NIOS Class 12 Chemistry Chapter 13 Electrochemistry

NIOS Class 12 Chemistry Chapter 13 Electrochemistry Solutions English Medium As Per New Syllabus to each chapter is provided in the list so that you can easily browse throughout different chapters NIOS Class 12 Chemistry Chapter 13 Electrochemistry Notes in English and select need one. NIOS Class 12 Chemistry Solutions English Medium Download PDF. NIOS Study Material of Class 12 Chemistry Notes Paper Code: 313.

NIOS Class 12 Chemistry Chapter 13 Electrochemistry

Also, you can read the NIOS book online in these sections Solutions by Expert Teachers as per National Institute of Open Schooling (NIOS) Book guidelines. These solutions are part of NIOS All Subject Solutions. Here we have given NIOS Class 12 Chemistry Notes, NIOS Senior Secondary Course Chemistry Solutions in English for All Chapter, You can practice these here.

Electrochemistry

Chapter: 13

Module – V: Chemical Dynamics

INTEXT QUESTIONS 13.1

1. Determine the Oxidation number of element in the bold letter in the following:

Ans: Oxidation Number:

–4, –3, +3, +2, +7, +5, 0, +5

2. How does oxidation number change in oxidation and reduction?

Ans: In oxidation O.N. increases.

In reduction O.N. decreases.

3. Mention the oxidising agent and reducing agent in the following.

H₂S + HNO₃ → NO + S + H₂O

Ans: Oxidising agent HNO₃ reducing agent H₂S

4. Write the half reaction for the following:

Mg (s) CI₂ (g) → MCI₂ (s)

I₂ + HNO₃ → HIO₃ + NO₂ + H₂O

Ans: I⁻(aq) → I₂(s)

(i) oxidation:

Fe³⁺ (aq) →Fe²⁺ (aq) (Reduction)

Reduction:

(ii) Mg + Cl₂ → MgCl₂

oxidation:

(iii) I₂ → HIO₃  Oxidation 

HNO₃ → NO₂ reduction

5. Balance the equation by oxidation number method:

(i) CuO + NH₃ → Cu + N₂+ H₂O

Ans: 

(ii) MnO₄ + HCl → MnCl₂ + C₂ + H₂O

Ans: 

6. Balance the following by ion electrode half reaction method:

Ans:

INTEXT QUESTION 13.2

1. How does the solution of electrolytes conduct electricity?

Ans: Electrolytes give ions in the solution and these ions conduct electricity by moving to their respective electrodes i.e. cations towards cathode and anions towards anode.

2. Define conductivity and molar conductivity.

Ans: Specific conductance is the conductance of a solution taken in a cell in which two electrodes are 1 cm apart and surface area of each one of them is 1 cm².

Equivalent conductance is the conductance of all the ions furnished by an equivalent of the electrolyte in a solution of given concentration.

3. Give the units of conductance and conductivity.

Ans: Conductance S; specific conductance Scm^–1.

4. List factors affecting the conductance of an electrolyte.

Ans: Nature of electrolyte (strong or weak), valency of its ions, speed of ions, concentration and temperature.

5. Draw a graph showing variation in molar conductivity of weak and strong electrolytes.

Ans: 

6. Write the expression for molar conductivity at infinite dilution for Al₂(SO₄)₃.

Ans: λ∞m Al₂ (SO₄)₃ = 2∞λ m Al3+ + 3∞λ m S _2–4O

INTEXT QUESTION 13.2

1. What type of process-spontaneous or non-spontaneous, occurs in (i) electrolytz cell (ii) galvanic cell.

Ans: (i) non-spontaneous (ii) spontaneous.

2. Atomic mass of setner is 108 u. What is its electrochemical equivalent?

Ans: 2. 1.12 × 10–3 g c.

3. Why is salt bridge used for setting up of galvanic cells.

Ans: Salt bridge is used in a galvanic cell for the following reasons:

(i) It maintains electrical neutrality in both half-cells by allowing the movement of ions.

(ii) It completes the electrical circuit, enabling the flow of current.

(iii) It prevents mixing of the solutions of the two half-cells.

(iv) It minimizes liquid junction potential, ensuring steady cell potential.

4. A galvanic cell is made in which the following reaction occurs.

Fe(s) + CuSOu(aq) → FeSou(aq) + Cu(s)

Write down the cell notation, for this cell.

Ans: Fe(s) | Fe SO₄(aq) || CuSO₄(aq) | Cu(s)

5. Predict whether the following reaction is feasible or not?

Cu(s) + Zn²⁺(aq) → Cu²⁺(aq) + 2n(s)

Ans: In feasible since E° = –1.10 V