AIPMT Prelims Chemistry Electrochemistry Class 12 Questions

Limiting molar conductivity of NH₄OH (i.e., Λₘ(NH₄OH)) is equal to:

The electrode potentials for Cu²⁺(aq) + e⁻ → Cu⁺(aq) and Cu⁺(aq) + e⁻ → Cu(s) are +0.15 V and +0.50 V respectively. The value of E° for Cu²⁺/Cu will be

Standard electrode potential for Sn⁴⁺/Sn²⁺ couple is +0.15 V and that for the Cr³⁺/Cr couple is −0.74 V. These two couples in their standard state are connected to make a cell. The cell potential will be

If the E°cell for a given reaction has a negative value, then which of the following gives the correct relationships for the values of ΔG° and Keq?

Standard electrode potential of three metals X, Y and Z are –1.2 V, +0.5 V and –3.0 V respectively. The reducing power of these metals will be

An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to

For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46 V at 25°C. The value of standard Gibbs energy, ΔG⁰ will be (F = 96500 C mol⁻¹)

Given:

(i) Cu²⁺ + 2e⁻ ⟶ Cu, E° = 0.337 V

(ii) Cu⁺ + e⁻ ⟶ Cu, E° = 0.153 V

Electrode potential, E° for the reaction, Cu⁺ + e⁻ ⟶ Cu, will be:

Al₂O₃ is reduced by electrolysis at low potentials and high currents. If 4.0 × 10⁴ amperes of current is passed through molten Al₂O₃ for 6 hours, what mass of aluminium is produced? (Assume 100% current efficiency. At. mass of Al = 27 g mol⁻¹)

The equivalent conductance of M/32 solution of a weak monobasic acid is 8.0 mhos cm² and at infinite dilution is 400 mhos cm². The dissociation constant of this acid is:

On the basis of the following E° values, the strongest oxidizing agent is : [Fe(CN)₆]³⁻ → [Fe(CN)₆]⁴⁻ + e⁻, E° = -0.35 V Fe³⁺ → Fe²⁺ + e⁻, E° = -0.77 V

Kohlrausch's Law states that at :

Standard free energies of formation (in kJ/mol) at 298 K ar$e^{-237}$.2, -394.4 an$d^{-8}$.2 for H₂O(l), CO₂(g) and pentane(g) respectively The value of E°cell for the pentane-oxygen fuel cell is:

A steady current of 1.5 amp flows through a copper voltameter for 10 minutes. If the electrochemical equivalent of copper is 30 × 10⁻⁵ g coulomb⁻¹, the mass of copper deposited on the electrode will be

The efficiency of a fuel cell is given by

The equilibrium constant of the reaction: Cu(s) + 2Ag⁺(aq) ⟶ Cu²⁺(aq) + 2Ag(s) ; E° = 0.46 V at 298 K is

If E°Fe²⁺/Fe = -0.441 V and E°Fe³⁺/Fe²⁺ = 0.771 V, the standard emf of the reaction: Fe + 2Fe³⁺ → 3Fe²⁺ will be:

A hypothetical electrochemical cell is shown below AlA₊ (xM)∥ B₊ (yM)∥ B The emf measured is +0.20V. The cell reaction is:

4.5g of aluminium (at. mass 27 amu) is deposited at cathode from Al³⁺ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H⁺ ions in solution by the same quantity of electric charge will be:

A battery is charged at a potential of 15V for 8 hours when the current flowing is 10A. The battery on discharge supplies a current of 5A for 15 hours. The mean terminal voltage during discharges is 14 V. The "Watt hour" efficiency of the battery is :-

The standard e.m.f. of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25°C. The equilibrium constant of the reaction would be :- (Given F = 96500 C mol⁻¹; R = 8.314 JK⁻¹ mol⁻¹)

On the basis of the information available from the reaction: $\frac{4}{3} \text{Al} + \text{O}_2 \rightarrow \frac{2}{3} \text{Al}_2\text{O}_3, \Delta G = -827 \text{kJ mol}^{-1}$ of $\text{O}_2$, the minimum e.m.f. required to carry out electrolysis of $\text{Al}_2\text{O}_3$ is $(F = 96500 \text{ C mol}^{-1})$

The e.m.f. of a Daniell cell at 298 K is E₁. Zn/SO₄(0.01 M) || CuSO₄(1.0 M)/Cu When the concentration of ZnSO₄ is 1.0 M and that of CuSO₄ is 0.01 M, the e.m.f. is changed to E₂. What is the relationship between E₁ and E₂:

In electrolysis of NaCl when Pt electrode is taken then H₂ is liberated at cathode while with Hg cathode it forms sodium amalgam :-

In the silver plating of copper, K[Ag(CN)₂] is used instead of AgNO₃. The reason is :-

Stand electrode potential are Fe²⁺/Fe E° = – 0.44 Fe³⁺/Fe²⁺ E° = 0.77 If Fe²⁺, Fe³⁺ and Fe block be kept together, then :-

Which of the following will exhibit maximum ionic conductivity :

The most convenient method to protect the bottom of ship made of iron is :

According to the Faraday Law of electrolysis, the mass deposited at electrode proportional to:

For the disproportionation of copper : 2 Cu⁺ → Cu²⁺ + Cu, E° is : - (Given E° for Cu²⁺/Cu is 0.34 V & E° for Cu²⁺/Cu⁺ is 0.15 V :

Cell reaction is spontaneous when :

At infinite dilution equivalent conductances of Ba²⁺ & Cl⁻ ions are 127 & 76ohm⁻¹cm² eq⁻¹ respectively. Equivalent conductance of BaCl₂ at infinite dilutions is :