NEET Questions - Chemistry - Redox Reactions & Electrochemisty

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Question bank:

If temperature of the cell $ Mg | Mg^{2+}_{(0.005M)} || Ag^+_{(0.04M)} | Ag $ increases then what changes observed in the cell potential of the cell?

increases
decreases
do not change
cannot predict

If temperature of the cell $ Ni | Ni^{2+} _{0.05M} || Cu^{2+}_{(0.08M)} | Cu $ increases then what changes observed (0.05 M) in the cell potential of the cell?

increases
decreases
do not change
cannot predict

If temperature of the cell $ Fe | Fe^{2+}_{(xM)} || Cu^{2+} _{(0.08M)} | Cu $ decreases then theoritically cell potential of the cell increases then which value of x is possible?

x = 0.5
x = 0.02
x =0.05
x = 0.04

If temperature of the cell $ Zn | Zn^{2+}_{C_1} || Sn^{2+}_{C_2} | Sn (C_1 < C_2) $ decreases then theoritically cell potential what changes are observed in the cell potential of the cell?

increases
decreases
do not change
cannot predict

What is the equilibrium constant of the reaction taking place in the cell $ Zn | Zn^{2+}_{(C-1)} || Cu^{2+}_{(C-2)} | Cu at 25 ^\circ C? ( E ^ \circ _{Zn ^{2+} |Zn} = − 0.76 V., E ^\circ Cu ^{ 2+} | Cu= 0.34 V.)$

3.3791
$ 1.9413 \times 10 ^ {37 } $
$ 4.406 \times 10 ^ {18} $
$ 5.15 \times 10 ^ {-38} $

If for the reaction taking place in one electrochemical cell $ Kc = 1.3141 \times 10^{107} M^{– 1} $ and n = 2 then for that cell value of E ^\circ $ Cell is _.

6.32 V
0.1186 V
0.32 V
3.16 V

If for the reaction taking place in an electrochemical cell $ c = 1.3141 \times 10^{307} $ and n = 6. if standard reduction potential of the cathode is 1.36 V then what is the standard oxidation potential of the anode?

6.32 V
1.66 V
2.71 V
3.16 V

What is the pH of the solution of HCl if cell potentila of the cell $ Pt | H_{2(g. 1.0 bar)}| HCl_{(xM)} || Au ^{3+}_{(0.001M)} | Au is 1.6655 V ? (E^0_{Au^{3+}|Au} = 1.4 V.) $

3.5
4.17
5.5
4.83

Mention the value of n for the reaction taking place in the cell if its cell potential is 3.16V and equilibrium constant is $ 1.727 \times 10^{214}M ^{-2} at 25 ^ \circ C $ temperature.

1
2
3
4

If for the cell $ Mg | Mg^{2+}_{(0.2M)} || H^+_{(xM)}∣ H_{2(g,1.0 bar )}|Pt $ values of E and $ E^0_{cell} are 2.3629 V.(0.2 M)(X M)Cell and 2.36 V. respectively at 25 ^\circ C $ temperature then value of x is _.

0.4 M
0.5 M
0.1 M
0.25 M

If standard potential of the reaction $ 2H_2O_(l) \rightleftharpoons O_{2(g,1 bar )} + 4H^+_{aq} + 4e^− is -1.23V and [H+] = 10^{-7} at 25 ^\circ C $ temperature then what is the value of potential for the reaction? OR What is the oxidation potential of the pure water?

-0.41 M
-2.62 M
-0.817 V
0.41 V

If for the reaction $ 2H_2O_(l) + 2 e ^ - \rightleftharpoons H_{2 (g, 1 bar)} + 2 OH ^ - _{aq, 10 ^ {-7} M } E = -0.417 V at 25 ^ \circ C $ temperature what is the value of E 0 for the reaction? OR what is the standard reduction potential of the pure water at $ 25 ^\circ C $ if potential is – 0.417 V.

-0.83 V
-2.62 V
-0.817 V
0.41 V

If $ Co | Co^{3+}, Co^{2+}| Co ^{3+}, Fe | Fe ^ {3+}, Fe^{2+}| Fe^{3+} std. oxidation potential are − 0.4167 V., − 1.81 V., 0.0367 V., − 0.77 V. respectively then what is the std. potential of the cell Fe | Fe^{2+} || Co^{2+} Co $ ?

0.72 V
-2.62 V
-0.817 V
0.41 V

If cell potentisl of the cell $ Pt | H_{2(g,1.0 bar ) | HCl_{(X M)}║ Cu ^{2+} _{(0.01)} | Cu 0.635 V. at 25 ^\circ C then what is the pH of the HCl solution? (E ^\circ Cu ^{2+}|Cu = 0.34 V.) $

0.72 V
-0.11V
1.0 V
0.16 V

If cell potentisl of the cell $ Mg | Mg^{2+}_{(0.01M)} ║ HCl_{(X M)} | H_{2(g,1.0 bar)}| Pt 2 .09V. at 25 ^\circ C then what is the pH of the HCl solution? (E ^0 _{Mg ^{2+}|Mg }= - 2.36 V )$

2
5
6
4

NEET Chemistry Questions: Redox Reactions & Electrochemisty

Question bank:

If temperature of the cell $ Mg | Mg^{2+}_{(0.005M)} || Ag^+_{(0.04M)} | Ag $ increases then what changes observed in the cell potential of the cell?

If temperature of the cell $ Ni | Ni^{2+} _{0.05M} || Cu^{2+}_{(0.08M)} | Cu $ increases then what changes observed (0.05 M) in the cell potential of the cell?

If temperature of the cell $ Fe | Fe^{2+}_{(xM)} || Cu^{2+} _{(0.08M)} | Cu $ decreases then theoritically cell potential of the cell increases then which value of x is possible?

If temperature of the cell $ Zn | Zn^{2+}_{C_1} || Sn^{2+}_{C_2} | Sn (C_1 < C_2) $ decreases then theoritically cell potential what changes are observed in the cell potential of the cell?

What is the equilibrium constant of the reaction taking place in the cell $ Zn | Zn^{2+}_{(C-1)} || Cu^{2+}_{(C-2)} | Cu at 25 ^\circ C? ( E ^ \circ _{Zn ^{2+} |Zn} = − 0.76 V., E ^\circ Cu ^{ 2+} | Cu= 0.34 V.)$

If for the reaction taking place in one electrochemical cell $ Kc = 1.3141 \times 10^{107} M^{– 1} $ and n = 2 then for that cell value of E ^\circ $ Cell is _.

If for the reaction taking place in an electrochemical cell $ c = 1.3141 \times 10^{307} $ and n = 6. if standard reduction potential of the cathode is 1.36 V then what is the standard oxidation potential of the anode?

What is the pH of the solution of HCl if cell potentila of the cell $ Pt | H_{2(g. 1.0 bar)}| HCl_{(xM)} || Au ^{3+}_{(0.001M)} | Au is 1.6655 V ? (E^0_{Au^{3+}|Au} = 1.4 V.) $

Mention the value of n for the reaction taking place in the cell if its cell potential is 3.16V and equilibrium constant is $ 1.727 \times 10^{214}M ^{-2} at 25 ^ \circ C $ temperature.

If for the cell $ Mg | Mg^{2+}_{(0.2M)} || H^+_{(xM)}∣ H_{2(g,1.0 bar )}|Pt $ values of E and $ E^0_{cell} are 2.3629 V.(0.2 M)(X M)Cell and 2.36 V. respectively at 25 ^\circ C $ temperature then value of x is _.

If standard potential of the reaction $ 2H_2O_(l) \rightleftharpoons O_{2(g,1 bar )} + 4H^+_{aq} + 4e^− is -1.23V and [H+] = 10^{-7} at 25 ^\circ C $ temperature then what is the value of potential for the reaction? OR What is the oxidation potential of the pure water?

If $ Co | Co^{3+}, Co^{2+}| Co ^{3+}, Fe | Fe ^ {3+}, Fe^{2+}| Fe^{3+} std. oxidation potential are − 0.4167 V., − 1.81 V., 0.0367 V., − 0.77 V. respectively then what is the std. potential of the cell Fe | Fe^{2+} || Co^{2+} Co $ ?

If cell potentisl of the cell $ Pt | H_{2(g,1.0 bar ) | HCl_{(X M)}║ Cu ^{2+} _{(0.01)} | Cu 0.635 V. at 25 ^\circ C then what is the pH of the HCl solution? (E ^\circ Cu ^{2+}|Cu = 0.34 V.) $

If cell potentisl of the cell $ Mg | Mg^{2+}_{(0.01M)} ║ HCl_{(X M)} | H_{2(g,1.0 bar)}| Pt 2 .09V. at 25 ^\circ C then what is the pH of the HCl solution? (E ^0 _{Mg ^{2+}|Mg }= - 2.36 V )$