.1M)\] half-cell is connected to a \[{{H}^{+}}\left( aq \right)\left| {{H}_{2}}\left( \text{1}bar \right) \right|Pt\] half cell and e.m.f. is found to be\[0.7714V.if\,{{E}^{{}^\circ }}_{{{I}_{2}}|{{I}^{-}}}=0.535\text{ }V\], find the pH of \[{{H}^{+}}|{{H}_{2}}\] half-cell.

A)

1

B)

3

C)

5

D)

7

View Solution

93)

Consider the following standard electrode potentials and calculate the equilibrium constant at 25° C for the indicated disproportion nation reaction:

\[3M{{n}^{2+}}(aq)\xrightarrow{{}}Mn(s)+2M{{n}^{3+}}(aq)\]

\[M{{n}^{3+}}\left( aq \right)+{{e}^{-}}\xrightarrow{{}}M{{n}^{2+}}\left( aq \right);{{E}^{{}^\circ }}=1.51\text{ }V\]

\[M{{n}^{2+}}(aq)+2{{e}^{-}}\xrightarrow{{}}Mn(s);E{}^\circ =-1.185V\]

A)

\[1.2\times {{10}^{-43}}\]

B)

\[2.4\times {{10}^{-73}}\]

C)

\[6.3\times {{10}^{-92}}\]

D)

\[1.5\times {{10}^{-62}}\]

View Solution

94)

In a hydrogen-oxygen fuel cell, combustion of hydrogen occurs to

A)

produce high purity water

B)

create potential difference between two electrodes

C)

generate heat

D)

remove adsorbed oxygen from electrode surfaces

View Solution

95)

The standard reduction potentials at \[25{}^\circ C\] of \[L{{i}^{+}}/Li,B{{a}^{2+}}/Ba,N{{a}^{+}}/Na\] and \[M{{g}^{2+}}/Mg\] are \[-3.03,-2.73,-2.71\] and \[-2.37\] volt respectively Which one of the following is the strongest oxidising agent?

A)

\[N{{a}^{+}}\]

B)

\[L{{i}^{+}}\]

C)

\[B{{a}^{2+}}\]

D)

\[M{{g}^{2+}}\]

View Solution

96)

The \[E{{{}^\circ }_{{{M}^{3+}}/{{M}^{2+}}}}\] values for \[Cr,Mn,Fe\] and Co are \[-0.41,+1.57,+0.77\] and + 1.97V respectively For which one of these metals the change in oxidation state from +2 to +3 is easiest?

A)

Fe

B)

Mn

C)

Cr

D)

Co

View Solution

97)

The solution of \[CuS{{O}_{4}}\] in which copper rod is immersed is diluted to 10 times. The reduction electrode potential

A)

Increases by \[30m\text{ }V\]

B)

Decreases by \[30m\text{ }V\]

C)

Increases by \[59m\text{ }V\]

D)

Decreases by \[59m\text{ }V\]

View Solution

98)

For a given reaction: \[M(x+n)+n{{e}^{-}}\xrightarrow{{}}{{M}^{x+}},{{E}^{-}}_{red}\] is known along with \[{{M}^{(x+n)}}\] and \[{{M}^{x+}}\] ion concentrations. Then

A)

n can be evaluated

B)

x can be evaluated

C)

\[\left( x+n \right)\] can be evaluated

D)

\[n,x,\left( x+n \right)\] can be evaluated

View Solution

99)

The emf of the cell \[Pt\,C{{l}_{2}}(g)({{P}_{1}}atm)/C{{l}^{-}}(aq)\]\[(1M)/C{{l}_{2}}(g)({{P}_{2}}atm)Pt\] will be positive when

A)

\[{{P}_{1}}={{P}_{2}}\]

B)

\[{{P}_{1}}<{{P}_{2}}\]

C)

\[{{P}_{1}}>{{P}_{2}}\]

D)

None of these

View Solution

100)

Equivalent conductivity can be expressed in terms of specific conductance \[\kappa \] and concentration (N) in gram equivalent per \[d{{m}^{-3}}\] as:

A)

\[\kappa\times n\]

B)

\[\frac{\kappa\times 1000}{N}\]

C)

\[\frac{\kappa\times N}{1000}\]

D)

\[\kappa\times N\times 1000\]

View Solution

NEET Chemistry Electrochemistry / विद्युत् रसायन Question Bank

done Self Evaluation Test - Electrochemistry Total Questions - 100

Study Package

Self Evaluation Test - Electrochemistry

Self Evaluation Test - Electrochemistry Total Questions - 100