Redox Reactions – Balancing, Half-Reaction Method, Electrochemical Cells
Chemistry · Grade 11 · Week 23 · 25 questions
In Grade 11 chemistry, Redox Reactions builds your grasp of Balancing, Half-Reaction Method, and Electrochemical Cells. These fundamentals show up repeatedly in NCERT exemplar problems and board questions.
What you'll practise
- Identify Balancing
- Explain Half-Reaction Method
- Identify Electrochemical Cells
- Apply redox reactions concepts to NCERT exercise and exemplar problems
All 25 questions in this Redox Reactions – Balancing, Half-Reaction Method, Electrochemical Cells quiz
Grade 11 Chemistry — Redox Reactions – Balancing, Half-Reaction Method, Electrochemical Cells: 25 practice questions with instant scoring and explanations.
- In oxidation number method, first balance:
- In half-reaction method for acidic solution, balance O by adding:
- In half-reaction method for acidic solution, balance H by adding:
- In basic solution, after balancing as acidic, add OH⁻ to:
- Balance Fe²⁺ + MnO₄⁻ + H⁺ → Fe³⁺ + Mn²⁺ + H₂O. Fe²⁺ coef =
- Electrons lost by reducing agent =
- Galvanic cell converts:
- Daniell cell: Zn | Zn²⁺ || Cu²⁺ | Cu. Anode is:
- Cathode in Daniell cell:
- EMF of Daniell cell ~
- Salt bridge maintains:
- Standard hydrogen electrode E° =
- Standard electrode potential of Zn²⁺/Zn:
- Standard electrode potential of Cu²⁺/Cu:
- E°_cell =
- ΔG° =
- F (Faraday constant) =
- Nernst equation at 298 K:
- At equilibrium, E_cell =
- Higher E° means:
- Most powerful oxidizing agent from list:
- Most powerful reducing agent:
- Electrolysis of molten NaCl produces:
- Faraday's first law: mass deposited ∝
- Equivalent mass in electrolysis =
Question 1 of 250 correct so far