Retro (Past 13 Year) JEE Main (Electrochemistry) - JEE MCQ

Given below are the half-cell reactions 

(JEE Main 2014)

Based on the data given above, strongest oxidising agent will be

(AIEEE 2013)

The standard reduction potentials for Zn²⁺ / Zn, Ni²⁺ /Ni and Fe²⁺ / Fe are - 0.76, - 0.23 and - 0.44 V, respectively. The reaction X + y²⁺→ X²⁺ + Y will be spontaneous when

(AIEEE 2012)

The reduction potential of hydrogen half-cell will be negative if 

Resistance of 0.2 M solution of an electrolyte is 50 Ω The specific conductance of the solution is 1.3 Sm^-1. If resistance of the 0.4 M solution of the same electrolyte is 260 Ω, its molar conductivity is

(AIEEE 2011)

The Gibbs energy for the decomposition of Al₂O₃ at 500°C is as follows

The potential difference needed for electrolytic reduction of Al₂O₃ at 500°C is at least 

(AIEEE 2010)

The value of standard electrode potenital for the charge,

(AIEEE 2009)

The potential for the cell

Cr | Cr3⁺ (0.1 M) || Fe²⁺ (0.01 M) | Fe is

(AIEEE 2008)

The equivalent conductances of two strong electrolytes at infinite dilution in H₂O (where ions move freely through a solution) at 25°C a re given below

What additional information /quantity one needs to calculateof an aqueous solution of acetic acid?

The cell, Zn | Zn²⁺ (1 M) || Cu²⁺ (1 M) | Cu

(E°_cell = 1.10 V), was allowed to be completely discharged at 298 K. The relative concentration 

(AIEEE 2007)

Resistance of a conductivity cell filled with a solution of an electrolyte of concentration 0.1 M is 100 Ω. The conductivity of this solution is 1.29 Sm^-1. Resistance of the same cell when filled with 0.2 M of the same solution is 520 Ω. The molar conductivity of 0.2 M solution of the electrolyte will be

The molar conductivities and at infinite dilution in water at 25°C are 91.0 and 426.2S cm²/mol, respectively. To calculate a additional value required is

(AIEEE 2006)

Given the data at 25°C,

What is the value of log K_sp for Agl?

(AIEEE 2006)

Calculate using appropriate molar conductances of the electrolytes listed above at infinite dilution in H₂O at 25°C

(AIEEE 2005)

Aluminium oxide may be electrolysed at 1000°C to furnish aluminium metal (atomic mass = 27 u; 1 Faraday = 96500 C). The cathode reaction is

To prepare 5.12 kg of aluminium metal by this method would require

(AIEEE 2005)

The limiting molar conductivities for NaCI, KBr and KCI are 126, 152 and 150S cm² mol^-1, respectively . The for NaBr is

(AIEEE 2004)

The E°_{m³⁺/m²⁺} values for Cr, Mn, Fe and Co are

- 0.41, + 1.57, + 0.77 and + 1.97 V,

respectively . For which one of these metals, the change in oxidation state from + 2 to + 3 is easiest?

(AIEEE 2004)

Consider the following E^o values :

Under standard conditions, the potential for the reaction,

(AIEEE 2004)

In a cell that utilises the reaction,
Zn (s)+ 2H + (aq) → Zn²⁺ (aq),+ H₂(g)

addition of H₂SO₄ to cathode compartment will

(AIEEE 2004)

The standard emf of a cell, involving one electron change is found to be 0.591 V at 25° C. The equilibrium constant of the reaction is (F= 96500 C mol^-1)

(AIEEE2004)

When during electrolysis of a solution of AgNO₃, 9650 C of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be

(AIEEE 2003)

Standard reduction electrode potentials of three metals A, B and C are + 0.5 V, - 3.0 V and - 1.2 V, respectively. The reducing power of these metals are

(AIEEE 2003)

For a cell reaction involving a two electron change, the standard emf of the cell is found to be 0.295 V at 25°C. The equilibrium constant of the reaction at 25°C will be

(AIEEE 2003)

Conductivity (Seimen’s S) is directly proportional to area of the vessel and the concentration of the solution in it and is inversely proportional to the length of the vessel, then constant of proportionality is expressed in

(AIEEE 2002)

(AIEEE 2002)

For the following cell with hydrogen electrodes at two different pressures p₁ and p₂

emf is given by 

(AIEEE 2002)