Electro chemistry practice · Mixed difficulty

An electronic conductor is

Cathode used in Leclanche cell is

${E^ \circ }$ of an electrode is :

If the standard electrode potential for a cell $A_{\left( {aq} \right)}^{2 + } + 2{B_{\left( s \right)}} \to {A_{\left( s \right)}} + 2B_{\left( {aq} \right)}^ +$ is 1.9 V, then the standard Gibbs energy for the reaction is

In a cell containing zinc electrode and standard hydrogen electrode(SHE), the zinc electrode acts as :

Which ion has exceptionally higher ${\mathrm{\Lambda }^\infty }$ values?

Statement I: $96,500 \mathrm{C}$ charge is required for the reduction of one mole of silver ions.

Statement II: The amount of electricity (or) charge required for oxidation or reduction depends on the stoichiometry of the electrode reaction.

If the $\Delta G$ of a cell reaction $\mathrm{AgCl} + {e^ - } \to \mathrm{Ag} + \mathrm{C}{\mathrm{l}^ - }$ is $- 21.20$ kJ, the standard emf of cell is

A standard hydrogen electrode has Zero electrode potential because

The equation representing kohlrausch law from the following is (${V^ + } =$ No. of cations, ${V^ - } =$ No. of anions)

The reaction occurring at anode when the electrolysis of an aqueous solution containing $\mathrm{Na}_2 \mathrm{SO}_4$ and $\mathrm{CuSO}_4$ is done using $\mathrm {Pt}$ electrode is

The unit of equivalent conductivity is

Passage of 96500 coulomb of electricity liberates ….litre of ${\mathrm{O}_2}$ at NTP during electrolysis.

The amount of substance deposited by the passage of 1 A of current for 1 s is equal to

The fraction of the total current carried by an ion is known as:

Which one of the following nitrates will leave behind A metal on strong heating?

During the electrolysis of an electrolyte, the number of ions produced, is directly proportional to the

If the ${H^ + }$ concentration is decreased from 1 M to ${10^{ - 4}}$ M at ${25^ \circ }C$  for the couple $MnO_4^ - /M{n^{(2 + )}}$, then the oxidising power of the $MnO_4^ - /M{n^{(2 + )}}$ couple decreases by

The product obtained at anode when 50% ${\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}$ aqueous solution is electrolysed using platinum electrodes is

Two platinum electrodes were immersed in a solution of cupric sulphate and electric current passed through the solution. After sometime, it was found that the colour of copper sulphate disappeared with evolution of gas at the electrode. The colourless solution contains:

Quantity of charge is measured in :

Cell constant of a conductivity cell is usually derived by using a solution of :

Hydrogen-oxygen fuel cells are used in spacecraft to supply :

Read the following statements carefully.

(i) According to a convention cell potential of hydrogen electrode (S.H.E.) is considered to be zero at all temperatures.

(ii) e.m.f. of the cell ${Pt}({s}) / {H}_2({~g}, 1 {bar}) / {H}^{+}({aq}, 1 {M})$ $\| {Zn}^{2+}({aq}, 1 {M}) / {Zn}$ is -0.76 . This negative value indicates that ${Zn}^{2+}$ ion reduces less easily then ${H}^{+}$ ions.

(iii) Copper does not dissolve in ${HCl}$ but dissolves in ${HNO}_3$ as in nitric acid it gets oxidised by nitrate ion.

(iv) Inert metals like $Pt$ or Au are used in certain electrodes i.e., these metals does not participate in reaction but provide surface for oxidation and reduction reactions.

(v) Fluorine has the highest electrode potential thereby making it strongest oxidising agent whereas lithium with lowest electrode potential is the weakest oxidising and strongest reducing agent.

Which of the following is the correct coding for the statements above.

The calomel electrode is a :

The product obtained from the electrolytic oxidation of acidified sulphate solutions, is

Hydrogen peroxide is obtained by electrolysis of

The electrolytic bath used in gold plating of copper articles contains :

Which of the following statement(s) is/an incorrect for corrosion of iron?

(i) Reaction occurring at anode is

${O}_2(g)+4 {H}^{+}(a q)+4 e^{-} \rightarrow 2 {H}_2 {O}(\ell)$

(ii) Reaction occurring at cathode is

$2 {Fe}({s}) \rightarrow 2 {Fe}^{2+}+4 e^{-}$

(iii) Rust is ${Fe}_2 {O}_3 \cdot {H}_2 {O}$

(iv) ${H}^{+}$involved in corrosion reaction is provided from ${H}_2 {CO}_3$ which is formed due to dissolution of carbon dioxide from air in to water.

Assertion (A) At the end of electrolysis using platinum electrodes, an aqueous solution of $\mathrm{CuSO}_4$ turns colourless.

Reason (R) During the electrolysis $\mathrm{CuSO}_4$ changes to $\mathrm{Cu}(\mathrm{OH})_2$ during electrolysis.