Electro chemistry practice · Mixed difficulty

Galvanic cell is A device in which

In electrolysis of aqueous copper sulphate, the gas at anode and cathode are

A solution of $\mathrm{CuS}{\mathrm{O}_4}$ is electrolysed for 10 min with a current of 1.5 amperes. What is the mass of copper deposited at the cathode?

The equilibrium constant for the reaction given below at 298 K is :

$\mathrm{Zn}\left( s \right) + \mathrm{F}{\mathrm{e}^{2 + }}\left( {aq} \right) \to \mathrm{Z}{\mathrm{n}^{2 + }}\left( {aq} \right) + \mathrm{Fe}\left( s \right)$ ;

$E_{cell}^ \circ$ = 2905 V at 298 K

How many coloumbs of electricity are required for the oxidation of 1 mole of ${H_2}O$ to ${O_2}$

The oxidation potential of Mg and Al are + 2.37 and + 1.66 volt respectively. The Mg in chemical reactions :

How much time is required to decompose 18 g water electrolytically into ${H_2}$ and ${O_2}$ by passing 3A current?

Assuming that copper contains only iron, silver and gold as impurities. After passage of $12.4 \mathrm{~A}$ for $4825 \mathrm{~s},$ the mass of anode decreased by $20.00 \mathrm{~g}$ and the cathode increased by $19.05 \mathrm{~g}.$ The percentages of iron and copper in the original sample are, respectively, $(\mathrm{Cu}=63.5, \mathrm{Fe}=56)$

The quantity of charge required to obtain one mole of aluminium from $A{l_2}{O_3}$ is

Which of the following statements is wrong ?

The standard potential at ${25^ \circ }C$ for the following half-reactions are given against them $\mathrm{Z}{\mathrm{n}^{2 + }} + 2{e^ - } \to \mathrm{Zn},{E^ \circ } = - 0.762\mathrm{V}$

$\mathrm{M}{\mathrm{g}^{2 + }} + 2{e^ - } \to \mathrm{Mg},{E^ \circ } = - 2.37\mathrm{V}$

When zinc dust is added to the solution of $\mathrm{MgC}{\mathrm{l}_2}$,

The same current is passed through acidulated water and stannous chloride solution. What volume of dry detonating gas at $0^{\circ} \mathrm{C}$ and $1 \mathrm{~atm}$ is evolved from water, when $1.20 \mathrm{~g}$ of tin is deposited from the other solution? $(\mathrm{Sn}=120)$

Which of the following will form a cell with the highest voltage?

Ionic mobility of $\mathrm{A}{\mathrm{g}^ + }$ is
( ${\lambda _{\mathrm{A}{\mathrm{g}^ + }}} = 5 \times {10^{ - 1}}{\kern 1pt} {\kern 1pt}{\Omega ^{ - 1}}{\kern 1pt} {\kern 1pt}\mathrm{c}{\mathrm{m}^2}{\kern 1pt} {\kern 1pt}\mathrm{equi}{\mathrm{v}^{ - 1}}$ )

In the concentration cells, the electrical energy is produced due to :

The equivalent conductivity of a solution containing 2.54 g of $\mathrm{CuS}{\mathrm{O}_4}{\kern 1pt} {\kern 1pt} \mathrm{per L is}{\kern 1pt} {\kern 1pt} {\kern 1pt} 91.0{\mathrm{\Omega }^{ - 1}}\mathrm{c}{\mathrm{m}^2}\mathrm{e}{\mathrm{q}^{ - 1}}$. Its conductivity would be

The factor temperature coefficient of e.m.f. is :

Standard reduction potentials of the half reactions are given below :

${\mathrm{F}_2}\left( \mathrm{g} \right) + 2{e^ - } \to 2{\mathrm{F}^ - }\left( {aq} \right);{E^ \circ } = + 2.85\mathrm{V}$

$\mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right) + 2{e^ - } \to 2\mathrm{C}{\mathrm{l}^ - }\left( {aq} \right);{E^ \circ } = + 1.36\mathrm{V}$

$\mathrm{B}{\mathrm{r}_2}\left( l \right) + 2{e^ - } \to 2\mathrm{B}{\mathrm{r}^ - }\left( {aq} \right);{E^ \circ } = + 1.06\mathrm{V}$

${\mathrm{I}_2}\left( s \right) + 2{\mathrm{e}^ - } \to 2{\mathrm{I}^ - }\left( {aq} \right);{E^ \circ } = + 0.53V$

The strongest oxidising and reducing agents respectively are :

When Cu reacts with $\mathrm{AgN}{\mathrm{O}_3}$ solution, the reaction takes place is

The number of Faraday’s needed to reduce 4 g-equivalents of $\mathrm{C}{\mathrm{u}^{2 + }}$ to Cu metal will be

The charge in coulomb on $\mathrm{C}{\mathrm{u}^{2 + }}$ ion is :

Which of the following statements is incorrect regarding electrochemistry?

The value of equilibrium constant for a feasible cell reaction is :

For the following cell with hydrogen electrodes at two different pressures ${p_1}{\kern 1pt} {\kern 1pt} \mathrm{and}{\kern 1pt} {\kern 1pt} {p_2}$

$\mathop {\mathrm{Pt}\left( {{\mathrm{H}_2}} \right)}\limits_{{p_1}} \left| {\mathop {{\mathrm{H}^ + }\left( {aq} \right)}\limits_{1\mathrm{ }M} } \right|\mathop {Pt\left( {{\mathrm{H}_2}} \right)}\limits_{{p_2}}$

emf is given by

Total charge on 1 mole of a monovalent metal ion is equal to :

${E^0}\left( {N{i^{2 + }}/Ni} \right) = - 0.25V;\,{E^0}\left( {A{u^{3 + }}/Au} \right) = 1.50V$
The emf of the voltaic cell
$Ni/N{i^{2 + }}\left( {1.0M} \right)//A{u^{3 + }}\left( {1.0M} \right)/Au$ is

The laws of electrolysis were proposed by

During discharging of lead storage battery, the density of $38 \% \mathrm{H}_2 \mathrm{SO}_4(\mathrm{w} / \mathrm{w})$ fell from $1.274 \mathrm{~g} / \mathrm{mL}$ to $1.2 \mathrm{~g} / \mathrm{mL}$ of $19.6 \%(\mathrm{w} / \mathrm{w}) \mathrm{H}_2 \mathrm{SO}_4$. What is the number of faradays that have been exchanged during the discharging process? (vol. of $\mathrm{H}_2 \mathrm{SO}_4$ in lead storage battery $=2.36 \mathrm{~L}$ )

Among the following which is the strongest oxidizing agent?

Assertion: More negative the electrode potential greater is the power to act as oxidising agent.

Reason: As the electrode potential becomes more negative there is greater tendency to undergo oxidation.