Electro chemistry practice · Mixed difficulty

In the electrochemical reaction,

$2\mathrm{F}{\mathrm{e}^{3 + }} + \mathrm{Zn} \to \mathrm{Z}{\mathrm{n}^{2 + }} + 2\mathrm{F}{\mathrm{e}^{2 + }}$

increasing the concentration of $\mathrm{F}{\mathrm{e}^{2 + }}$

Electrolytic conduction is due to migration of :

The number of correct statements from the
following is ________

(A) Conductivity always decreases with decrease
in concentration for both strong and weak
electrolytes.

(B) The number of ions per unit volume that carry
current in a solution increases on dilution.

(C) Molar conductivity increases with decrease in
concentration.

(D) The variation in molar conductivity is different
for strong and weak electrolytes.

(E) For weak electrolytes, the change in molar
conductivity with dilution is due to decrease in
degree of dissociation.

The E0 values at ${25^0}C$ for ${A^ + }/A,\mathrm{ }{B^{2 + }}/B,\mathrm{ }{D^{3 + }}/D$ and ${E^ + }/E$ are -2.15, -1.75, +0. 15 and +0.21 volt respectively. Which of the following is the strongest oxidising agent ?

Which of the following is/are correct statement(s) for the addition of ${Li}, {K}, {Rb}$ to the aqueous solution of ${Na}^{+}$.

(i) The correct order of metals in which they reduce the ${Na}^{+}$ion is ${Rb} < {K} < {Li}$.

(ii) Reduction of metal ions would not take place.

What flows in the internal circuit of A galvanic cell?

The standard reduction potential&nbsp;${E^ \circ }$ for the half reactions are as
$\mathrm{Zn} \to \mathrm{Z}{\mathrm{n}^{2 + }} + 2{e^ - },{E^ \circ } = 0.76V$
$\mathrm{Cu} \to \mathrm{C}{\mathrm{u}^{2 + }} + 2{e^ - },{E^ \circ } = 0.34V$
The emf for the cell reaction,
$\mathrm{Zn} + \mathrm{C}{\mathrm{u}^{2 + }} \to \mathrm{Z}{\mathrm{n}^{2 + }} + \mathrm{Cu}$

Faraday’s laws hold good at :

When Zn piece is kept in $\mathrm{CuS}{\mathrm{O}_4}$ solution, copper gets precipitated because:

Molar conductivities (${\mathop \mathrm{\Lambda }\limits^ \circ _m}$) at infinite dilution of $\mathrm{NaCl},\mathrm{HCl}$ and $\mathrm{C}{\mathrm{H}_3}\mathrm{COONa}$ are 126.4, 425.9 and 91.0 ${\rm{S {\kern 1pt} {\kern 1pt}c}}{\mathrm{m}^2}{\kern 1pt} \mathrm{mo}{\mathrm{l}^{ - 1}}$ respectively.${\mathop \mathrm{\Lambda }\limits^ \circ _m}$ for $\mathrm{C}{\mathrm{H}_3}\mathrm{COOH}$ will be :

During electrolysis of fused $\mathrm{Ca}{\mathrm{H}_2},{\mathrm{H}_2}$ is liberated at :

Which colourless gas evolves when $\mathrm{N}{\mathrm{H}_4}\mathrm{Cl}$ reacts with zinc in A dry cell battery?

Statement I: When iron rod is immersed in $\mathrm{NaCl}$ solution such that half of its length is corroded and other half part when exposed to air is not corroded.

Statement II: Metal portion with less access to $\mathrm{O}_2$ corrodes.

The equilibrium constant for the reaction at 298 K is

Select the correct statement for $\Lambda_{\mathrm{m}}=\Lambda_{\mathrm{m}}^{\circ}-A C^{1 / 2}$.

Statement I: During electrolysis of aqueous
sodium acetate solution, the molar ratio of gases
formed at cathode and anode is 1:3.

Statement II: Acetate ion discharges at anode and
$\text{H}^+$ ion, at cathode.

A current of 12 A is passed through an electrolytic cell containing aqueous $\mathrm{NiS}{\mathrm{O}_4}$ solution. Both Ni and ${\mathrm{H}_2}$ gas are formed at the cathode. The current efficiency is 60%. What is the mass of nickel deposited on the cathode per hour?

$100 {~mL}$ of $0.05 {MCuSO}_4($ aq) solution was electrolyzed using inert electrodes by passing current till the ${pH}$ of the resulting solution was 2 . The solution after electrolysis was neutralized and then treated with excess ${KI}$ and formed ${I}_2$ titrated with $0.04 M {Na}_2{~S}_2 {O}_3$. Calculate the required volume (in ${mL}$ ) of ${Na}_2 {~S}_2 {O}_3$ :

The equilibrium constant for the reaction,&nbsp;$Cu(s) + 2A{g^ + }(aq) \rightleftharpoons C{u^{(2 + )}}(aq) + 2Ag(s),$ ${E^ \circ } = 0.46\text{ V}$ at 298 K is:

The hydrogen electrode is dipped in a solution of $\mathrm{pH} = 3{\kern 1pt} {\kern 1pt} {\kern 1pt} \mathrm{at}{\kern 1pt} {\kern 1pt} {\kern 1pt} {25^ \circ }C$. The potential of the cell would be ($\mathrm{the value of}\frac{{2.303RT}}{T}\mathrm{is}{\kern 1pt} {\kern 1pt} {\kern 1pt} 0.059\mathrm{V}$)

$E^\circ$ values of some redox couples are given below on the basis of these values. Choose the correct option
$E^\circ$ values:
$\begin{array}{l} B{r_2}\mathrm{/}B{r^ - } = + 1.90\\ A{g^ + }\mathrm{/}Ag(s) = + 0.80\\ C{u^{2 + }}\mathrm{/}Cu(s) = + 0.34\\ {I_2}(s)\mathrm{/}{I^ - } = + 0.54 \end{array}$

Which one of the following statements is correct for electrolysis of brine solution?

A student made the following observations in the laboratory,
i) Clean copper metal did not react with 1 molar $\mathrm{Pb}{\left( {\mathrm{N}{\mathrm{O}_3}} \right)_2}$ solution.
ii) Clean lead metal dissolved in a 1 molar $\mathrm{AgN}{\mathrm{O}_3}$ solution and crystals of $\mathrm{Ag}$ metal appeared.
iii) Clean silver metal did not react with 1 molar $\mathrm{Cu}{\left( {\mathrm{N}{\mathrm{O}_3}} \right)_2}$ solution.
The order of decreasing reducing character of the three metals is :

In which cell, electrical energy is converted into chemical energy?

On passing 0.5 F electricity through molten sodium chloride, sodium deposited at cathode will be

1.8 g of metal were deposited by a current of 3 amperes for 50 minute. The equivalent wt. of metal is :

$\mathrm{Cu} + 2\mathrm{HCl} \to \mathrm{CuC}{\mathrm{l}_2} + {\mathrm{H}_2}\left( \mathrm{g} \right)$

$\left[ {E_{C{u^{2 + }}/Cu}^ \circ = + 0.34V} \right]$

$\mathrm{Zn} + 2\mathrm{HCl} \to \mathrm{ZnC}{\mathrm{l}_2} + {\mathrm{H}_2}\left( \mathrm{g} \right)$

$\left[ {E_{Z{n^{2 + }}/Zn}^ \circ = - 0.76V} \right]$

$\mathrm{Ag} + 2\mathrm{HCl} \to \mathrm{AgCl} + \frac{1}{2}{\mathrm{H}_2}\left( \mathrm{g} \right)$

$\left[ {E_{A{g^ + }/Ag}^ \circ = + 0.80V} \right]$

Which of the following reaction is feasible ?

What will be pH of aqueous solution of electrolyte in electrolytic cell during electrolysis of $\mathrm{CuS}{\mathrm{O}_4}\left( {aq} \right)$ between graphite electrodes?

Which one of the following solutions will have highest conductivity?

Which one is correct relation :