The E° in the given diagram is,

(1) 0.5

(2) 0.6

(3) 0.7

(4) 0.8

Subtopic:  Relation between Emf, G, Kc & pH |
 62%
From NCERT
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Hints

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)

(1) 0.40 V

(2) 0.81 V

(3) 1.23 V

(4) –0.40 V

Subtopic:  Relation between Emf, G, Kc & pH |
From NCERT
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Hints
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NEET 2023 - Target Batch - Aryan Raj Singh

Which of the following cell can produce more electric work.

(1) pt,H2|NH4Cl||0.1MCH3COOH|H2,pt

(2) pt,H2|0.1MHCl||0.1MNaOH|H2,pt

(3) pt,H2|0.1MHCl||0.1MCH3COOK|H2,pt

(4) pt,H2|0.1MCH3COOK||0.1MHCl|H2,pt

 

Subtopic:  Relation between Emf, G, Kc & pH |
From NCERT
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Hints

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

(1) 1 × 10–7

(2) 2 × 10–7

(3) 3 × 10–7

(4) 4 × 10–7

Subtopic:  Relation between Emf, G, Kc & pH |
 73%
From NCERT
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Hints

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:

1. 2

2. 3

3. 4

4. 5

Subtopic:  Nernst Equation |
 62%
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Hints

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

(1) 0.0315 volt

(2) 0.0629 volt

(3) 0.0455 volt

(4) 0.0545 volt

Subtopic:  Nernst Equation |
 68%
From NCERT
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Hints

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& Clions would the emf of the cell be zero ?

(1) 1 : 200

(2) 1 : 100

(3) 1 : 500

(4) 200 : 1

Subtopic:  Nernst Equation |
From NCERT
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Hints

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

(1) 110 kJ/mol

(2) 220 kJ/mol

(3) 55kJ/mol

(4) 1000 kJ/mol

Subtopic:  Relation between Emf, G, Kc & pH |
 65%
From NCERT
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Hints
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NEET 2023 - Target Batch - Aryan Raj Singh

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 ;

Fe3+/Fe2+ = 0.77 V ;E°Fe2+Fe = –0.44 V ;E°O2,H+/H2O = 1.23 V

(1) Cu+, Co3+

(2) Co3+

(3) Cu+

(4) Co3+, Cu+, Fe2+

Subtopic:  Electrode & Electrode Potential |
 53%
From NCERT
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NEET 2023 - Target Batch - Aryan Raj Singh

Select the correct statement if –

Mg2+/Mg = –2.4V, E°Sn4+/Sn2+ = 0.1 V, \(E_{MnO_{4}^{-}\, ,H^{+}\,/\,Mn^{+2} }^{\circ}\) = 1.5 V, \(E_{I_{2}\,/\,I^{-}}^{\circ} \)= 0.5 V

Here,

1. MnO4– is the strongest oxidizing agent and Mg is the strongest reducing agent.
2. Sn4+ + 2I Sn2+ + I2 is a spontaneous reaction.
3. Mg2+ + Sn2+ Mg + Sn4+ is a spontaneous reaction.
4. Weakest oxidizing agent is Sn4+ and weakest reducing agent is Mn2+.
Subtopic:  Electrode & Electrode Potential |
 76%
From NCERT
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Hints
To view explanation, please take trial in the course.
NEET 2023 - Target Batch - Aryan Raj Singh