Electrochemistry

At 298 K, the equilibrium constant is 2 * 10¹⁵ for the reaction:

Cu(s) + 2Ag⁺(aq)   $\rightleftharpoons$ Cu²⁺(aq) + 2Ag(s)

The equilibrium constant for the reaction

$\frac{1}{2}C{u}^{2+}\left(ag\right)$ + Ag(s)    + Ag⁺ (aq)

is x * 10^-8. The value of x is _____________. (Nearest Integer)

20mL of 0.02 M hypo solution is used for the titration of 10mL of copper sulphate solution, in the presence of excess of KI using starch as an indicator. The molarity of Cu²⁺ is found to be__________* 10^-2 M. [nearest integer]

Given: 2Cu²⁺ + 4I^- ® Cu₂I₂ + I₂

 I₂ +   $2S_2{O}_3^{2-}\to 2I^{-}+S_4{O}_6^{2-}$

Identify the incorrect statement from the options below for the above cell:

The quantity of electricity in Faraday needed to reduce 1 mol of $C{r}_2{O}_7^{2-}$  to Cr³⁺ is________.

The solubility product of a sparingly soluble salt A₂X₃ is 1.1 * 10^-23. If specific conductance of the solution is 3 * 10^-1, the limiting molar conductivity of the solution is x * 10^-3 S m² mol^-1. The value of x is_________.

Resistance of a conductivity cell (cell constant 129 m1) filled with 74.5 ppm solution of KCl is $100\Omega$ (labeled as solution 1). When the same cell is filled with KCl solution of 149 ppm, the resistance is $50\Omega$ (labeled as solution 2). The ratio of molar conductivity of solution 1 and solution 2 is i.e. $\frac{{\wedge }_1}{{\wedge }_2}=x*10^{-3}.$ The value of x is________. (Nearest integer)

$250\mathrm{m}\mathrm{L}$ of a waste solution obtained from the workshop of a goldsmith contains $0.1\mathrm{M}$ ${\mathrm{A}\mathrm{g}\mathrm{N}\mathrm{O}}_3$ and $0.1\mathrm{M}\mathrm{A}\mathrm{u}\mathrm{C}\mathrm{l}$ . The solution was electrolyzed at $2\mathrm{V}$ by passing a current of $1\mathrm{A}$ for 15 minutes. The metal/metals electrodeposited will be : $\left({\mathrm{E}}_{{\mathrm{A}\mathrm{g}}^{+}/\mathrm{A}\mathrm{g}}^{\mathrm{o}}=0.8\mathrm{V},{\mathrm{E}}_{{\mathrm{A}\mathrm{u}}^{+}/\mathrm{A}\mathrm{u}}^{\mathrm{o}}=1.69\mathrm{V}\right)$

$250\mathrm{m}\mathrm{L}$ of a waste solution obtained from the workshop of a goldsmith contains $0.1\mathrm{M}$ ${\mathrm{A}\mathrm{g}\mathrm{N}\mathrm{O}}_3$ and $0.1\mathrm{M}\mathrm{A}\mathrm{u}\mathrm{C}\mathrm{l}$ . The solution was electrolyzed at $2\mathrm{V}$ by passing a current of $1\mathrm{A}$ for 15 minutes. The metal/metals electrodeposited will be : $\left({\mathrm{E}}_{{\mathrm{A}\mathrm{g}}^{+}/\mathrm{A}\mathrm{g}}^{\mathrm{o}}=0.8\mathrm{V},{\mathrm{E}}_{{\mathrm{A}\mathrm{u}}^{+}/\mathrm{A}\mathrm{u}}^{\mathrm{o}}=1.69\mathrm{V}\right)$

For the reaction taking place in the cell:

$Pt\left(s\right)\left|H_2\left(g)\right)\right|H^{+}\left(aq\right)|\left|A{g}^{+}\left(aq\right)\right|Ag\left(s\right)$            

$E_{cell}^0=+0.5332V.$            

The value of ${\Delta }_f{G}^{\Theta }$  is________________kJ mol^-1 (in nearest integer)

How are NCERT Exemplar questions different from regular NCERT textbook questions in Electrochemistry?