17 public questions tagged with this topic.
Chlorobenzene undergoes electrophilic substitution with Cl₂ and FeCl₃ , forming 1,4-dichlorobenzene ( C₆H₄Cl₂ ) as the major product (para).
Ref: NCERT Class 12 Chemistry > Chapter 6: Haloalkanes and Haloarenes > Topic: Classification and Nomenclature and Isomerism of Haloalkanes
Chlorination of pentane favors the secondary position (C₂/C₄) due to stability, forming CH₃CHClCH₂CH₂CH₃ (2-chloropentane) as the major product.
Ref: NCERT Class 12 Chemistry > Chapter 6: Haloalkanes and Haloarenes > Topic: Classification and Nomenclature and Isomerism of Haloalkanes
E°cell = 1.36 - 0.34 = 1.02 V . Ecell = 1.02 - (0.059/2) log ([Cu²⁺][Cl⁻]²/PCl_₂) = 1.02 - 0.0295 log (0.01 × 0.0025/0.5) = 1.02 + 0.053 = 1.073 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant
Let Cl = x. O = -2. Equation: 2x + 7(-2) = 0, 2x - 14 = 0, x = +7.
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Redox Titrations and Equivalent Weight and Normality
The reducing agent is oxidized. Fe (0) loses electrons to become Fe (+3) in FeCl₃, reducing Cl₂.
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Redox Titrations and Equivalent Weight and Normality
Let Cl = x. H = +1, O = -2. Equation: +1 + x + 4(-2) = 0, 1 + x - 8 = 0, x = +7.
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Oxidizing and Reducing Agents and Strength
The reducing agent is oxidized. Cl (0 in Cl₂) becomes +5 in NaClO₃ and -1 in NaCl; Cl₂ reduces itself.
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Oxidizing and Reducing Agents and Strength
Cl₂ (0) gains electrons to become Cl− (-1), oxidizing I− to I₂.
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Oxidizing and Reducing Agents and Strength
Cl₂ (0) is reduced to -1 in KCl, oxidizing Br (-1 to 0).
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Oxidizing and Reducing Agents and Strength
Oxidation involves electron loss. S (-2 in H₂S) becomes 0 in S, losing electrons.
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Electrode Potential and Electrochemical Series and Galvanic Cells
Let Cl = x. O = -2. Equation: x + 2(-2) = 0, x - 4 = 0, x = +4.
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Classical and Electronic Concept of Redox and Oxidation Number
Let Cl = x. K = +1, O = -2. Equation: +1 + x + 3(-2) = 0, 1 + x - 6 = 0, x = +5.
Ref: NCERT Class 11 Chemistry > Chapter 7: Redox Reactions > Topic: Classical and Electronic Concept of Redox and Oxidation Number
