11 public questions tagged with this topic.
3 half-lives → fraction remaining = 1/8 = 12.5%.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Temperature Dependence - Arrhenius Equation and Activation Energy
t = (0.25 − 0.1)/(5.0×10⁻³) = 30 min.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Rate of Reaction - Average and Instantaneous Rate and Rate Law
t = (2.303/0.0173) log 5 ≈ 93 min.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Pseudo First Order and Complex Reactions
k = (0.15 − 0.06)/90 = 1.0 × 10⁻³ mol L⁻¹ s⁻¹.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Pseudo First Order and Complex Reactions
k = 0.693/40. t₉₀ = (2.303/k) log 10 ≈ 133 min.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Pseudo First Order and Complex Reactions
k = 0.693/12 ≈ 0.05775 min⁻¹. For 90% completion t = (2.303/k) log 10 ≈ 40 min.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Pseudo First Order and Complex Reactions
t = (0.1 − 0.06)/(2.0×10⁻³) = 20 min.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Order and Molecularity and Units of Rate Constant
t = (0.16 − 0.04)/(8.0×10⁻⁴) = 150 s.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Order and Molecularity and Units of Rate Constant
t = (1/0.05 − 1/0.25)/0.07 ≈ 228.57 s.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Order and Molecularity and Units of Rate Constant
t = [R]₀/k = 0.08/(4.0×10⁻⁴) = 200 s.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Integrated Rate Equations - Zero Order Reactions
t = ([R]₀ − [R])/k = (0.18 − 0.12)/(6.0×10⁻³) = 10 min.
Ref: NCERT Class 12 Chemistry > Chapter 3: Chemical Kinetics > Topic: Collision Theory - Effective Collisions and Catalyst Effect
