Chemistry Electrochemistry

Time required for complete decomposition of 4 mol of water using a current of 4 ampere is y * 10⁵ seconds. Value of y is ? (Use F = 96500 Cmol^-1)

In a cell, the following reactions take place

Fe²⁺ ® Fe³⁺                           $E_{F{e}^{3+}/F{e}^{2+}}^0=0.77V$  

2I^- ® I₂ + 2e^-                       $E_{I_2/I^{-}}^0=0.54V$  

The standard electrode potential for the spontaneous reaction in the cell is x * 10^-2 V 298 K. The value of x is________(Nearest Integer)

For the cell Cu(s) | Cu²⁺ (aq)(0.1M) Ag⁺ (aq)(0.01M) | Ag(s)
The cell potential E₁ = 0.3095V
For the cell Cu(s) | Cu²⁺ (aq)(0.01M) Ag⁺ (aq)(0.001M) | Ag(s)
The cell potential = _____ *10⁻² V. (Round off to the Nearest Integer).
[Use : (2.303RT/F) = 0.059 ]

Cu(s) + Sn2+(0.001M) Cu2+ (0.01M) + Sn(s)

The Gibbs free energy change for the above reaction at 298 K is x * 101 KJmol1. The value of x is __________. (nearest integer)

[Given : ${}_{{}^{}}^{}$ 0.34V; ${}_{{}^{}}^{}$ = 0.14V; F = 96500 Cmol1]

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R:
Assertion A: In equation ΔG = -nFEcell, value of ΔG depends on n.
Reason R: Ecell is an intensive property and ΔG is an extensive property.

In the light of the above statements, choose the correct answer from the options given below:

The conductivity of centimolar solution of KCl at 25°C is 0.0210 ohm^-1 cm^-1 and the resistance of the cell containing the solution at 25°C is 60 ohm. The value of cell constant is:

The product formed in the following chemical reaction is:

Match List-I with List-II.
List-I
(a) PCl₅
(b) SF₆
(c) BrF₅
(d) BF₃
List-II
(i) Square pyramidal
(ii) Trigonal planar
(iii) Octahedral
(iv) Trigonal bipyramidal
Choose the correct answer from the options given below.

Choose the correct option for graphical representation of Boyle's law, which shows a graph of pressure vs. volume of a gas at different temperatures :

Find the emf of the cell in which the following reaction takes place at 298 K
Ni(s) + 2Ag⁺(0.001M) → Ni²⁺(0.001M) + 2Ag(s)
(Given that E°cell = 1.05 V, 2.303RT/F = 0.059 at 298 K)