NEET Questions - Chemistry - Redox Reactions & Electrochemisty

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If cell potential of standard cell is 0.59 V then equilibrium constant for the cell reaction occuring in the cell at $ 25 ^\circ C $ is _______. (n = 1)

1
10.0
$ 10 ^ {10} $
1/10

Which of the following cell is different?

Daniel cell
lead storage cell
laclanche cell
electrolytic cell

If equilibrium constant of a cell for reaction occuring in the electrochemical cell is $ 1.9413 \times 10^{37} at 25 ^\circ C $ then what is the std. cell potential of the cell (n=2)

2.2 v
1.1 V
0.0085 V
0.013 V

On which of the following cell potential of the cell does not depend?

temperature
concentration fo the solution of salt bridge
concentration of the solution related with cell reaction
nature of electrodes

What is the value of term $ {2.303 RT \over F} in nemst equation at 80 ^\circ $ C ?

0.007 V
0.01587 V
0.01857 V
0.07 V

Mention n and Q for the cell reaction taking place in the $ Pt ∣ Cl_{2(g,1.0 bar) ∣ Cl ^−_{(C_1)}|| Au^{3+}_{(C_2)} ∣ Au $ cell.

$ n = 6 , Q = {[Cl^−]^6 \over [Au ^{3+} ] ^ 2 }$
$ n = 6 , Q = [Au ^{3+} ] ^ 2 [Cl^−]^6 $
$ n = 6 , Q = [Au ^{3+} ] [Cl^−]^3 $
$ n = 6 , Q = { 1 \over [Au ^{3+} ] ^ 2 [Cl^−]^6 }$

Mention the oxidation reaction takes place in half cell $Pt ∣ H_{2(g,1.0 bar)} ∣ OH−^_{(aq)} $ .

$ H_{2(g)} + 2OH^− \rightleftharpoons 2H_2O_{(l)} + 2e^− $
$ 2OH^- \rightleftharpoons H_{2(g)} + O_{2(g)} + 2e^− $
$ H_2 O_{(I)} + 2 OH ^ - _{(aq)} \rightleftharpoons 3 H_{2(g)} + 2 e ^ - $
$ H_{2(g)} + 2 OH ^ - _{(aq)} \rightleftharpoons 2 H_2O _{(I)} + O_{2(g)} + 2 e ^ - $

Which of the following relation is correct for Faradays 2nd law? where and is quanitity of substance while and are equivalent mass of the substance.

$ m_1 E_1 = m_2 E_2 $
$ m_1 E_2 = m_2 E_1 $
$ m_1 + m_2 = E_1 + E_2 $
$ E_1 E_2 = m_1 m_2 $

Which of the following cell representation is in correct with reference to cell reaction taking place in the cell at $ 25 ^\circ C ? (E ^\circ _{{Pb}^{2 +} |Pb} = − 0.13 V. , E ^\circ _{ Sn^{2+}|Sn}= − 0.14 V.) $

$ Sn| Sn ^{2+} _{(0.1M)} || Pb ^{2+} _{(0.01M)} | Pb $
$ Sn| Sn ^{2+} _{(0.02M)} || Pb ^{2+} _{(0.2M)} | Pb $
$ Pb |Pb ^{2+} _{(0.01M)} || Sn ^{2+} _{(0.1M)} | Sn$
$ Sn| Sn ^{2+} _{(0.05M)} || Pb ^{2+} _{(0.5M)} | Pb $

A2+ | A, B2+| B, C2+ | D is increasing order of std. reduction potential then choose correct option for the given state ments. (T = true and F = false ) (i) rod of metal A dissolve in the solution of metal $ B^{2+} $ (ii) solution of $ A^{2+} $ ion can not be filled in the container of the metal C. (iii) reaction $ D_{(s)} + B^{2+} _{(aq1.0M)} \rightleftharpoons D^{2+} _{( aq 0.1 M)} + B_{(s)} $ spontaneously in forward direction. (iv) atoms of metal C can not displace $ B^{2+} $ ioin from its solution.

TFFT
FTTF
FTFT
TFTF

What is the value of $ E_{Mg | Mg ^{2+} _{(0.5 M)}} at 25 ^\circ C ? ( E^ \circ _{Mg|Mg ^{ 2+} = 2.36 V. ) $

2.3689 V
-2.3689 V
2.88V
-2.38 V

If potential of the cell formed by connecting half cell Ag | Ag+ and Al | Al3+ is 2.546V then what is the std. cell potential of the cell at 250C?

1.46 V
2.46 V
2.64 V
2 .76 V

For cell $ Mg | Mg^{2+} _{(0.005M)} ║ Ag^+_{0.04M} | Ag $ which of the following option is correct for the value of Q related to n ?

$ n = 1, Q = 3.125 M^{1/2} $
n = 2, Q = 1.7677 M
$ n = 3, Q = 5.5243 M ^ {3/2} $
$n = 4, Q = 0.156 M ^ 2 $

For the cell $ Co | Co^ {2+} _{(0.04M)} | Cl^-_{(0.1M)}| Cl_{2(g,1.0 bar)}| Pt $ which of the following option is correct for the value of Q related to the value of n? (a) n = 1 (b) n = 2 (c) n = 3 (d) n = 4 (1) $ Q = 4.0 \times 10 ^ {-4} M^3 $ (2) $ Q = 8 M ^ {-3/2} $ (3) $ Q = 8.0 \times 10 ^ {-6} M ^ {9/2} $ (4) $ Q = 2 M ^ {-1/2} $ (5) $ Q = 4 M^{-1} $ (6) $ Q = 1.6 × 10^{-7} M^6 $ (7) $ Q = 0.002 M ^ {3/2} $ (8) $ Q = 16 M ^ {-2} $

a – 4, b − 5, c – 2, d − 8
a – 7, b – 5, c – 2, d − 6
a – 7, b – 1, c – 3, d − 6
a – 4, b – 8, c – 7, d − 1

For the cell $ Pt | Br_{2(g,1.0 bar)} | Br ^ - _{(0.5M)} || Au ^{3+}_{(0.4M)} | Au value of Q = 20M^{-4} $ then what is the appropriate value of n?

n =6
n = 2
n = 3
n =4

NEET Chemistry Questions: Redox Reactions & Electrochemisty