Electrochemistry
218 Questions
2020
JEE Mains
MCQ
JEE Main 2020 (Online) 4th September Morning Slot
$E_{C{u^{2 + }}|Cu}^0$ = +0.34 V
$E_{Z{n^{2 + }}|Zn}^0$ = -0.76 V
Identify the incorrect statement from the option below for the above cell :
A.
If Eext < 1.1 V, Zn dissolves at anode and Cu
deposits at cathode
B.
If Eext = 1.1 V, no flow of e– or current
occurs
C.
If Eext > 1.1 V, e– flows from Cu to Zn
D.
If Eext > 1.1 V, Zn dissolves at Zn electrode
and Cu deposits at Cu electrode
2020
JEE Mains
MCQ
JEE Main 2020 (Online) 3rd September Morning Slot
Let CNaCl
and CBaSO4 be the conductances (in S) measured for saturated aqueous solutions of NaCl
and BaSO4, respectively, at a temperature T.
Which of the following is false?
A.
Ionic mobilities of ions from both salts increase with T.
B.
CNaCl(T2) > CNaCl(T1) for T2 > T1
C.
CBaSO4(T2) > CBaSO4(T1) for T2 > T1
D.
CNaCl >> CBaSO4 at a given T
2020
JEE Mains
MCQ
JEE Main 2020 (Online) 7th January Evening Slot
The equation that is incorrect is :
A.
${\left( {\Lambda _m^0} \right)_{KCl}} - {\left( {\Lambda _m^0} \right)_{NaCl}} = {\left( {\Lambda _m^0} \right)_{KBr}} - {\left( {\Lambda _m^0} \right)_{NaBr}}$
B.
${\left( {\Lambda _m^0} \right)_{NaBr}} - {\left( {\Lambda _m^0} \right)_{NaI}} = {\left( {\Lambda _m^0} \right)_{KBr}} - {\left( {\Lambda _m^0} \right)_{NaBr}}$
C.
${\left( {\Lambda _m^0} \right)_{NaBr}} - {\left( {\Lambda _m^0} \right)_{NaCl}} = {\left( {\Lambda _m^0} \right)_{KBr}} - {\left( {\Lambda _m^0} \right)_{KCl}}$
D.
${\left( {\Lambda _m^0} \right)_{{H_2}O}} = {\left( {\Lambda _m^0} \right)_{HCl}} + {\left( {\Lambda _m^0} \right)_{NaOH}} - {\left( {\Lambda _m^0} \right)_{NaCl}}$
2020
JEE Mains
MCQ
JEE Main 2020 (Online) 7th January Morning Slot
Given that the standard potentials (Eo) of Cu2+/Cu and Cu+/Cu are 0.34 V and 0.522 V respectively, the Eo of Cu2+/Cu+ :
A.
- 0.182 V
B.
- 0.158 V
C.
0.182 V
D.
+0.158 V
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 12th April Morning Slot
Given
CO3+ + e– $ \to $ CO2+ ; Eo = + 1.81 V
Pb4+ + 2e– $ \to $ Pb2+ ; Eo = + 1.67 V
Ce4+ + e– $ \to $ Ce3+ ; Eo = + 1.61 V
Bi3+ + 3e– $ \to $ Bi ; Eo = + 0.20 V
Oxidizing power of the species will increase in the order :
CO3+ + e– $ \to $ CO2+ ; Eo = + 1.81 V
Pb4+ + 2e– $ \to $ Pb2+ ; Eo = + 1.67 V
Ce4+ + e– $ \to $ Ce3+ ; Eo = + 1.61 V
Bi3+ + 3e– $ \to $ Bi ; Eo = + 0.20 V
Oxidizing power of the species will increase in the order :
A.
Co3+ < Ce4+
< Bi3+ < Pb4+
B.
Co3+ < Pb4+ < Ce4+
< Bi3+
C.
Ce4+
< Pb4+ < Bi3+ < Co3+
D.
Bi3+ < Ce4+
< Pb4+ < Co3+
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 10th April Evening Slot
Which one of the following graphs between molar conductivity (${\Lambda _m}$) versus $\sqrt C $ is correct ?
A.
B.
C.
D.
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 10th April Morning Slot
Consider the statements S1 and S2
S1 : Conductivity always increases with decrease in the concentration of electrolyte.
S2 : Molar conductivity always increases with decrease in the concentration of electrolyte.
The correct option among the following is :
S1 : Conductivity always increases with decrease in the concentration of electrolyte.
S2 : Molar conductivity always increases with decrease in the concentration of electrolyte.
The correct option among the following is :
A.
Both S1 and S2 are wrong
B.
S1 is correct and S2 is wrong
C.
Both S1 and S2 are correct
D.
S1 is wrong and S2 is correct
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 9th April Evening Slot
A solution of Ni(NO3)2 is electrolysed between
platinum electrodes using 0.1 Faraday
electricity. How many mole of Ni will be
deposited at the cathode?
A.
0.10
B.
0.15
C.
0.20
D.
0.05
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 9th April Morning Slot
The standard Gibbs energy for the given cell
reaction in kJ mol–1 at 298 K is :
Zn(s) + Cu2+ (aq) $ \to $ Zn2+ (aq) + Cu (s),
E° = 2 V at 298 K
(Faraday's constant, F = 96000 C mol–1)
Zn(s) + Cu2+ (aq) $ \to $ Zn2+ (aq) + Cu (s),
E° = 2 V at 298 K
(Faraday's constant, F = 96000 C mol–1)
A.
384
B.
–192
C.
–384
D.
192
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 8th April Evening Slot
Calculate the standard cell potential in (V) of the
cell in which following reaction takes place :
Fe2+(aq) + Ag+(aq) $ \to $ Fe3+(aq) + Ag (s)
Given that
$E_{A{g^ + }/Ag}^o = xV$
$E_{Fe^{2+ }/Fe}^o = yV$
$E_{Fe^{3+ }/Fe}^o = zV$
Fe2+(aq) + Ag+(aq) $ \to $ Fe3+(aq) + Ag (s)
Given that
$E_{A{g^ + }/Ag}^o = xV$
$E_{Fe^{2+ }/Fe}^o = yV$
$E_{Fe^{3+ }/Fe}^o = zV$
A.
x + 2y - 3z
B.
x - z
C.
x - y
D.
x + y - z
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 8th April Morning Slot
Given that ${E^\Theta }_{{O_2}/{H_2}O} = 1.23\,V$ ;
${E^\Theta }_{{S_2}O_8^{2 - }/SO_4^{2 - }} = 2.05\,V$
${E^\Theta }_{B{r_2}/B{r^ - }} = 1.09\,V$
${E^\Theta }_{A{u^{3 + }}/Au} = 1.4\,V$
The strongest oxidizing agent is :
${E^\Theta }_{{S_2}O_8^{2 - }/SO_4^{2 - }} = 2.05\,V$
${E^\Theta }_{B{r_2}/B{r^ - }} = 1.09\,V$
${E^\Theta }_{A{u^{3 + }}/Au} = 1.4\,V$
The strongest oxidizing agent is :
A.
O2
B.
Au3+
C.
Br2
D.
${S_2}O_8^{2 - }$
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 12th January Evening Slot
$ \wedge _m^ \circ $ for NaCl, HCl and NaA are 126.4, 425.9 and 100.5 S cm2 mol–1, respectively. If the conductivity of 0.001 M HA is-
5 $ \times $ 10–5 S cm–1, degree of dissociation of HA is -
5 $ \times $ 10–5 S cm–1, degree of dissociation of HA is -
A.
0.50
B.
0.125
C.
0.25
D.
0.75
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 12th January Morning Slot
The standard electrode potential ${E^o }$ and its temperature coefficient $\left( {{{d{E^o }} \over {dT}}} \right)$ for a cell are 2V and $-$ 5 $ \times $ 10$-$4 VK$-$1 at 300 K respectively.
The cell reaction is
Zn(s) + Cu2+ (aq) $\buildrel \, \over \longrightarrow $ Zn2+ (aq) + Cu(s)
The standard reaction enthalpy ($\Delta $rH${^o }$) at 300 K in kJ mol–1 is, [Use R = 8 JK–1 mol–1 and F = 96,000C mol–1]
The cell reaction is
Zn(s) + Cu2+ (aq) $\buildrel \, \over \longrightarrow $ Zn2+ (aq) + Cu(s)
The standard reaction enthalpy ($\Delta $rH${^o }$) at 300 K in kJ mol–1 is, [Use R = 8 JK–1 mol–1 and F = 96,000C mol–1]
A.
$-$ 412.8
B.
$-$ 384.0
C.
192.0
D.
206.4
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 11th January Evening Slot
Given the equilibrium constant:
KC of the reaction :
Cu(s) + 2Ag+ (aq) $ \to $ Cu2+ (aq) + 2Ag(s) is
10 $ \times $ 1015, calculate the E$_{cell}^0$ of this reaciton at 298 K
[2.303 ${{RT} \over F}$ at 298 K = 0.059V]
KC of the reaction :
Cu(s) + 2Ag+ (aq) $ \to $ Cu2+ (aq) + 2Ag(s) is
10 $ \times $ 1015, calculate the E$_{cell}^0$ of this reaciton at 298 K
[2.303 ${{RT} \over F}$ at 298 K = 0.059V]
A.
0.4736 mV
B.
0.04736 V
C.
0.4736 V
D.
0.04736 mV
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 11th January Morning Slot
For the cell Zn(s) |Zn2+ (aq)| |Mx+ (aq)| M(s), different half cells and their standard electrode potentials are given below :
If $E_{z{n^{2 + }}/zn}^0$ = $-$ 0.76 V, which cathode will give maximum value of Eocell per electron transferred?
| Mx+ (aq)/M(s) | Au3+(aq)/Au(s) | Ag+(aq)/Ag(s) | Fe3+(aq)/Fe2+ (aq) | Fe2+(aq)/Fe(s) |
|---|---|---|---|---|
| E0Mx+/M/(V) | 1.40 | 0.80 | 0.77 | $-$0.44 |
If $E_{z{n^{2 + }}/zn}^0$ = $-$ 0.76 V, which cathode will give maximum value of Eocell per electron transferred?
A.
Ag+/Ag
B.
Fe3+/Fe2+
C.
Au3+/Au
D.
Fe2+/Fe
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 10th January Evening Slot
In the cell
Pt$\left| {\left( s \right)} \right|$H2(g, 1 bar)$\left| {HCl\left( {aq} \right)} \right|$AgCl$\left| {\left( s \right)} \right|$Ag(s)|Pt(s)
the cell potential is 0.92 V when a 10–6 molal HCl solution is used. The standard electrode potential of (AgCl/ AgCl– ) electrode is :
$\left\{ {} \right.$Given, ${{2.303RT} \over F} = 0.06V$ at $\left. {298} \right\}$
Pt$\left| {\left( s \right)} \right|$H2(g, 1 bar)$\left| {HCl\left( {aq} \right)} \right|$AgCl$\left| {\left( s \right)} \right|$Ag(s)|Pt(s)
the cell potential is 0.92 V when a 10–6 molal HCl solution is used. The standard electrode potential of (AgCl/ AgCl– ) electrode is :
$\left\{ {} \right.$Given, ${{2.303RT} \over F} = 0.06V$ at $\left. {298} \right\}$
A.
0.94 V
B.
0.40 V
C.
0.76 V
D.
0.20 V
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 10th January Morning Slot
Consider the following reduction processes :
Zn2+ + 2e– $ \to $ Zn(s) ; Eo = – 0.76 V
Ca2+ + 2e– $ \to $ Ca(s); Eo = –2.87 V
Mg2+ + 2e– $ \to $ Mg(s) ; Eo = – 2.36 V
Ni2 + 2e– $ \to $ Ni(s) ; Eo = – 0.25
The reducing power of the metals increases in the order :
Zn2+ + 2e– $ \to $ Zn(s) ; Eo = – 0.76 V
Ca2+ + 2e– $ \to $ Ca(s); Eo = –2.87 V
Mg2+ + 2e– $ \to $ Mg(s) ; Eo = – 2.36 V
Ni2 + 2e– $ \to $ Ni(s) ; Eo = – 0.25
The reducing power of the metals increases in the order :
A.
Ca < Mg < Zn < Ni
B.
Ni < Zn < Mg < Ca
C.
Zn < Mg < Ni < Ca
D.
Ca < Zn < Mg < Ni
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 9th January Evening Slot
If the standard electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction
Zn(s) + Cu2+ (aq) $\rightleftharpoons$ Zn2+(aq) + Cu(s)
at 300 K is approximately,
(R = 8 JK$-$1mol$-$1, F = 96000 C mol$-$1)
Zn(s) + Cu2+ (aq) $\rightleftharpoons$ Zn2+(aq) + Cu(s)
at 300 K is approximately,
(R = 8 JK$-$1mol$-$1, F = 96000 C mol$-$1)
A.
e$-$80
B.
e$-$160
C.
e320
D.
e160
2019
JEE Mains
MCQ
JEE Main 2019 (Online) 9th January Morning Slot
The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of PbSO4 electrolyzed in g during the process is : (Molar mass of PbSO4 = 303 g mol$-$1)
A.
22.8
B.
15.2
C.
7.6
D.
11.4
2018
JEE Mains
MCQ
JEE Main 2018 (Online) 16th April Morning Slot
When 9.65 ampere current was passed for 1.0 hour into nitrobenzene in acidic medium, the amount of p-aminophenol produced is :
A.
9.81 g
B.
10.9 g
C.
98.1 g
D.
109.0 g
2018
JEE Mains
MCQ
JEE Main 2018 (Offline)
How long (approximate) should water be electrolysed by passing through 100 amperes current so that the
oxygen released can completely burn 27.66 g of diborane?
(Atomic weight of B = 10.8 u)
(Atomic weight of B = 10.8 u)
A.
1.6 hours
B.
6.4 hours
C.
0.8 hours
D.
3.2 hours
2018
JEE Mains
MCQ
JEE Main 2018 (Online) 15th April Morning Slot
When an electric currents passed through acidified water, 112 mL of hydrogen gas at N.T.P. was collected at the cathode in 965 seconds. The current passed, in ampere, is :
A.
1.0
B.
0.5
C.
0.1
D.
2.0
2017
JEE Mains
MCQ
JEE Main 2017 (Online) 9th April Morning Slot
To find the standard potential of M3+/M electrode,the following cell is constituted : Pt/M/M3+(0.001 mol L−1 )/Ag+(0.01 mol L−1 )/Ag
The emf of the cell is found to be 0.421 volt at 298 K. The standard potential of half reaction M3+ + 3e−$ \to $ M at 298 K will be :
(Given $E_{A{g^ + }\,/\,Ag}^ - $ at 298 K = 0.80 Volt)
The emf of the cell is found to be 0.421 volt at 298 K. The standard potential of half reaction M3+ + 3e−$ \to $ M at 298 K will be :
(Given $E_{A{g^ + }\,/\,Ag}^ - $ at 298 K = 0.80 Volt)
A.
0.38 Volt
B.
0.32 Volt
C.
1.28 Volt
D.
0.66 Volt
2017
JEE Mains
MCQ
JEE Main 2017 (Online) 8th April Morning Slot
Consider the following standard electrode potentials (Eo in volts) in aqueous solution :
Based on these data, which of the following statements is correct ?
| Element | M3+ /M | M+ /M |
|---|---|---|
| A1 | -1.66 | + 0.55 |
| T1 | +1.26 | - 0.34 |
Based on these data, which of the following statements is correct ?
A.
T1+ is more stable than A13+
B.
A1+ is more stable than A13+
C.
T1 + is more stable than A1+
D.
T13+ is more stable than A13+
2017
JEE Mains
MCQ
JEE Main 2017 (Online) 8th April Morning Slot
What is the standard reduction potential (Eo) for Fe3+ $ \to $ Fe ?
Given that :
Fe2+ + 2e$-$ $ \to $ Fe; $E_{F{e^{2 + }}/Fe}^o$ = $-$0.47 V
Fe3+ + e$-$ $ \to $ Fe2+; $E_{F{e^{3 + }}/F{e^{2 + }}}^o$ = +0.77 V
Given that :
Fe2+ + 2e$-$ $ \to $ Fe; $E_{F{e^{2 + }}/Fe}^o$ = $-$0.47 V
Fe3+ + e$-$ $ \to $ Fe2+; $E_{F{e^{3 + }}/F{e^{2 + }}}^o$ = +0.77 V
A.
$-$ 0.057 V
B.
+ 0.057 V
C.
+ 0.30 V
D.
$-$ 0.30 V
2017
JEE Mains
MCQ
JEE Main 2017 (Offline)
Given
$E_{C{l_2}/C{l^ - }}^o$ = 1.36 V, $E_{C{r^{3 + }}/Cr}^o$ = - 0.74 V
$E_{C{r_2}{O_7}^{2 - }/C{r^{3 + }}}^o$ = 1.33 V, $E_{Mn{O_4}^ - /Mn ^{2+}}^o$ = 1.51 V
Among the following, the strongest reducing agent is :
$E_{C{l_2}/C{l^ - }}^o$ = 1.36 V, $E_{C{r^{3 + }}/Cr}^o$ = - 0.74 V
$E_{C{r_2}{O_7}^{2 - }/C{r^{3 + }}}^o$ = 1.33 V, $E_{Mn{O_4}^ - /Mn ^{2+}}^o$ = 1.51 V
Among the following, the strongest reducing agent is :
A.
Mn2+
B.
Cr3+
C.
Cl–
D.
Cr
2016
JEE Mains
MCQ
JEE Main 2016 (Online) 10th April Morning Slot
Identify the correct statement :
A.
Iron corrodes in oxygen-free water.
B.
Iron corrodes more rapidly in salt water because its electrochemical
potential is higher.
C.
Corrosion of iron can be minimized by forming a contact with another
metal with a higher reduction potential.
D.
Corrosion of iron can be minimized by forming an impermeable barrier
at its surface.
2016
JEE Mains
MCQ
JEE Main 2016 (Online) 10th April Morning Slot
Oxidation of succinate ion produces ethylene and carbon dioxide gases. On passing 0.2 Faraday electricity through an aqueous solution of potassium succinate, the total volume of gases (at both cathode and anode) at STP (1 atm and 273 K) is :
A.
2.24 L
B.
4.48 L
C.
6.72 L
D.
8.96 L
2016
JEE Mains
MCQ
JEE Main 2016 (Online) 9th April Morning Slot
What will occur if a block of copper metal is dropped into a beaker containing a
solution of 1M ZnSO4?
A.
The copper metal will dissolve and zinc metal will be deposited.
B.
The copper metal will dissolve with evolution of hydrogen gas.
C.
The copper metal will dissolve with evolution of oxygen gas.
D.
No reaction will occur.
2016
JEE Mains
MCQ
JEE Main 2016 (Offline)
Galvanization is applying a coating of :
A.
Cr
B.
Cu
C.
Zn
D.
Pb
2015
JEE Mains
MCQ
JEE Main 2015 (Offline)
Two Faraday of electricity is passed through a solution of CuSO4. The mass of copper deposited at the
cathode is: (at. mass of Cu = 63.5 amu)
A.
63.5 g
B.
2 g
C.
127 g
D.
0 g
2014
JEE Mains
MCQ
JEE Main 2014 (Offline)
The equivalent conductance of NaCl at concentration C and at infinite dilution are ${\lambda _C}$ and ${\lambda _\infty }$, respectively. The correct relationship between ${\lambda _C}$ and ${\lambda _\infty }$ is given as:
(where the constant B is positive)
A.
${\lambda _C} = {\lambda _\infty } + (B)C$
B.
${\lambda _C} = {\lambda _\infty } - (B)C$
C.
${\lambda _C} = {\lambda _\infty } - (B)\sqrt C$
D.
${\lambda _C} = {\lambda _\infty } + (B)\sqrt C$
2014
JEE Mains
MCQ
JEE Main 2014 (Offline)
Resistance of 0.2 M solution of an electrolyte is 50 $\Omega$. The specific conductance of the solution is 1.4 S m-1. The resistance of 0.5 M solution of the same electrolyte is 280 $\Omega$. The molar conductivity of 0.5 M solution of the electrolyte in S m2 mol-1 is :
A.
5 × 103
B.
5 × 102
C.
5 × 10-4
D.
5 × 10-3
2014
JEE Mains
MCQ
JEE Main 2014 (Offline)
Given below are the half-cell reactions:
Mn2+ + 2e- $\to$ Mn; Eo = -1.18 V
2(Mn3+ + e- $\to$ Mn2+); Eo = +1.51 V
The Eo for 3Mn2+ $\to$ Mn + 2Mn3+ will be :
Mn2+ + 2e- $\to$ Mn; Eo = -1.18 V
2(Mn3+ + e- $\to$ Mn2+); Eo = +1.51 V
The Eo for 3Mn2+ $\to$ Mn + 2Mn3+ will be :
A.
– 0.33 V; the reaction will not occur
B.
– 0.33 V; the reaction will occur
C.
– 2.69 V; the reaction will not occur
D.
– 2.69 V; the reaction will occur
2013
JEE Mains
MCQ
JEE Main 2013 (Offline)
Given
$E_{C{r^{2 + }}/Cr}^o$ = -0.74 V; $E_{MnO_4^ - /M{n^{2 + }}}^o$ = 1.51 V
$E_{C{r_2}O_7^{2 - }/C{r^{3 + }}}^o$ = 1.33 V; $E_{Cl/C{l^ - }}^o$ = 1.36 V
Based on the data given above, strongest oxidising agent will be :
$E_{C{r^{2 + }}/Cr}^o$ = -0.74 V; $E_{MnO_4^ - /M{n^{2 + }}}^o$ = 1.51 V
$E_{C{r_2}O_7^{2 - }/C{r^{3 + }}}^o$ = 1.33 V; $E_{Cl/C{l^ - }}^o$ = 1.36 V
Based on the data given above, strongest oxidising agent will be :
A.
Cr3+
B.
Mn2+
C.
$MnO_4^ - $
D.
Cl-
2012
JEE Mains
MCQ
AIEEE 2012
The standard reduction potentials for Zn2+/ Zn, Ni2+/ Ni, and Fe2+/ Fe are –0.76, –0.23 and –0.44 V respectively. The reaction
X + Y2+ $\to$ X2+ + Y will be spontaneous when :
X + Y2+ $\to$ X2+ + Y will be spontaneous when :
A.
X = Ni, Y = Fe
B.
X = Ni, Y = Zn
C.
X = Fe, Y = Zn
D.
X = Zn, Y = Ni
2011
JEE Mains
MCQ
AIEEE 2011
The reduction potential of hydrogen half cell will be negative if :
A.
p(H2) = 1 atm and [H+] = 1.0 M
B.
p(H2) = 1 atm and [H+] = 2.0 M
C.
p(H2) = 2 atm and [H+] =1.0 M
D.
p(H2) = 2 atm and [H+] =2.0 M
2010
JEE Mains
MCQ
AIEEE 2010
The correct order of $E_{{M^{2 + }}/M}^o$ values with negative sign for the four successive elements Cr, Mn, Fe
and Co is :
A.
Mn > Cr > Fe > Co
B.
Cr > Fe > Mn > Co
C.
Fe > Mn > Cr > Co
D.
Cr > Mn > Fe > Co
2010
JEE Mains
MCQ
AIEEE 2010
The Gibbs energy for the decomposition of Al2O3 at 500oC is as follows :
${2 \over 3}A{l_2}{O_3}$ $\to$ ${4 \over 3}Al + {O_2}$, ${\Delta _r}G$ = + 966 kJ mol–1
The potential difference needed for electrolytic reduction of Al2O3 at 500oC is at least :
${2 \over 3}A{l_2}{O_3}$ $\to$ ${4 \over 3}Al + {O_2}$, ${\Delta _r}G$ = + 966 kJ mol–1
The potential difference needed for electrolytic reduction of Al2O3 at 500oC is at least :
A.
4.5 V
B.
3.0 V
C.
2.5 V
D.
5.0 V
2009
JEE Mains
MCQ
AIEEE 2009
Given : $E_{F{e^{3 + }}/Fe}^o$ = -0.036V; $E_{F{e^{2 + }}/Fe}^o$ = -0.439 V
The value of standard electrode potential for the change,
Fe3+ (aq) + e- $\to$ Fe2+ (aq) will be
The value of standard electrode potential for the change,
Fe3+ (aq) + e- $\to$ Fe2+ (aq) will be
A.
-0.072 V
B.
0.385 V
C.
0.770 V
D.
0.270
2009
JEE Mains
MCQ
AIEEE 2009
In a fuel cell methanol is used as fuel and oxygen gas is used as an oxidizer. The reaction is
CH3OH(l) + 3/2O2 $\to$ CO2 (g) + 2H2O (l)
At 298K standard Gibb’s energies of formation for CH3OH(l), H2O(l) and CO2 (g) are -166.2, -237.2 and -394.4 kJ mol−1 respectively. If standard enthalpy of combustion of methanol is -726 kJ mol−1, efficiency of the fuel cell will be
CH3OH(l) + 3/2O2 $\to$ CO2 (g) + 2H2O (l)
At 298K standard Gibb’s energies of formation for CH3OH(l), H2O(l) and CO2 (g) are -166.2, -237.2 and -394.4 kJ mol−1 respectively. If standard enthalpy of combustion of methanol is -726 kJ mol−1, efficiency of the fuel cell will be
A.
87%
B.
90%
C.
97%
D.
80%
2008
JEE Mains
MCQ
AIEEE 2008
Given $E_{C{r^{3 + }}/Cr}^o$ = -0.72 V; $E_{Fe^{2+}/Fe}^o$ = -0.42V, The potential for the cell Cr | Cr3+ (0.1M) || Fe2+ (0.01 M) | Fe is
A.
0.26 V
B.
0.399 V
C.
−0.339 V
D.
−0.26 V
2007
JEE Mains
MCQ
AIEEE 2007
The equivalent conductances of two strong electrolytes at infinite dilution in H2O (where ions move
freely through a solution) at 25oC are given below:
$ \wedge _{C{H_3}COONa}^o$ = 91.0 S cm2/equiv
$ \wedge _{HCl}^o$ = 426.2 S cm2/equiv
What additional information/quantity one needs to calculate $ \wedge ^o$ of an aqueous solution of acetic acid?
$ \wedge _{C{H_3}COONa}^o$ = 91.0 S cm2/equiv
$ \wedge _{HCl}^o$ = 426.2 S cm2/equiv
What additional information/quantity one needs to calculate $ \wedge ^o$ of an aqueous solution of acetic acid?
A.
$ \wedge ^o$ of chloroacetic acid (C/CH2COOH)
B.
$ \wedge ^o$ of NaCl
C.
$ \wedge ^o$ of CH3COOK
D.
The limiting equivalent conductance of ${H^ + }( \wedge _{{H^ + }}^o)$
2007
JEE Mains
MCQ
AIEEE 2007
The cell, Zn | Zn2+ (1M) || Cu2+ (1M) | Cu($E_{cell}^o$ = 1.10V) was allowed to be completely discharged at 298 K. The relative concentration of Zn2+ to Cu2+ $\left[ {{{\left[ {Z{n^{2 + }}} \right]} \over {\left[ {C{u^{2 + }}} \right]}}} \right]$ is
A.
antilog (24.08)
B.
37.3
C.
1037.3
D.
9.65 $\times$ 104
2006
JEE Mains
MCQ
AIEEE 2006
The molar conductivities $ \wedge _{NaOAc}^o$ and $ \wedge _{HCl}^o$ and at infinite dilution in water at 25oC are 91.0 and 426.2 Scm2/mol respectively. To calculate $ \wedge _{HOAc}^o$ , the additional value required is
A.
$ \wedge _{{H_2}O}^o$
B.
$ \wedge _{KCl}^o$
C.
$ \wedge _{NaOH}^o$
D.
$ \wedge _{NaCl}^o$
2006
JEE Mains
MCQ
AIEEE 2006
Given the data at 25oC,
Ag + I- $\to$ AgI + e- , Eo = 0.152 V
Ag $\to$ Ag+ + e-, Eo = -0.800 V
What is the value of log Ksp for AgI? (2.303 RT/F = 0.059 V)
Ag + I- $\to$ AgI + e- , Eo = 0.152 V
Ag $\to$ Ag+ + e-, Eo = -0.800 V
What is the value of log Ksp for AgI? (2.303 RT/F = 0.059 V)
A.
–8.12
B.
+8.612
C.
–37.83
D.
–16.13
2006
JEE Mains
MCQ
AIEEE 2006
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 S m–1. Resistance of the same cell when filled with 0.2 M of
the same solution is 520 $\Omega $, The molar conductivity of 0.02 M solution of the electrolyte will be
A.
124 $\times$ 10–4 S m2 mol–1
B.
1240 $\times$ 10–4 S m2 mol–1
C.
1.24 $\times$ 10–4 S m2 mol–1
D.
12.4 $\times$ 10–4 S m2 mol–1
2005
JEE Mains
MCQ
AIEEE 2005
The highest electrical conductivity of the following aqueous solutions is of :
A.
0.1 M acetic acid
B.
0.1 M chloroacetic acid
C.
0.1 M fluoroacetic acid
D.
0.1 M difluoroacetic acid
2005
JEE Mains
MCQ
AIEEE 2005
| Electrolyte: | KCl | KNO3 | HCl | NaOAc | NaCl |
|---|---|---|---|---|---|
| ${ \wedge ^\infty }(Sc{m^2}mo{l^{ - 1}}):$ |
149.9 | 145 | 426.2 | 91 | 126.5 |
A.
517.2
B.
552.7
C.
390.7
D.
217.5
2005
JEE Mains
MCQ
AIEEE 2005
For a spontaneous reaction the ∆G , equilibrium constant (K) and $E_{cell}^o$ will be respectively
A.
-ve, >1, +ve
B.
+ve, >1, -ve
C.
-ve, <1, -ve
D.
-ve, >1, -ve