NEET Questions - Chemistry - Redox Reactions & Electrochemisty

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Question bank:

How much time is required for the complete decomposition of 2 moles of water using a current of 2 ampere-

26.805 h
53.61 h
107.22 h
None of these

A certain current liberates 0.504 g of hydrogen in 2 hours. How many gram of copper can be liberated by the same current flowing for the same time in aqueous $C u S O_{4}$ solution :

12.7
16
31.8
63.5

Calculate the maximum work that can be obtained from the Daniell cell given below -

$Z n (s) | Z n^{2 +} (a q) | | C u^{2 +} (a q) | C u (s) .$

Given that $E_{Z n^{2 +} / Z n}^{°} = - 0.76 V a n d E_{C u^{2 +} / C u}^{°} = + 0.34 V$

– 212300 J
– 202100 J
– 513100 J
– 232120 J

The metal that cannot be produced on reduction of its oxide by aluminium is :

K
Mn
Cr
Fe

We have taken a saturated solution of $A g B r, K_{s p}$ of AgBr is $12 \times 10^{- 14} .$ If $10^{- 7}$ mole of $A g N O_{3}$ are added to 1 litre of this solution then the conductivity of this solution in terms of $10^{- 7}$ $S m^{- 1}$ units will be

$[λ °_{(A g^{+})} = 4 \times 10^{- 3} S m^{2} m o l^{- 1}; λ °_{(B r^{-})} = 6 \times 10^{- 3} S m^{2} m o l^{- 1}, λ °_{(N O_{3}^{-})} = 5 \times 10^{- 3} S m^{2} m o l^{- 1}]$

39
55
15
41

The standard reduction potentials, $E^{\circ}$ , for the half reactions are as $Z n = Z n^{2 +} + 2 e; E ° = + 0.76 V$ and $F e = F e^{2 +} + 2 e; E ° = + 0.41$ V; the e.m.f. for the cell reaction, $F e^{2 +} + Z n = Z n^{2 +} + F e i s -$

– 0.35 V
+ 0.35 V
+ 1.17 V
– 1.17 V

The calomel electrode is reversible with respect to-

Mercury

H^{+}

H g^{2 +}

C l^{-}

Zn amalgam is prepared by electrolysis of aqueous $Z n C l_{2}$ using Hg cathode (9 gm). How much current is to be passed through $Z n C l_{2}$ solution for 1000 seconds to prepare a Zn Amalgam with 25% Zn by wt. (Zn = 65.4)

5.6 amp
7.2 amp
8.85 amp
11.2 amp

The standard oxidation potentials of $C u / C u^{2 +}$ and $C u^{+} / C u^{2 +} a r e - 0.34 V a n d - 0.16 V$ respectively. The standard electrode potential of $C u^{+} / C u$ would be :

0.18V
0.52V
0.82V
0.49V

Acidified water is electrolysed using an inert electrode. The volume of gases liberated at STP is 0.168L. The quantity of charge passed through the acidified water would be:

96,500 C
9,650 C
965 C
168 C

$E^{0} f o r t h e r e a c t i o n F e + Z n^{2 +} = Z n + F e^{2 +} i s - 0.35 V . T h e g i v e n c e l l r e a c t i o n i s -$

Feasible
Not feasible
In equilibrium
None

How much charge should be supplied to a cell for the electrolytic production of 245 gm $N a C l O_{4}$ from $N a C l O_{3}$ if the anode efficiency for the required reaction is 60%?

6.43 ×

10^{5} C

6.67 F
6.43 ×

10^{6} C

66.67 F

During an electrolysis of conc. $H_{2} S O_{4}$ , perdisulphuric acid $(H_{2} S_{2} O_{8}) a n d O_{2}$ form in equimolar amount. The amount of $H_{2}$ that will form simultaneously will be

$(2 H_{2} S O_{4} \to H_{2} S_{2} O_{8} + 2 H^{+} + 2 e^{-})$

thrice that of

O_{2}

in moles
twice that of

O_{2}

in moles
equal to that of

O_{2}

in moles
half of that of

O_{2}

in moles

The specific conductivity of solution depends upon :

Number of ions as well as mobility of ions
Number of ions per c.c solution
Number of ions per c.c as well as mobilities of ions
Mobilities of ions only

Value of ${\land_{m}}^{0}$ for $S r C l_{2}$ in water at $25 ° C$ from the following data

Conc. (mol/It) 0.25 1

$\land_{m} (Ω^{- 1} c m^{2} m o l^{- 1})$ 260 250

270
260
250
255

NEET Chemistry Questions: Redox Reactions & Electrochemisty

Question bank:

How much time is required for the complete decomposition of 2 moles of water using a current of 2 ampere-

A certain current liberates 0.504 g of hydrogen in 2 hours. How many gram of copper can be liberated by the same current flowing for the same time in aqueous CuSO4 solution :

Calculate the maximum work that can be obtained from the Daniell cell given below - Zn(s) | Zn2+ (aq) || Cu2+ (aq) | Cu(s). Given that EZn2+/Zn°=-0.76 V and ECu2+/Cu°=+0.34 V

The metal that cannot be produced on reduction of its oxide by aluminium is :

We have taken a saturated solution of AgBr, Ksp of AgBr is 12 × 10-14. If 10-7mole of AgNO3 are added to 1 litre of this solution then the conductivity of this solution in terms of 10-7 Sm-1 units will be [λ°Ag+=4×10-3Sm2mol-1 ;λ°Br-=6×10-3Sm2mol-1,λ°NO3-=5×10-3Sm2mol-1]

The standard reduction potentials, E∘, for the half reactions are as Zn = Zn2++ 2e; E° = + 0.76 Vand Fe = Fe2+ + 2e ; E° = + 0.41 V; the e.m.f. for the cell reaction, Fe2++ Zn = Zn2++ Fe is-

The calomel electrode is reversible with respect to-

Zn amalgam is prepared by electrolysis of aqueous ZnCl2 using Hg cathode (9 gm). How much current is to be passed through ZnCl2 solution for 1000 seconds to prepare a Zn Amalgam with 25% Zn by wt. (Zn = 65.4)

The standard oxidation potentials of Cu/Cu2+and Cu+ /Cu2+ are – 0.34V and – 0.16 Vrespectively. The standard electrode potential of Cu+ /Cu would be :