Class 10 Chemistry Chapter 16 Electrochemistry Test 4 – Board Pattern
Grade 10 Chemistry Electrochemistry Chapter 16
Prepare for your matric examinations with the Class 10 Chemistry Chapter 16 Electrochemistry Class Test 4, part of the Punjab Board 2027 Model Papers. This test is designed to help students revise important concepts, practise Chemistry questions, and assess their understanding of Electrochemistry according to their course syllabus. Students preparing for the Class 10 Chemistry Board Exam 2027 can use this Chapter 16 test for self-assessment, classroom practice, and exam preparation. Visit 786Times.com for more Class 10 Chemistry chapter tests, model papers, and educational resources.
Chapter Wise Class Test
NOTE: Four possible answers A, B, C and D to each question are given. The choice which you think is correct, fill that circle in front of that question with Marker or Pen ink. Cutting or filling two or more circles will result in zero mark in that question.
Which of the following statements is NOT correct about Zn-Cu electrochemical cell?
For metals like lead and nickel, if the halide solution is concentrated, then at the cathode:
Which product will be obtained at the anode when a concentrated solution of NaCl will be electrolysed?
The electrolyte used in the hydrogen-oxygen fuel cell is:
When a dilute aqueous solution of ZnCl2 is electrolysed which product you will get at the cathode?
The electrolytic tank used in electroplating is made of:
What is produced at the cathode in hydrogen-oxygen fuel cell?
Which metal is highest in the electrochemical series?
- i.
Why fuel cells are regarded as environment friendly?Fuel cells (e.g. H2–O2 cell) produce only water as the by-product. They give no smoke, CO2 or other harmful pollutants, so they do not pollute the environment.
- ii.
Why must lead (II) chloride be heated before electrolysis?Solid PbCl2 is an ionic compound whose ions are fixed in the crystal lattice and cannot move, so it does not conduct. On heating (m.p. about 501°C) it melts and Pb2+ and Cl− ions become free to move and carry current.
- iii.
Why corrosion becomes fast during rainy season?In the rainy season moisture and dissolved gases (O2, CO2) and salts are abundant. Water acts as an electrolyte and increases the conductivity for the electrochemical reactions of rusting, so corrosion speeds up.
- iv.
What is the colour of CuSO4 solution and why?It is blue. In water Cu2+ ions form hydrated complex ions, [Cu(H2O)4]2+, which absorb red-orange light and transmit blue light.
- v.
What is the function of a porous partition in a galvanic cell?It separates the two electrolyte solutions so they do not mix, while allowing ions to pass through. This completes the internal circuit and keeps both half-cells electrically neutral.
- vi.
Why is chromium plating done on copper or nickel plated iron?Chromium does not stick well on iron directly. A layer of copper or nickel gives a smooth, adherent base. The top chromium layer is hard, shiny and highly resistant to corrosion, so the article is both protected and decorative.
- Ionisation: PbCl2(l) → Pb2+ + 2Cl−
- At cathode (reduction): Pb2+ ions gain electrons. Pb2+ + 2e− → Pb(l) Molten grey lead collects at the bottom.
- At anode (oxidation): Cl− ions lose electrons. 2Cl− → Cl2(g) + 2e− Greenish-yellow chlorine gas is released.
- Overall reaction: PbCl2(l) → Pb(l) + Cl2(g)
