Galvanic cells and EMF

An electrochemical cell is constructed using half cells in the direction of spontaneous change
$$\ce{Fe(OH)2(s) + 2e- -> Fe(s) + 2OH-(aq)}\qquad E^\theta=-0.88\ \mathrm V$$
and $$\ce{AgBr(s) + e- -> Ag(s) + Br-(aq)}\qquad E^\theta=+0.07\ \mathrm V$$
Which of the following option is correct ?

An aqueous solution of hydrazine ($\ce{N2H4}$) is electrochemically oxidized by $\ce{O2}$, thereby releasing chemical energy in the form of electrical energy. One of the products generated from the electrochemical reaction is $\ce{N2(g)}$.

Choose the correct statement(s) about the above process

The reduction potential ($E^0$, in V) of $\ce{MnO4^-(aq)}/\ce{Mn(s)}$ is _____.

[Given: $E^0_{(\ce{MnO4^-(aq)}/\ce{MnO2(s)})} = 1.68$ V; $E^0_{(\ce{MnO2(s)}/\ce{Mn^2+(aq)})} = 1.21$ V; $E^0_{(\ce{Mn^2+(aq)}/\ce{Mn(s)})} = -1.03$ V]

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.

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 ?

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

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]

Which of the following has least tendency to liberate $\mathrm{H_2}$ from mineral acids ?

The E° (volt) values are : Al$^{3+}$/Al, −1.66, Sc$^{3+}$/Sc, −2.08, Fe$^{3+}$/Fe$^{2+}$, +0.77, Hg$_2^{2+}$/Hg, +0.79. Arrangement of cations, Al$^{3+}$, Sc$^{3+}$, Fe$^{3+}$ and Hg$_2^{2+}$ in decreasing order of oxidizing strength is

Some standard electrode potentials at 298 K are given below:

Couple	$E^\circ$
$\ce{Pb^{2+}/Pb}$	−0.13 V
$\ce{Ni^{2+}/Ni}$	−0.24 V
$\ce{Cd^{2+}/Cd}$	−0.40 V
$\ce{Fe^{2+}/Fe}$	−0.44 V

To a solution containing 0.001 M of $\mathbf X^{2+}$ and 0.1 M of $\mathbf Y^{2+}$, the metal rods $\mathbf X$ and $\mathbf Y$ are inserted (at 298 K) and connected by a conducting wire. This resulted in dissolution of $\mathbf X$. The correct combination(s) of $\mathbf X$ and $\mathbf Y$, respectively, is(are)

(Given: Gas constant, R = 8.314 J K$^{-1}$ mol$^{-1}$, Faraday constant, F = 96500 C mol$^{-1}$)

The electrode potential of M$^{2+}$/M of 3d-series elements shows positive value for :

The correct option(s) to distinguish nitrate salts of $\mathrm{Mn^{2+}}$ and $\mathrm{Cu^{2+}}$ taken separately is (are)

Given $E^\circ_{\ce{Cl2/Cl-}}=1.36$ V, $E^\circ_{\ce{Cr^3+/Cr}}=-0.74$ V, $E^\circ_{\ce{Cr2O7^2-/Cr^3+}}=1.33$ V, $E^\circ_{\ce{MnO4-/Mn^2+}}=1.51$ V.

Among the following, the strongest reducing agent is :

Consider the following standard electrode potentials (E° in volts) in aqueous solution :

Element	$\ce{M^3+/M}$	$\ce{M+/M}$
Al	−1.66	+0.55
Tl	+1.26	−0.34

Based on these data, which of the following statements is correct ?

To find the standard potential of $\ce{M^3+/M}$ electrode, the following cell is constituted : $\ce{Pt/M/M^3+}$(0.001 mol L$^{-1}$)/$\ce{Ag+}$(0.01 mol L$^{-1}$)/Ag

The emf of the cell is found to be 0.421 volt at 298 K. The standard potential of half reaction $\ce{M^3+ + 3e- -> M}$ at 298 K will be :

(Given $E^\circ_{\ce{Ag+/Ag}}$ at 298 K = 0.80 Volt)

Which of the following ions does not liberate hydrogen gas on reaction with dilute acids ?

Galvanization is applying a coating of :