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3 half-lives → % remaining = 12.5%.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
k = 1/(20×0.3) ≈ 0.1667 L mol⁻¹ s⁻¹.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
New rate = 8 × initial rate.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
t = 0.05/(2.0×10⁻³) = 25 s.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
New rate = 4.5 × initial rate.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
Three molecules collide → molecularity = 3.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
Overall order = 1/2 + 3/2 = 2.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
t½ = 1/(0.1×0.2) = 50 min.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
Δ[C]/Δt = 2 × (0.12/3) = 0.08 mol L⁻¹ s⁻¹.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
New rate = k(3[A])([B]/3) = initial rate.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
3 half-lives → fraction remaining = 1/8.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
Overall order = 1/3 + 2/3 = 1.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
