Electrochemical Series

Q. An electrolytic solution contains ${\mathrm{Al}}^{3+}$, and ${\mathrm{Au}}^{3+}$ ions. If the solution is electrolysed, ________ ion would be deposited at the ________.

1. Au, cathode
2. Al, anode
3. Au, anode
4. Al, cathode

Q.

The element A placed above element B in the electrochemical series can displace element B from its salt.

1. False

2. True

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. For the reduction of /( NO_{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 NO_{3}^{\ominus } in aqueous solution is/are
(IIT-JEE, 2010)

1. (a) Fe and Au
2. (b) Hg and Fe
3. (c) V and Hg
4. (d) Fe and V

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. Tin vessel

3. Silver vessel

4. Magnesium vessel

Q. Given, $E_{C{r}^{(}3+)/Cr}^0=-0.74V;E_{Mn{O}_4^{-}/M{n}^{2+}}^0=1.51V$
$E_{C{r}_2{O}_7^{2-}/C{r}^{3+}}^0=1.33V;E_{Cl/C{l}^{-}}^0=1.36V$
Based on the data given above strongest oxidising agent will be

1. $C{r}^{3+}$
2. $M{n}^{2+}$
3. $Mn{O}_4^{-}$
4. $C{l}^{-}$

Q. Which of the following elements cannot displace hydrogen form $H_{2}S{O}_4$?

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

Q.

$E_{A{g}^{+}|Ag}^{\circ }=0.8$ volt and $E_{Z{n}^{2+}|Zn}^{\circ }=-0.76$ volt

Which of the following is correct?

1. 
2. 
3. 
4. 

Q.

Which of the following statements about electrochemical series is wrong?

1. It does not compare the relative reactivity of metals
2. It compares relative strengths of oxidizing agents
3. H₂ is centrally placed element
4. It is the representation of element in order of increasing or decreasing standard electrode reduction potential

Q.

The standard reduction potential data at ${25}^{\circ }C$ is given below.

$E^{\circ }\left(F{e}^{3+}/F{e}^{2+}\right)=0.77V;E^{\circ }\left(F{e}^{2+}/Fe\right)=-0.44V;E^{\circ }\left(C{u}^{2+}/Cu\right)=0.34V;E^{\circ }\left(C{u}^{+}/Cu\right)=+0.52V;E^{\circ }\left(O_2\right(g)+4H^{+}+4e^{-})\to 2H_{2}O=+1.23V;E^{\circ }\left(O_2\right(g)+2H_{2}O+4e^{-})\to 4O{H}^{-}=+0.40V{E}^{\circ }\left(C{r}^{3+}/Cr\right)=-0.74V;E^{\circ }\left(C{r}^{2+}/Cr\right)=+0.91V$

Match $E^{\circ }$ of the rebox pair in Column I with the values given in Column II and select the correct answer using the code given below the lists.

$\begin{array}{cc}ColumnI& ColumnII\\ P.E^{\circ }\left(F{e}^{3+}/Fe\right)& 1.-0.18V\\ Q.E^{\circ }(4H_{2}O\rightleftharpoons 4H^{+}+4O{H}^{-})& 2.-0.4V\\ R.E^{\circ }(C{u}^{2+}+Cu\to 2C{u}^{+})& 3.-0.04V\\ S.E^{\circ }\left(C{r}^{3+}/C{r}^{2+}\right)& 4.-0.83V\end{array}$

1. P - (2) Q - (3) R - (4) S - (1)

2. P - (1) Q - (2) R - (3) S - (4)

3. P - (3) Q - (4) R - (1) S - (2)

4. P - (4) Q - (1) R - (2) S - (3)