When NaCl solution is electrolysed using Pt electrodes then pH of solution

By how much will the potential of half cell Cu²⁺|Cu change if the solution is diluted to 100 times at 298 K . It will  :

What will be the molar conductance at infinite dilution for NH₄OH. If at infinite dilution the molar conductances of Ba(OH)₂, BaCl₂ and NH₄Cl are 523.28, 280.0 and 129.8 ohm^-1 cm^-1 mol^-1 respectively.

At 25$°$C the specific conductance of sturated solution of AgCl is 2.3 X 10-6 ohm^-1cm^-1. What will be the solubility of AgCl at 25$°$C if ionic conductances of ${\mathrm{Ag}}^{\oplus }$ and ${\mathrm{Cl}}^{⊝}$ at infinite dilution are 61.9 and 76.3 ohm^-1cm²mol^-1 respectively.

$2{\stackrel{\oplus }{\mathrm{Ag}}}_{\left(\mathrm{aq}\right)} + {\mathrm{Cu}}_{\left(\mathrm{s}\right)} \stackrel{ }{\rightleftharpoons } {{\mathrm{Cu}}_{\left(\mathrm{aq}\right)}}^{+2} + 2{\mathrm{Ag}}_{\left(\mathrm{s}\right)}$

The cell potential for this reaction is 0.46V. Which of the following change will increase the potential the most ?

Standard free energies of formation (in kJ/mol) at 298 K are -237.2, -394.4 and -8.2 for H₂O(l), CO₂(g) and pentane (g), respectively. The value of E°_cell for the pentane-oxygen fuel cell is

The equilibrium constant of the reaction:

 Cu (s) + 2Ag⁺ (aq) $\to$Cu²⁺ (aq) + 2Ag(s) ;

E$°$ = 0.46 V at 298 K is:

Rusting of iron is envisaged as setting up of an electrochemical cell because: 

What will be the value of $∆\mathrm{G}°$ for the rection ${\mathrm{Cu}}^{+2} + \mathrm{Fe} \stackrel{ }{\rightleftharpoons } {\mathrm{Fe}}^{+2} + \mathrm{Cu} ,$

if ${\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Cu}}^{+2}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Cu}$}\right.}^{\circ } = +0.34 \mathrm{V} \mathrm{and} {\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Fe}}^{+2}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Fe}$}\right.}^{\circ } = -0.44 \mathrm{V}$$$

At 298 K the Emf of following cell is :-

Pt|H_2(1atm)|${\mathrm{H}}^{\oplus }$_(0.02M)||${\mathrm{H}}^{\oplus }$_(0.01M)|H_2(1atm)|Pt

At 25$°$C temperature Zn electrode is placed in 0.1M solution of zinc salt then what will be the reduction potential ? If it is assumed that salt dissociates 25% at this dilution (${\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Zn}}^{2+}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Zn}$}\right.}^{°} = -0.76 \mathrm{V}$)

The reduction potential of Hydrogen electrode is -118mV then the concentration of ${\mathrm{H}}^{\oplus }$ion in solution will be :-

The maximum work which can be obtained from a Daniel cell -

${\mathrm{Zn}}_{\left(\mathrm{s}\right)} | {{\mathrm{Zn}}^{+2}}_{\left(\mathrm{aq}\right)} || {{\mathrm{Cu}}^{+2}}_{\left(\mathrm{aq}\right)} | {\mathrm{Cu}}_{\left(\mathrm{s}\right)}$

if : ${\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Zn}}^{+2}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Zn}$}\right.}^{\circ } = -0.76 \mathrm{V} \mathrm{and} {\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Cu}}^{+2}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Cu}$}\right.}^{\circ } = 0.34 \mathrm{V}$

CuSO₄ solution is treated separately with KCl and KI. In which case, Cu⁺² will be reduced to ${\mathrm{Cu}}^{\oplus }$ ?

How many coulombs are required to oxidise 1 mol H₂O₂ to O₂ ?

The quantity of electricity required to reduce 12.3g of nitrobenzene to aniline with 50% current efficiency is :-

Electrolysis of hot aqueous solution of NaCl gives NaClO₄ as-

$\mathrm{NaCl} +\hspace{0.17em}4{\mathrm{H}}_2\mathrm{O} \stackrel{ }{\to }{\mathrm{NaClO}}_4 + 4{\mathrm{H}}_2$

How many faraday are required to obtain 1000 g of sodium perchlorate ?

The cell reaction of micro electrochemical cell formed during rusting of iron is:-

Which of the following is an incorrect statement :- 

For the cell reaction

${\mathrm{Cu}}_{{\mathrm{c}}_1}^{+2} \left(\mathrm{aq}\right) +\hspace{0.17em}\mathrm{Zn}\left(\mathrm{s}\right) \stackrel{ }{\to } {\mathrm{Zn}}_{{\mathrm{C}}_2}^{+2} \left(\mathrm{aq}\right) + \mathrm{Cu}\left(\mathrm{s}\right)$

the change in free energy at a given temperature is a function of 

EMF of the following cell will be zero if

Pt(H₂)|H⁺||H⁺|(H₂)Pt

    P1   C1  C₂    P₂

During electrolysis of conc. H₂SO₄, perdisulphuric acid (H₂S₂O₈), and O₂ form in equimolar amount. The amount of H₂ that will form simultaneously will be : 

${\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Ni}}^{+2}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Ni}$}\right.}^0 = -0.25 \mathrm{V}, {\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Au}}^{+3}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Au}$}\right.}^0 = 1.50 \mathrm{V}$

the emf of Voltaic cell

$\mathrm{Ni} | {\mathrm{Ni}}^{+2}(1\mathrm{M}) || {\mathrm{Au}}^{+3}(1\mathrm{M}) \mathrm{Au} \mathrm{is}:-$

The same amount of electric current is apassed through aqueous solution of MgSO₄ and AlCl₃. If 2.8 g Mg metal is deposited at amount of Al metal deposited in second cell will be

The potential of the following concentration cell at room temperature is-

$\mathrm{Pt}, {\mathrm{H}}_2\left(\mathrm{g}\right) \left|{\mathrm{H}}^{\oplus }\right({10}^{-6}\mathrm{M}\left)\right|\left|{\mathrm{H}}^{\oplus }\right({10}^{-4} \mathrm{M}) | {\mathrm{H}}_2\left(\mathrm{g}\right), \mathrm{Pt}$

Select the incorrect statement for dry cell

What is the current efficiency of an electrode deposition of Cu metal from CuSO₄ solution in which 9.8 gm copper is deposited by the passage of 5 amperes current for 2 hours?

During electrolysis, 2A current is passed through an electrolytic solution for 965 s. The number of moles of electrons passed will be

The electrochemical cell:

Zn || ZnSO₄ (0.01 M)lCuSO₄(1.0M) Cu, the emf of this Daniel cell is E₁ When the concentration ZnSO₄ is changed to 1.0 M and that of CuSO₄ changed to 0.01 M, the emf changes to E₂. The relationship between E₁ and E₂ is : 
( Given, $\frac{RT}{F}$=0.059)

The molar conductivity of a 0.5 mol/dm³ solution of AgNO₃ with electrolytic conductivity of 5.76x10^-3 S cm^-1 at 298 K is