Electro chemistry practice · Mixed difficulty

Which metal is most readily corroded in moist air?

Four alkali metals$A,B,C$ and $D$ are having respectively standard electrode potential as $- 3.05, - 1.66, - 0.40{\kern 1pt} {\kern 1pt} \mathrm{and}{\kern 1pt} {\kern 1pt} 0.80$. Which one will be the most reactive?

In the electrodeposition of Ag, the silver ions are:

STATEMENT-1 : If $\left(\frac{d E_{\text {cell }}}{d T}\right)_p>0$ for a cell reaction then $\Delta S$ is positive.

STATEMENT-2 : $\Delta S=n F T\left(\frac{d E}{d T}\right)_p$

In a gas lighter, mechanical energy is converted into electrical energy by using crystals of barium titanate. Barium titanate is

Which represents a concentration cell?

The atomic weight of Al is 27. When a current of 5 faraday is passed through a solution of $\mathrm{A}{\mathrm{l}^{3 + }}$ ions, the wt.of Al deposited is :

The value of electronic charge is equal to :

For the cell reaction $\mathrm{Fe} + 2\mathrm{F}{\mathrm{e}^{3 + }} = 3\mathrm{F}{\mathrm{e}^{2 + }}$, which is not possible?

The${E^ \circ }$ for half-cell $\mathrm{Fe}/\mathrm{F}{\mathrm{e}^{2 + }}$ and $\mathrm{Cu}/\mathrm{C}{\mathrm{u}^{2 + }}$ are$- 0.44\mathrm{V}$ and $+ 0.32\mathrm{V}$ respectively, then

${E_1},{E_2}$ , and ${E_3}$ are the emfs of the following three galvanic cells respectively
I. Zn (s) |$Z{n^{2 + }}$ (1 M) || $\mathrm{C}{\mathrm{u}^{2 + }}$ (0.1 M) | Cu (s)
II. Zn (s) |$Z{n^{2 + }}$ (1 M) || $\mathrm{C}{\mathrm{u}^{2 + }}$ (1 M) | Cu (s)
III. Zn (s) | $Z{n^{2 + }}$ (0.1 M) || $\mathrm{C}{\mathrm{u}^{2 + }}$ (1 M) | Cu (s)
Which one of the following is true?

Which of the following reactions is correct for a given electrochemical cell at ${25^ \circ }C$?

$\mathrm{Pt}\left| {\mathrm{B}{\mathrm{r}_2}\left( \mathrm{g} \right)} \right|\mathrm{B}{\mathrm{r}^ - }\left( \mathrm{g} \right)||\mathrm{C}{\mathrm{l}^ - }\left( {aq} \right)\left| {\mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right)} \right|\mathrm{Pt}$

The hydrogen electrode is dipped in a solution of pH = 3 at ${25^ \circ }C$. The reduction potential of the cell would be :

The conductance of a solution of an electrolyte is same as that of its conductivity. The cell used can be said to have cell constant equal to :

The position of some metals in the electrochemical series in decreasing electropositive character is given as $\mathrm{Mg} > Al > Zn > Cu > Ag$. What will happen, if a copper spoon is used to stir a solution of aluminium nitrate?

The reaction $(1/2)\,{H_2}(g) + AgCl(s) = {H^ + }(aq) + C{l^ - }(aq) + Ag(s)$ occurs in the galvanic cell:

The tendency of an electrode to lose electrons is known as

Assertion: When aqueous sodium chloride solution is electrolysed, Oxygen gas is produced at the anode.

Reason: It is due to the overpotential for oxidation of water to oxygen.

The passage of electricity in the Daniell cell when Zn and Cu electrodes are connected:

EMF of hydrogen electrode in term of pH is (at 1 atm pressure)

If ϕ denotes standard reduction potential, which is true:

The cell reaction is spontaneous, when

Indicator electrode is :

Small quantities of solutions of compounds $TX,TY$ and $TZ$ are put into separate test tubes containing X, Y and Z solutions. $TX$ does not react with any of these. $TY$ reacts with both X and Z. $TZ$ reacts with X. The decreasing order of ease of oxidation of the anions ${X^ - },{Y^ - },{Z^ - }$ is

Conductance ‘$C$’ (in$S$) in directly proportional to the area of the electrode and concentration and inversely proportional to length of separation of electrode, the unit of constant of proportionality is:

The minimum equivalent conductance in fused state is shown by :

1 liter of 1M $CuS{O_4}$ solution is electrolysed. After passing 2 F charge, the molarity of $CuS{O_4}$ will be

$\mathrm{Cu}\left( {\mathrm{II}} \right)$ sulphate solution is treated separately with $\mathrm{KCl}$ and KI. In which case, $\mathrm{C}{\mathrm{u}^{2 + }}$ be reduced to $\mathrm{C}{\mathrm{u}^ + }?$

Equal quantities of electricity are passed through three voltameters containing $\mathrm{FeSO}_4, \mathrm{Fe}_2\left(\mathrm{SO}_4\right)_3$, and $\mathrm{Fe}\left(\mathrm{NO}_3\right)_3$. Consider the following statements in this regard:
(1) The amount of iron deposited in $\mathrm{FeSO}_4$ and $\mathrm{Fe}_2\left(\mathrm{SO}_4\right)_3$ is equal
(2) The amount of iron deposited in $\mathrm{Fe}\left(\mathrm{NO}_3\right)_3$ is two thirds of the amount of iron deposited in $\mathrm{FeSO}_4$
(3) The amount of iron deposited in $\mathrm{Fe}_2\left(\mathrm{SO}_4\right)_3\,\mathrm{Fe}\left(\mathrm{NO}_3\right)_3$ is equal
Of these statements:

Daniel cell, anode and cathode are respectively