Electrochemistry

Among the following, which is the strongest oxidizing agent ?

In a cell, the following reactions take place
$$\mathrm{Fe^{2+}\rightarrow Fe^{3+}+e^-}\qquad E^\circ_{\mathrm{Fe^{3+}/Fe^{2+}}}=0.77\ \mathrm V$$
$$\mathrm{2I^-\rightarrow I_2+2e^-}\qquad E^\circ_{\mathrm{I_2/I^-}}=0.54\ \mathrm V$$
The standard electrode potential for the spontaneous reaction in the cell is $x\times10^{-2}$ V 298 K. The value of $x$ is ______. (Nearest Integer)

The correct order of reduction potentials of the following pairs is

A. $\mathrm{Cl_2/Cl^-}$

B. $\mathrm{I_2/I^-}$

C. $\mathrm{Ag^+/Ag}$

D. $\mathrm{Na^+/Na}$

E. $\mathrm{Li^+/Li}$

Choose the correct answer from the options given below.

A solution of $\mathrm{Fe_2(SO_4)_3}$ is electrolyzed for 'x' min with a current of 1.5 A to deposit 0.3482 g of Fe. The value of x is ______. [nearest integer]

Given : 1 F = 96500 C mol$^{-1}$

Atomic mass of Fe = 56 g mol$^{-1}$

The $\left(\dfrac{\partial E}{\partial T}\right)_P$ of different types of half cells are as follows :
$$\begin{array}{cccc}A&B&C&D\\1\times10^{-4}&2\times10^{-4}&0.1\times10^{-4}&0.2\times10^{-4}\end{array}$$
(Where E is the electromotive force)

Which of the above half cells would be preferred to be used as reference electrode ?

$$\mathrm{Cu(s)+Sn^{2+}(0.001M)\rightarrow Cu^{2+}(0.01M)+Sn(s)}$$
The Gibbs free energy change for the above reaction at 298 K is $x\times10^{-1}$ kJ mol$^{-1}$. The value of $x$ is ______. [nearest integer]

[Given : $E^\ominus_{\mathrm{Cu^{2+}/Cu}}=0.34$ V; $E^\ominus_{\mathrm{Sn^{2+}/Sn}}=-0.14$ V; $F=96500$ C mol$^{-1}$]

The limiting molar conductivities of NaI, $\mathrm{NaNO_3}$ and $\mathrm{AgNO_3}$ are 12.7, 12.0 and 13.3 mS m$^2$ mol$^{-1}$, respectively (all at 25°C). The limiting molar conductivity of AgI at this temperature is ______ mS m$^2$ mol$^{-1}$.

In 3d series, the metal having the highest $\mathrm{M^{2+}/M}$ standard electrode potential is

For the reaction taking place in the cell:
$$\mathrm{Pt(s)|H_2(g)|H^+(aq)\,||\,Ag^+(aq)|Ag(s)}$$
$E^\circ_{\rm cell}=+0.5332$ V.

The value of $\Delta_fG^\ominus$ is ______ kJ mol$^{-1}$. (in nearest integer)

The solubility product of a sparingly soluble salt $\mathrm{A_2X_3}$ is $1.1\times10^{-23}$. If specific conductance of the solution is $3\times10^{-5}$ S m$^{-1}$, the limiting molar conductivity of the solution is $x\times10^{-3}$ S m$^2$ mol$^{-1}$. The value of $x$ is ______.

The quantity of electricity in Faraday needed to reduce 1 mol of $\mathrm{Cr_2O_7^{2-}}$ to $\mathrm{Cr^{3+}}$ is ______

For the given reactions

$$\mathrm{Sn^{2+}+2e^-\rightarrow Sn}$$
$$\mathrm{Sn^{4+}+4e^-\rightarrow Sn}$$

the electrode potentials are ; $E^\circ_{\mathrm{Sn^{2+}/Sn}}=-0.140$ V and $E^\circ_{\mathrm{Sn^{4+}/Sn}}=0.010$ V. The magnitude of standard electrode potential for $\mathrm{Sn^{4+}/Sn^{2+}}$ i.e. $E^\circ_{\mathrm{Sn^{4+}/Sn^{2+}}}$ is ______ $\times10^{-2}$ V. (Nearest integer)

A dilute solution of sulphuric acid is electrolysed using a current of 0.10 A for 2 hours to produce hydrogen and oxygen gas. The total volume of gases produced at STP is ______ cm$^3$. (Nearest integer)

[Given : Faraday constant F = 96500 C mol$^{-1}$ at STP, molar volume of an ideal gas is 22.7 L mol$^{-1}$]

The cell potential for the given cell at 298 K

$\mathrm{Pt\,|\,H_2(g,1\,bar)\,|\,H^+(aq)\,||\,Cu^{2+}(aq)\,|\,Cu(s)}$

is 0.31V. The pH of the acidic solution is found to be 3, whereas the concentration of $\mathrm{Cu^{2+}}$ is $10^{-x}$ M. The value of $x$ is ______.

(Given: $E^\ominus_{\mathrm{Cu^{2+}/Cu}}=0.34$ V and $\dfrac{2.303RT}F=0.06$ V)

In which of the following half cells, electrochemical reaction is pH dependent ?

The cell potential for $\mathrm{Zn|Zn^{2+}(aq)||Sn^{x+}|Sn}$ is 0.801 V at 298 K. The reaction quotient for the above reaction is $10^{-2}$. The number of electrons involved in the given electrochemical cell reaction is ______.

(Given : $E^\circ_{\mathrm{Zn^{2+}|Zn}}=-0.763$ V, $E^\circ_{\mathrm{Sn^{x+}|Sn}}=+0.008$ V and $\dfrac{2.303RT}F=0.06$ V)

The molar conductivity of a conductivity cell filled with 10 moles of 20 mL NaCl solution is $\Lambda_{m1}$ and that of 20 moles another identical cell heaving 80 mL NaCl solution is $\Lambda_{m2}$. The conductivities exhibited by these two cells are same. The relationship between $\Lambda_{m2}$ and $\Lambda_{m1}$ is

The spin-only magnetic moment value of $\mathrm{M^{3+}}$ ion (in gaseous state) from the pairs $\mathrm{Cr^{3+}/Cr^{2+}}$, $\mathrm{Mn^{3+}/Mn^{2+}}$, $\mathrm{Fe^{3+}/Fe^{2+}}$ and $\mathrm{Co^{3+}/Co^{2+}}$ that has negative standard electrode potential, is ______ B.M. [Nearest integer]

The amount of charge in F (Faraday) required to obtain one mole of iron from $\mathrm{Fe_3O_4}$ is ______. (Nearest Integer)

Given below are two statements :

Statement I : For KI, molar conductivity increases steeply with dilution

Statement II : For carbonic acid, molar conductivity increases slowly with dilution

In the light of the above statements, choose the correct answer from the options given below :