Standard electrode potentials for a few half cells are mentioned below : $$\begin{array}{rl}& {\mathrm{E}}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}^{\circ }=0.34\mathrm{V},{\mathrm{E}}_{{\mathrm{Zn}}^{2+}/\mathrm{Zn}}^{\circ }=-0.76\mathrm{V}\\ & {\mathrm{E}}_{{\mathrm{Ag}}^{+}/\mathrm{Ag}}^{\circ }=0.80\mathrm{V},{\mathrm{E}}_{{\mathrm{Mg}}^{2+}/\mathrm{Mg}}^{\circ }=-2.37\mathrm{V}\end{array}$$ Which one of the following cells gives the most negative value of $\Delta {\mathrm{G}}^{\circ }$ ?

For the given cell $${\mathrm{Fe}}^{2+}(\mathrm{aq})+{\mathrm{Ag}}_{(\mathrm{aq})}^{+}\to {\mathrm{Fe}}^{3+}(\mathrm{aq})+{\mathrm{Ag}}_{(\mathrm{s})}$$ The standard cell potential of the above reaction is Given: $$\begin{array}{lr}{\mathrm{Ag}}^{+}+{\mathrm{e}}^{-}\to \mathrm{Ag}& {\mathrm{E}}^{\theta }=\mathrm{xV}\\ {\mathrm{Fe}}^{2+}+2{\mathrm{e}}^{-}\to \mathrm{Fe}& {\mathrm{E}}^{\theta }=\mathrm{yV}\\ {\mathrm{Fe}}^{3+}+3{\mathrm{e}}^{-}\to \mathrm{Fe}& {\mathrm{E}}^{\theta }=\mathrm{zV}\end{array}$$

Based on the data given below : $$\begin{array}{ll}{\mathrm{E}}_{{\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}/{\mathrm{Cr}}^{3+}}^{\circ }=1.33\mathrm{V}& {\mathrm{E}}_{{\mathrm{Cl}}_2/{\mathrm{Cl}}^{(-)}}^{\circ }=1.36\mathrm{V}\\ {\mathrm{E}}_{{\mathrm{MnO}}_4^{-}/{\mathrm{Mn}}^{2+}}^0=1.51\mathrm{V}& {\mathrm{E}}_{{\mathrm{Cr}}^{3+}/\mathrm{Cr}}^{\circ }=-0.74\mathrm{V}\end{array}$$ the strongest reducing agent is :

Correct order of limiting molar conductivity for cations in water at 298 K is :

Given below are two statements : 1 M aqueous solutions of each of Cu(NO3)2, AgNO3, Hg2(NO3)2, Mg(NO3)2 are electrolysed using inert electrodes. Given: E0Ag+/Ag = 0.80 V, E0Hg22+/Hg = 0.79 V, E0Cu2+/Cu = 0.24 V and E0Mg2+/Mg = -2.37 V.Statement (I) : With increasing voltage, the sequence of deposition of metals on the cathode will be Ag, Hg and Cu.Statement (II) : Magnesium will not be deposited at the cathode instead oxygen gas will be evolved at the cathode.In the light of the above statements, choose the most appropriate answer from the options given below :

On charging the lead storage battery, the oxidation state of lead changes from $x_1$ to $y_1$ at the anode and from $x_2$ to $y_2$ at the cathode. The values of $x_1,y_1,x_2,y_2$ are respectively :

The standard cell potential $\left({\mathrm{E}}_{\text{cell }}^{\ominus }\right)$ of a fuel cell based on the oxidation of methanol in air that has been used to power television relay station is measured as 1.21 V . The standard half cell reduction potential for ${\mathrm{O}}_2\left({\mathrm{E}}_{{\mathrm{O}}_2/{\mathrm{H}}_2\mathrm{O}}^{\circ }\right)$ is 1.229 V . Choose the correct statement :

The correct option with order of melting points of the pairs (Mn, Fe), (Tc, Ru) and (Re, Os) is :

Lanthanoid ions with $4{\mathrm{f}}^7$ configuration are : (A) ${\mathrm{Eu}}^{2+}$ (B) ${\mathrm{Gd}}^{3+}$ (C) ${\mathrm{Eu}}^{3+}$ (D) ${\mathrm{Tb}}^{3+}$ (E) ${\mathrm{Sm}}^{2+}$ Choose the correct answer from the options given below :

The amphoteric oxide among ${\mathrm{V}}_2{\mathrm{O}}_3,{\mathrm{V}}_2{\mathrm{O}}_4$ and ${\mathrm{V}}_2{\mathrm{O}}_5$, upon reaction with alkali leads to formation of an oxide anion. The oxidation state of V in the oxide anion is :

The correct set of ions (aqueous solution) with same colour from the following is:

Match List - I with List - II .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-c3ow{border-color:inherit;text-align:center;vertical-align:top} .tg .tg-7btt{border-color:inherit;font-weight:bold;text-align:center;vertical-align:top} .tg .tg-0pky{border-color:inherit;text-align:left;vertical-align:top} List - I List - II (A) Bronze (I) Cu, Ni (B) Brass (II) Fe, Cr, Ni, C (C) UK silver coin (III) Cu, Zn (D) Stainless steel (IV) Cu, Sn Choose the correct answer from the options given below :

Consider the following reactions $${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7\underset{-{\mathrm{H}}_2\mathrm{O}}{\overset{\mathrm{KOH}}{\to }}[\mathrm{A}]\underset{-{\mathrm{H}}_2\mathrm{O}}{\overset{{\mathrm{H}}_2{\mathrm{SO}}_4}{\to }}[\mathrm{B}]+{\mathrm{K}}_2{\mathrm{SO}}_4$$ The products $[A]$ and $[B]$, respectively are :

Preparation of potassium permanganate from ${\mathrm{MnO}}_2$ involves two step process in which the 1st step is a reaction with KOH and ${\mathrm{KNO}}_3$ to produce

Which of the following ions is the strongest oxidizing agent? (Atomic Number of $\mathrm{Ce}=58,\mathrm{Eu}=63,\mathrm{Tb}=65,\mathrm{Lu}=71$)

Match List - I with List - II. .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-baqh{text-align:center;vertical-align:top} .tg .tg-amwm{font-weight:bold;text-align:center;vertical-align:top} .tg .tg-0lax{text-align:left;vertical-align:top} List - I (Transition metal ion) List - II (Spin only magnetic moment (B.M.)) (A) ${\mathrm{Ti}}^{3+}$ (I) 3.87 (B) ${\mathrm{V}}^{2+}$ (II) 0.00 (C) ${\mathrm{Ni}}^{2+}$ (III) 1.73 (D) ${\mathrm{Sc}}^{3+}$ (IV) 2.84 Choose the correct answer from the options given below :

The metal ion whose electronic configuration is not affected by the nature of the ligand and which gives a violet colour in non-luminous flame under hot condition in borax bead test is

The correct decreasing order of spin only magnetic moment values (BM) of Cu+, Cu2+, Cr2+ and Cr3+ ions is :

The first transition series metal ' $M$ ' has the highest enthalpy of atomisation in its series. One of its aquated ion $\left({\mathrm{M}}^{\mathrm{n}+}\right)$ exists in green colour. The nature of the oxide formed by the above ${\mathrm{M}}^{\mathrm{n}+}$ ion is:

The metal ions that have the calculated spin-only magnetic moment value of 4.9 B.M. are : A. ${\mathrm{Cr}}^{2+}$ B. ${\mathrm{Fe}}^{2+}$ C. ${\mathrm{Fe}}^{3+}$ D. ${\mathrm{Co}}^{2+}$ E. ${\mathrm{Mn}}^{3+}$ Choose the correct answer from the options given below: