Electrochemistr...

Which cell will measure the standard electrode potential of zinc electrode?

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

 emf is given by

For the cell,

Thus (x/y) is

A solution of Fe²⁺  is titrated potentiometrically using Ce⁴⁺ solution.

Fe²⁺ → Fe³⁺ + e^- , E⁰ = -0.77 V

emf of the Pt | Fe²⁺ , Fe³⁺ pair at 50% and 90% titration of Fe²⁺ are   

Two half-cells are given

Ag | AgCl | KCl (0.2 M), Ag | AgBr | KBr (0.001 M),

K_sp(AgCl) = 2.8 x 10^-10, K_sp (AgBr) = 3.3 x 10 ^-13

For a spontaneous cell reaction, cell set up is    

In the following cell at 298 K,two weak acids (HA) and (HB) with pK_a (HA) = 3 and pK_a (HB) = 5 of equal molarity have been used as shown.

Thus, emf of the cell is   

A concentration cell reversible to anion (Cl^-) is set up

cell reaction is spontaneous ,if 

Which has the maximum potential at 298 K (numerical value) for the half-cell reaction?

2H⁺ + 2e^-  → H₂ (1 bar)   

For the cell,  and for the cell Pt(H₂) | H⁺ (1M)| Ag,  

Thus E_cell for the

Ag|Ag⁺ (0.1M) || Zn²⁺ (0.1M) | Zn is  ....................and cell reaction is...............

Consider the following cell reaction,

2Fe(s) + O₂(g) + 4H⁺ (aq) →2Fe²⁺ (aq) + 2H₂O(l) , E^°= 1.67 V

At [Fe²⁺] = 1 x 10^-3 M.  and pH = 3,the cell potential at 298 K is 

For the following cell with gas electrodes at p₁ and p₂ as shown:

Cell reaction is spontaneous , if  

For the half-cell, Cl^-|Hg₂Cl₂, Hg(l), E = 0.280V at 298K electrode potential has maximum value when KCl used is 

Given at 298 K standard oxidation potential of quinhydrone electrode = -0.699 V Standard oxidation potential of calomel electrode = -0.268 V

Thus, emf of the cell at 298 K is 

E^°_red (standard reduction electrode potentials) of different half-cell are given

In which cell , is ΔG^° most negative?

Given the following half-cell reactions and corresponding reduction potentials: 

Which combination of two half-cell would result in a cell with largest (E^°_cell > 0)?   

For

Then E^° for the reaction    

Following half-cell, Pt (H₂)|H₂O behaves as SHE at a pressure of

Electrode potential of the following half-cell is dependent on
Hg, HgO |OH^-(aq)

The aqueous solution of which of the following compounds is the best conductor of electric current?

An increase in the conductivity equivalent of a solid electrolyte with dilution is primarily due to

The equivalent conductance of Ba²⁺ and Cl^– are respectively 127 and 76 ohm^-1 cm^-1 eq^-1 at infinite dilution. The equivalent conductance of BaCl₂ at infinite dilution will be

When heating one end of a metal plate, the other end gets hot because of

Comprehension Type

This section contains a passage describing theory, experiments, data, etc. Two questions related to the paragraph have been given. Each question has only one correct answer out of the given 4 options (a), (b), (c) and (d)

Passage I

1.05 g of lead ore containing impurity of Ag was dissolved in HNO₃ and the volume was made 350 mL. A silver electrode was dipped in the solution and E_cell of Pt(H₂) | H⁺ (1M)|| Ag⁺| Ag was 0.500 V at 298 K. E°_Ag⁺/Ag = 0.80 V

Q.

Pure [Ag⁺] in the ore is    

Passage I

1.05 g of lead ore containing impurity of Ag was dissolved in HNO₃ and the volume was made 350 mL. A silver electrode was dipped in the solution and E_cell of Pt(H₂) | H⁺ (1M)|| Ag⁺| Ag was 0.500 V at 298 K. E°_Ag⁺/Ag = 0.80 V

Q.

Percentage of silver in the sample is      

Passage II

For the following,

Q.

pH of the solution in the half-cell containing 0.02 HA is(HA is a weak monobasic acid)   

Passage II

For the following,

Q.

pK_a of the weak monobasic acid is  

The weight of silver displaced by a quantity of electricity which displaces 5600ml of O₂ at STP will be

Once a current of 1.0 ampere was passed through one litre of CuCl₂ solution for 16 min and 5 sec, all of the solution’s copper was deposited at the cathode. The strength of solution CuCl₂ was (Molar mass of Cu = 63.5; Faraday constant = 96,500 C/mol)                                                                      

On electrolysis of dilute sulphuric acid using platinum electrodes, the product obtained at the anode will be