Electrolytic Cell

Q. How many electrons are present in 3.2g sulphide ions ?

Q.

A cell is prepared by dipping a chromium rod in 1M Cr₂(SO₄)₃ solution and an iron rod in 1M FeSO₄ solution. The standard reduction potentials of Chromium and Iron electrodes are -0.75 V and -0.45 V respectively. What will be the standard EMF of the cell?

1. -0.47 V

2. - 0.30 V

3. +0.30 V

4. +0.47 V

Q.

The salt bridge in the electrochemical cell serves to

1. accelerate the attainment of equilibrium

2. increase the voltage of the cell

3. maintain electrical neutrality

4. increase the oxidation/reduction rate

Q. What will be the toal no of ions and charge in A2B3 ? Solution needed.

Q. Why first ionization energy if sodium is less then magnesium?

Q. Starting with sodium chloride how would you proceed to prepare (i) sodium metal, (ii) sodium hydroxide, (iii) sodium peroxide, (iv) sodium carbonate?

Q. Does metallic hydrides conduct electricity in solid form?

Q. Depict the galvanic cell in which the reaction $Zn\left(s\right)+2A{g}^{+}\left(aq\right)\to Z{n}^{2+}\left(aq\right)+2Ag\left(s\right)$ takes place. Further show which of the electrode is negatively charged.

Q.

In the electrolytic cell, flow of electrons is fron:

1. Cathode to anode in solution

2. Cathode to anode through external supply

3. Cathode to anode through solution

4. Anode to cathode through external supply

Q. 3.State true or false with explained reason 1) electrical conduction reduces in schottky defect 2)in f centre defect electrical conductance increases 3) in extra positive ions and electron defect electrical conductance increases 4)in positive in absent defect conductance reduces Explain with reason all 4 statement and also retify the wrong ones

Q.

An electric current is passed through an aqueous solution of lithium bromide.
What are produced at the cathode and anode respectively?

1. At cathode : $H_2$(g)
   At anode : $O_2$(g)
2. At cathode : $Li\left(s\right)$
   At anode : $B{r}_2\left(l\right)$
3. At cathode : $B{r}_2$(l)
   At anode : $Li\left(s\right)$
4. At cathode : $O_2$(g)
   At anode : $H_2$(g)

Q. What is the difference between ionization enthalpy and ionization potential?

Q.

What is the number of moles of KMnO4 that will be needed to react with one mole of sulphite ion in acidic solution?

Q.

Give a reason for the following

Electrolysis of molten lead bromide is considered to be a reaction in which oxidation and rection go side by side, that is a redox reaction.

Q. What is the difference between ionization enthalpy and ionization energy?

Q. A reversible galvanic cell is connected to an external battery. If the electric potential of the battery is less than the electric potential of the galvanic cell, then the current:

1. Will flow from battery to the galvanic cell
2. 
   Will not pass through the circuit
3. Can flow in any direction
4. Will flow from galvanic cell to the battery

Q. How to find the partial charge ?; Its formula

Q. In a cell , the following reaction takes place:

$Fe\left(s\right)+CuS{O}_4\left(aq\right)\to FeS{O}_4\left(aq\right)+Cu\left(s\right)$

The correct cell representation is:

1. $C{u}^{2+}\left(aq\right)|Cu\left(s\right)||Fe\left(s\right)|F{e}^{2+}\left(aq\right)$
2. $C{u}^{2+}\left(aq\right)|Cu\left(s\right)||F{e}^{2+}\left(aq\right)|Fe\left(s\right)$
3. $Fe\left(s\right)|F{e}^{2+}\left(aq\right)||C{u}^{2+}\left(aq\right)|Cu\left(s\right)$
4. $Cu\left(s\right)|C{u}^{2+}\left(aq\right)||Fe\left(s\right)|F{e}^{2+}\left(aq\right)$

Q. is formal charge on sulphur in H2SO4 is 0 or +2

Q. IN MILLIKAN OIL DROP EXPERIMENT WHY HIGHLY VISCOUS LIQUID IS USED INSTEAD OF LOW VISCOUS LIQUID?

Q. A galvanic cell is formed by immersing $Ag\left(s\right)$ in $AgN{O}_3(aq,0.1M)$ and $Cu\left(s\right)$ in $CuS{O}_4(aq,4M)$ at $298\text{K}$
Calculate the EMF of the cell.
Given:
$E_{A{g}^{+}/Ag}^0=0.80V$
$E_{C{u}^{2+}/Cu}^0=0.34V$

1. $E_{cell}=0.301V$
2. $E_{cell}=0.383V$
3. $E_{cell}=0.45V$
4. $E_{cell}=1.04V$

Q. The product obtained from the electrolytic oxidation of acidified sulphate solution , is

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1. $HS{O}_4^{-}$
2. $H{O}_{2}SOS{O}_{2}H$
3. $H{O}_{3}SOS{O}_{3}H$
4. $H{O}_{3}SOOS{O}_{3}H$

Q. How to find n factor for salts and how to calculate cationic charge

Q. Sodium reacts with water more vigorously than lithium because:

1. it has higher atomic mass
2. it is more electronegative
3. it is a metal
4. it is more electropositive

Q. $\begin{array}{cccc}& \text{List - I}& & \text{List - II}\\ \text{(P)}& \text{Very dilute solution of HCl}& \text{(1)}& O_2\text{evolved at anode}\\ \text{(Q)}& \text{Very dilute solution of KCl}& \text{(2)}& H_2\text{evolved at cathode}\\ \text{(R)}& \text{Concentrated solution of NaCl}& \text{(3)}& C{l}_2\text{evolved at anode}\\ \text{(S)}& \text{Fairly concentrated solution of}AgN{O}_3& \text{(4)}& \text{Na deposition at cathode}\\ & & \text{(5)}& \text{Ag deposition at cathode}\\ & & \text{(6)}& \text{K deposition at cathode}\end{array}$
Match each product in LIST-I with one or more reaction in LIST-II and choose the correct option.

1. $P\to 1,2;Q\to 1,2;R\to 2,3;S\to 1,5$
2. $P\to 1,2;Q\to 2,3;R\to 2,3;S\to 1,5$
3. $P\to 2,3;Q\to 3,6;R\to 3,4;S\to 1,5$
4. $P\to 2,3;Q\to 3,6;R\to 2,3;S\to 2,5$

Q.

We know that an electrolytic cell has three main components, an electrolyte and two electrodes (an anode and a cathode) and the electrolyte can come in two forms, either as molten or in an aqueous solution. Which of the following statements accurately describes an electrolytic cell?

1. Alkali or alkaline earth metals, which are the cations of the electrolyte, do not get oxidized in an aqueous solution since water is more easily oxidized.
2. Polyatomic ions, which are the anions of the electrolyte, are typically more easily oxidized than water.
3. In both molten or aqueous forms, the cation will be reduced and the anion will be oxidized.
4. For aqueous solutions of the electrolyte, a gas may be produced at the anode.