Electrochemical Series

Q. What do you observe? When ​
(g) Sodium chloride solution is added to silver nitrate solution.

Q. Divide the following redox reactions into oxidation and reduction half reactions.​
Zn + $P{b}^2+$ → $Z{n}^2$${}^{+}$ + Pb​

Q.

Why cannot we store ${\mathrm{AgNO}}_3$ solution in a copper vessel?

Q. A reaction of a type: ​

$\text{AB}+\text{CD}\to \text{AD}+\text{CB}$, involves

1. Combination of AB and CD
2. Exchange of ions of AB and CD
3. Decomposition of AB and CD
4. No chemical change

Q. If a metal X displaces Fe, Zn and Cu but not Al, then which of these can displace X?

1. Fe
2. Al
3. Cu
4. Zn

Q. The increasing order of the oxidizing power of these following compounds :

Q.

For the reduction of $N{O}_3^{\ominus }$ ion in an aqueous solution, $E^{\ominus }$ is +0.96 V, the values of $E^{\ominus }$ for some metal ions are given below:
$\left(i\right)V^{2+}\left(aq\right)+2e^{-}\to V;E^{\ominus }=-1.19V$
$\left(ii\right)F{e}^{3+}\left(aq\right)+3e^{-}\to Fe;E^{\ominus }=-0.04V$
$\left(iii\right)A{u}^{3+}\left(aq\right)+3e^{-}\to Au;E^{\ominus }=+1.40V$
$\left(iv\right)H{g}^{2+}\left(aq\right)+2e^{-}\to Hg;E^{\ominus }=+0.86V$

The pair(s) of metals that is/are oxidized by $N{O}_3^{\ominus }$ in aqueous solution is/are
(IIT-JEE, 2010)

1. $Fe$ and $Au$

2. $Hg$ and $Fe$

3. $V$ and $Hg$

4. $Fe$ and $V$

Q.

A solution containing 1 mol per litre of each $Cu(N{O}_3{)}_2,AgN{O}_3,$ and $H{g}_2(N{O}_3{)}_2$ is being electrolyzed by using inert electrodes. The values of standard electrode potentials in volts (reduction potential) are
$Ag|A{g}^{⨁}=+0.80,2Hg|H{g}_2^{2+}=+0.79$
$Cu|C{u}^{2+}=+0.34,Mg|M{g}^{2+}=-2.37$
with increasing voltage, the sequence of deposition of metals at the cathode will be
(IIT-JEE, 1984)

1. $Ag,Hg,Cu$

2. $Ag,Hg,Cu,Mg$

3. $Mg,Cu,Hg,Ag$

4. $Cu,Hg,Ag$

Q. Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential $\left(E_{\ominus }\right)$ of two half cell reactions decided which way the reaction is expected to proceed. A simple example is a Daniell cell in which zinc goes into solution and copper gets deposited. Given below are a set of half cell reactions (acidic medium) along with their $E_{\ominus }$ (V with respect to normal hydrogen electrode) values. Using this data, obtain correct explanations for the following question
$I_2+2e^{-}\to 2I^{\ominus };E^{\ominus }=0.54$
$C{l}_2+2e^{-}\to 2C{l}^{\ominus };E^{\ominus }=1.36$
$M{n}^{3+}+e^{-}\to M{n}^{2+};E^{\ominus }=1.50$
$F{e}^{3+}+e^{-}\to F{e}^{2+};E^{\ominus }=0.77$
$O_2+4H^{⨁}+4e^{-}\to 2H_{2}O;E^{\ominus }=1.23$

While $F{e}^{3+}$ is stable, $M{n}^{3+}$ is not stable in acid solution because

1. $O_{2}oxidizesbothM{n}^{2+}toM{n}^{3+}andF{e}^{2+}toF{e}^{3+}$
2. $O_{2}oxidizesM{n}^{2+}toM{n}^{3+}$
3. $F{e}^{3+}oxidizes{H}_{2}Oto{O}_2$
4. $M{n}^{3+}oxidizes{H}_{2}Oto{O}_2$

Q. An aqueous solution containing one mole per litre of each $Cu(N{O}_3{)}_2,AgN{O}_3,H{g}_2(N{O}_3{)}_2$ and $Mg(N{O}_3{)}_2$, is being electrolysed by using inert electrodes. The values of standard electrode potentials in volts (reduction potentials) are $Ag/A{g}^{+}=+0.80,2Hg/H{g}_2^{2+}=+0.79,Cu/C{u}^{2+}=+0.34,Mg/M{g}^{2+}=-2.37$ with increasing voltage, the sequence of deposition of metals on the cathode will be

1. Ag, Hg, Cu
2. Cu, Hg, Ag
3. Ag, Hg, Cu, Mg
4. Mg, Cu, Hg, Ag

Q. This question and the following one were a part of a linked comprehension in the (IIT-JEE, 2008) exam.

Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential $\left(E_{\ominus }\right)$ of two half cell reactions decided which way the reaction is expected to proceed. A simple example is a Daniell cell in which zinc goes into solution and copper gets deposited. Given below are a set of half cell reactions (acidic medium) along with their $E_{\ominus }$ (V with respect to normal hydrogen electrode) values. Using this data, obtain correct explanations for the follwing questions.
$I_2+2e^{-}\to 2I_{\ominus };E^{\ominus }=0.54$
$C{l}_2+2e^{-}\to 2C{I}_{\ominus };E^{\ominus }=1.36$
$M{n}^{3+}+e^{-}\to M{n}^{2+};E^{\ominus }=1.50$
$F{e}^{3+}+e^{-}\to F{e}^{2+};E^{\ominus }=0.77$
$O_2+4H^{⨁}+4e^{-}\to 2H_{2}I;E^{\ominus }=1.23$

Among the following, identify the correct statement.

1. Chloride ion is oxidized by $O_2.$
2. $F{e}^{2+}$ is oxidized by iodine.
3. $M{n}^{2+}$ is oxidized by chlorine.
4. Iodide ion is oxidized by chlorine.

Q. You want to store a freshly made solution of copper sulphate. You have 4 options with you. Which of these is preferable to ensure that the solution remains intact?

Reduction potentials:
$Z{n}^{2+}/Zn=-0.76$
$M{g}^{2+}/Mg=-2.37$
$C{u}^{2+}/Cu=0.34$
$A{g}^{+}/Ag=0.8$
$S{n}^{2+}/Sn=0.16$

1. Zn vessel
2. Magnesium vessel
3. Tin vessel
4. Silver vessel

Q.

Complete the following ionic equations in reference to electrolysis and electroplating

$$\begin{gathered} 1.{\mathrm{CuSO}}_4\rightleftharpoons \mathrm{\_\_\_\_\_}+\mathrm{\_\_\_\_\_\_} \\ 2.{\mathrm{H}}_2\mathrm{O}\rightleftharpoons \mathrm{\_\_\_\_\_\_}+\mathrm{\_\_\_\_\_\_\_} \\ 3.{\mathrm{Cu}}^{+2}+\mathrm{\_\_\_\_}\to \mathrm{\_\_\_\_\_} \\ 4.\mathrm{Cu}-\mathrm{\_\_\_\_}\to \mathrm{\_\_\_\_\_\_} \end{gathered}$$

Q.
For the reduction of $N{O}_3^{-}$ ion in an aqueous solution $E^{\circ }$ is +0.96 V. Values of $E^{\circ }$ for some metal ions are given below:
$V^{2+}\left(aq\right)+2e^{-}\to V;E^0=-1.19V$
$F{e}^{3-}\left(aq\right)+3e^{-}\to Fe;E^{\circ }=-0.04V$
$A{u}^{3+}\left(aq\right)+3e^{-}\to Au;E^{\circ }=+1.40V$
$H{g}^{2+}\left(aq\right)+2e^{-}\to Hg;E^0=+0.86V$
The pair(s) of metals that is/are oxidised by $N{O}_3^{-}$ in aqueous solution is (are)

1. V and Hg
2. Hg and Fe
3. Fe and Au
4. Fe and V

Q. Iron reacts with conc.$HCl$ and conc.$H_2{SO}_4$. But it does not react with conc. $H{NO}_3$. Suggest your answer with proper reason.