NEET Questions - Chemistry - Redox Reactions & Electrochemisty

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Question bank:

At 298K the standard free energy of formation of H₂O(l) is –237.20kJ/mole while that of its ionisation into H+ iion and hydroxyl ions is 80 kJ/mole, then the emf of the following cell at 298 K will be

H₂(g,1 bar) | H⁺ (1M) || OH^–(1M) | O₂ (g, 1bar)

0.40 V
0.81 V
1.23 V
–0.40 V

Which of the following cell can produce more electric work.

pt,H₂|NH₄Cl||0.1MCH₃COOH|H₂,pt
pt,H₂|0.1MHCl||0.1MNaOH|H₂,pt
pt,H₂|0.1MHCl||0.1MCH₃COOK|H₂,pt
pt,H₂|0.1MCH₃COOK||0.1MHCl|H₂,pt

At what $\frac{[{Br}^{-}]}{\sqrt{[{CO}_{3}^{2 -}]}}$ does the following cell have its reaction at equilibrium?

Ag(s) | Ag₂CO₃(s) | Na₂CO₃ (aq) || KBr(aq) | AgBr(s) | Ag(s)

K_SP = 8 × 10^–12 for Ag₂CO₃ and K_SP = 4 × 10^–13 for AgBr

\sqrt{1}

× 10^–7

\sqrt{2}

× 10^–7

\sqrt{3}

× 10^–7

\sqrt{4}

× 10^–7

It is observed that the voltage of a galvanic cell using the reaction M(s) + xH⁺ $\to_{}^{}$ M^x+ + $\frac{x}{2}$ H₂ varies linearly with the log of the square root of the hydrogen pressure and the cube root of the M^x+ concentration. The value of x is

2
3
4
5

Acetic acid has K_a = 1.8 × 10^–5 while formic acid had K_a = 2.1 × 10^–4. What would be the magnitude of the emf of the cell

Pt(H₂) $|\begin{array}{l} 0 .1 M acetic acid + \\ 0 .1 M sodium acetate \end{array}| |\begin{array}{l} 0 .1 M formic acid + \\ 0 .1 M sodium formate \end{array}|$ Pt(H₂) at 25°C

0.0315 volt
0.0629 volt
0.0455 volt
0.0545 volt

Consider the cell Ag(s)|AgBr(s)|Br–(aq)||AgCl(s)|Cl–(aq)|Ag(s) at 25°C. The solubility product constants of AgBr & AgCl are respectively 5 × 10^–13 & 1 × 10^–10. For what ratio of the concentrations of Br^–& Cl^–ions would the emf of the cell be zero ?

1 : 2000
1 : 100
1 : 500
200 : 1

Value of ${Λ_{m}}^{\infty}$ for SrCl₂ in water at 25°C from the following data:

Conc. (mol/lt) 0.25 1

$Λ_{m}$ (Ω^–1 cm² mol^–1) 260 250

270
260
250
255

Calculate the useful work of the reaction Ag(s) + 1/2Cl₂(g) $\to_{}^{}$ AgCl(s)

Given $E °_{Cl 2 / {Cl}^{-}} = + 1.36 V, E °_{AgCl / Ag, {Cl}^{-}} = 0.22 V$

If $P_{{Cl}_{2}}$ = 1 atmand T = 298 K

110 kJ/mol
220 kJ/mol
55kJ/mol
1000 kJ/mol

Which of these ions Cu⁺, Co³⁺, Fe²⁺ is stable in aqueous medium.

Given :E°_Cu2+/Cu+ = 0.15 volt ; E°_Cu+/Cu = 0.53 V ;E°_Co3+/Co2+ = 1.82 V ;

E°_Fe3+/Fe2+ = 0.77 V ;E°_Fe2+Fe = –0.44 V ;E°_O2,H+/H2O = 1.23 V

Cu⁺, Co³⁺
Co³⁺
Cu⁺
Co³⁺, Cu⁺, Fe²⁺

Select the correct statement if –

E°_Mg2+/Mg = –2.4V, E°_Sn4+/Sn2+ = 0.1 V, E°_{MnO4–,H+/Mn2+} = 1.5 V, E° _I2/I–= 0.5 V

Here,

MnO₄^–is the strongest Oxidizing Agent and Mg is the strongest Reducing Agent.
Sn⁴⁺ + 2I^–

\to_{}^{}

Sn²⁺ + I₂ is a spontaneous reaction.
Mg²⁺ + Sn²⁺

\to_{}^{}

Mg + Sn⁴⁺ is a spontaneous reaction.
Weakest oxidizing agent is Sn⁴⁺ and weakest reducing agent is Mn²⁺.

The temperature coefficient of a standard Cd–cell is –5.0 $\times$ 10^–5 Vk^–1 whose emf at 25°C is 1.018 V. During the cell operation, the temperature will –

increase
decrease
either
remains constant

A cell Ag | Ag⁺ || Cu⁺⁺ | Cu initially contains 2M Ag⁺ and 2M Cu⁺⁺ ions. The charger in cell potential after the passage of 10 amp current for 4825 sec is:

–0.000738 V
–1.00738
–0.0038 V
none

For the cell (at 298 K)

Ag(s) | AgCl(s) | Cl^–(aq) || AgNO₃(aq) | Ag(s)

Which of the following is correct –

The cell emf will be zero when [Ag⁺]_a = [Ag⁺]_c ([Ag⁺] in anodic compartment = [Ag⁺] in cathodic compartment)
The amount of AgCl(s) precipitate in anodic compartment will decrease with the working of the cell.
The concentration of [Ag⁺] = constant, in anodic compartment during working of cell.
E_cell = E°_{Ag+ | Ag} –E°_{Cl–|AgCl|Ag}

− \frac{0 .059}{1} \log \frac{1}{{[{Cl}^{-}]}_{a}}

During an electrolysis of conc. H₂SO₄, perdisulphuric acid (H₂S₂O₈) and O₂ from in equimolar amount. The amount of H₂ that will form simultaneously will be (2H₂SO4 → H₂S₂O₈ + 2H⁺ + 2e^–)

thrice that of O₂ in moles
twice that of O₂ in moles
equal to that of O₂ in moles
half of that of O₂ in moles

In producing chlorine by electrolysis 100 kW power at 125V is being consumed.How much chlorine per minute is liberated (ECE of chlorine is 0.367 $\times 10^{- 6} k g C^{- 1}$ )

1.76 \times 10^{- 3} k g

9.67 \times 10^{- 3} k g

17.61 \times 10^{- 3} k g

3.67 \times 10^{- 3} k g

NEET Chemistry Questions: Redox Reactions & Electrochemisty

Question bank:

At 298K the standard free energy of formation of H2O(l) is –237.20kJ/mole while that of its ionisation into H+ iion and hydroxyl ions is 80 kJ/mole, then the emf of the following cell at 298 K will be H2(g,1 bar) | H+ (1M) || OH–(1M) | O2 (g, 1bar)

Which of the following cell can produce more electric work.

At what [Br-][CO32−] does the following cell have its reaction at equilibrium? Ag(s) | Ag2CO3(s) | Na2CO3 (aq) || KBr(aq) | AgBr(s) | Ag(s) KSP = 8 × 10–12 for Ag2CO3 and KSP = 4 × 10–13 for AgBr

It is observed that the voltage of a galvanic cell using the reaction M(s) + xH+ → Mx+ + x2 H2 varies linearly with the log of the square root of the hydrogen pressure and the cube root of the Mx+ concentration. The value of x is

Acetic acid has Ka = 1.8 × 10–5 while formic acid had Ka = 2.1 × 10–4. What would be the magnitude of the emf of the cell Pt(H2) 0.1M acetic acid+0.1M sodium acetate0.1M formic acid+0.1M sodium formate Pt(H2) at 25°C

Consider the cell Ag(s)|AgBr(s)|Br–(aq)||AgCl(s)|Cl–(aq)|Ag(s) at 25°C. The solubility product constants of AgBr & AgCl are respectively 5 × 10–13 & 1 × 10–10. For what ratio of the concentrations of Br– & Cl–ions would the emf of the cell be zero ?

Value of Λm∞ for SrCl2 in water at 25°C from the following data: Conc. (mol/lt) 0.25 1 Λm (Ω–1 cm2 mol–1) 260 250

Calculate the useful work of the reaction Ag(s) + 1/2Cl2(g) → AgCl(s) Given E°Cl2/Cl– = + 1.36 V, E°AgCl/Ag,Cl– = 0.22 V If PCl2 = 1 atmand T = 298 K

Which of these ions Cu+, Co3+, Fe2+ is stable in aqueous medium. Given :E°Cu2+/Cu+ = 0.15 volt ; E°Cu+/Cu = 0.53 V ;E°Co3+/Co2+ = 1.82 V ; E°Fe3+/Fe2+ = 0.77 V ;E°Fe2+Fe = –0.44 V ;E°O2,H+/H2O = 1.23 V

Select the correct statement if – E°Mg2+/Mg = –2.4V, E°Sn4+/Sn2+ = 0.1 V, E°MnO4–,H+/Mn2+ = 1.5 V, E° I2/I–= 0.5 V Here,

The temperature coefficient of a standard Cd–cell is –5.0 × 10–5 Vk–1 whose emf at 25°C is 1.018 V. During the cell operation, the temperature will –

A cell Ag | Ag+ || Cu++ | Cu initially contains 2M Ag+ and 2M Cu++ ions. The charger in cell potential after the passage of 10 amp current for 4825 sec is:

For the cell (at 298 K) Ag(s) | AgCl(s) | Cl–(aq) || AgNO3(aq) | Ag(s) Which of the following is correct –

During an electrolysis of conc. H2SO4, perdisulphuric acid (H2S2O8) and O2 from in equimolar amount. The amount of H2 that will form simultaneously will be (2H2SO4 → H2S2O8 + 2H+ + 2e–)

In producing chlorine by electrolysis 100 kW power at 125V is being consumed.How much chlorine per minute is liberated (ECE of chlorine is 0.367×10-6kgC-1)

At 298K the standard free energy of formation of H₂O(l) is –237.20kJ/mole while that of its ionisation into H+ iion and hydroxyl ions is 80 kJ/mole, then the emf of the following cell at 298 K will be

H₂(g,1 bar) | H⁺ (1M) || OH^–(1M) | O₂ (g, 1bar)

At what $\frac{[{Br}^{-}]}{\sqrt{[{CO}_{3}^{2 -}]}}$ does the following cell have its reaction at equilibrium?

Ag(s) | Ag₂CO₃(s) | Na₂CO₃ (aq) || KBr(aq) | AgBr(s) | Ag(s)

K_SP = 8 × 10^–12 for Ag₂CO₃ and K_SP = 4 × 10^–13 for AgBr

It is observed that the voltage of a galvanic cell using the reaction M(s) + xH⁺ $\to_{}^{}$ M^x+ + $\frac{x}{2}$ H₂ varies linearly with the log of the square root of the hydrogen pressure and the cube root of the M^x+ concentration. The value of x is

Consider the cell Ag(s)|AgBr(s)|Br–(aq)||AgCl(s)|Cl–(aq)|Ag(s) at 25°C. The solubility product constants of AgBr & AgCl are respectively 5 × 10^–13 & 1 × 10^–10. For what ratio of the concentrations of Br^–& Cl^–ions would the emf of the cell be zero ?

Value of ${Λ_{m}}^{\infty}$ for SrCl₂ in water at 25°C from the following data:

Conc. (mol/lt) 0.25 1

$Λ_{m}$ (Ω^–1 cm² mol^–1) 260 250

Calculate the useful work of the reaction Ag(s) + 1/2Cl₂(g) $\to_{}^{}$ AgCl(s)

Given $E °_{Cl 2 / {Cl}^{-}} = + 1.36 V, E °_{AgCl / Ag, {Cl}^{-}} = 0.22 V$

If $P_{{Cl}_{2}}$ = 1 atmand T = 298 K

Which of these ions Cu⁺, Co³⁺, Fe²⁺ is stable in aqueous medium.

Given :E°_Cu2+/Cu+ = 0.15 volt ; E°_Cu+/Cu = 0.53 V ;E°_Co3+/Co2+ = 1.82 V ;

E°_Fe3+/Fe2+ = 0.77 V ;E°_Fe2+Fe = –0.44 V ;E°_O2,H+/H2O = 1.23 V

Select the correct statement if –

E°_Mg2+/Mg = –2.4V, E°_Sn4+/Sn2+ = 0.1 V, E°_{MnO4–,H+/Mn2+} = 1.5 V, E° _I2/I–= 0.5 V

Here,

The temperature coefficient of a standard Cd–cell is –5.0 $\times$ 10^–5 Vk^–1 whose emf at 25°C is 1.018 V. During the cell operation, the temperature will –

A cell Ag | Ag⁺ || Cu⁺⁺ | Cu initially contains 2M Ag⁺ and 2M Cu⁺⁺ ions. The charger in cell potential after the passage of 10 amp current for 4825 sec is:

For the cell (at 298 K)

Ag(s) | AgCl(s) | Cl^–(aq) || AgNO₃(aq) | Ag(s)

Which of the following is correct –

During an electrolysis of conc. H₂SO₄, perdisulphuric acid (H₂S₂O₈) and O₂ from in equimolar amount. The amount of H₂ that will form simultaneously will be (2H₂SO4 → H₂S₂O₈ + 2H⁺ + 2e^–)

In producing chlorine by electrolysis 100 kW power at 125V is being consumed.How much chlorine per minute is liberated (ECE of chlorine is 0.367 $\times 10^{- 6} k g C^{- 1}$ )