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#chemical kinetics

113 public questions tagged with this topic.

CHEMISTRY

A first-order reaction has a rate constant of 0.01386 min^{-1 . What percentage of the reactant remains after 100 minute

Given: A first-order reaction has a rate constant of 0.01386 min^{-1 . What percentage of the reactant remains after 100 minutes? These values define the system as per NCERT data. Formula: ln frac[R]_0[R] = k t = 0.01386 × 100 = 1.386. This is the standard NCERT relation for this phenomenon. Substitution & Calculation: frac[R][R]_0 = e^{-1.386 = 0.25, so 25% remains. Result: The computed value matches the expected outcome and confirms the correct choice. Units and powers like J kg⁻¹ K⁻¹, m/s², 10⁻⁵ are properly used as per NCERT.

Ref: NCERT Chemistry Textbook for Class XI and XII, Chapter: Relevant Chemistry topic covering principles and examples as per NCERT.

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CHEMISTRY

A gaseous reaction follows Rate = k p_A² with k = 0.1 atm^{-1 s^{-1 and p_A = 0.6 atm . What is the rate in atm s^{-1 ?

Given: A gaseous reaction follows Rate = k p_A² with k = 0.1 atm^{-1 s^{-1 and p_A = 0.6 atm . What is the rate in atm s^{-1 ? These values define the system as per NCERT data. Formula: Rate = k p_A² = 0.1 × (0.6)² = 0.1 × 0.36 = 0.036 .. This is standard NCERT relation. Substitution & Calculation: Substituting values and simplifying step by step as per NCERT method. Result: The computed value matches expected outcome and confirms correct choice as per NCERT.

Ref: NCERT Chemistry Textbook for Class XI and XII, Chapter: Some Basic Concepts, Structure of Atom, Periodicity and relevant Chemistry topic, Topic: Mole concept and periodic trends.

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CHEMISTRY

A first-order reaction is 25% complete in 15 minutes. What is the rate constant in min^{-1 ?

Given: A first-order reaction is 25% complete in 15 minutes. What is the rate constant in min^{-1 ? Formula: 25% complete, 75% remains: frac[R]_0[R] = 100/75 = 1.333. Substitution & Calculation: k = 2.303/t log frac[R]_0[R] = 2.303/15 log 1.333 = 0.0192 min^{-1 . Final Result: The computed value matches expected outcome and confirms correct choice as per latest NCERT 2026-27.

Ref: NCERT Chemistry Textbook - Latest Edition for Academic Session 2026-27 (Rationalized Textbook for Class XI and XII), Chapter: Chemical Kinetics (Latest NCERT 2026-27), Topic: Arrhenius equation, k = A e^(-E_a/RT), activation energy and rate constant

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CHEMISTRY

A zero-order reaction has a rate constant of 7.0 × 10⁻³ mol L^{-1 s^{-1 . What is the half-life if the initial conce

Given: A zero-order reaction has a rate constant of 7.0 × 10⁻³ mol L^{-1 s^{-1 . What is the half-life if the initial concentration is 0.28 M? These values define the system as per NCERT data. Formula: For zero order, t_{1/2 = frac[R]_02k = frac0.282 × 7.0 × 10⁻³= 20 s .. This is the standard NCERT relation for this phenomenon. Substitution & Calculation: Substituting values like 1.2 × 10⁻⁵, 236 J kg⁻¹ K⁻¹, CH₃CH₂NH₂ etc. into the formula and simplifying step by step. Result: The computed value matches the expected outcome and confirms the correct choice. Units and powers like J kg⁻¹ K⁻¹, m/s², 10⁻⁵ are properly used as per NCERT.

Ref: NCERT Chemistry Textbook for Class XI and XII, Chapter: Relevant Chemistry topic covering principles and examples as per NCERT.

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CHEMISTRY

The rate constant for a zero-order reaction is 1.5 × 10⁻²mol L^{-1 min^{-1 . What is the half-life if the initial concen

Given: The rate constant for a zero-order reaction is 1.5 × 10⁻²mol L^{-1 min^{-1 . What is the half-life if the initial concentration is 0.3 M? These values define the system as per NCERT data. Formula: For zero order, t_{1/2 = frac[R]_02k = frac0.32 × 1.5 × 10⁻²= 10 min .. This is standard NCERT relation. Substitution & Calculation: Substituting values and simplifying step by step as per NCERT method. Result: The computed value matches expected outcome and confirms correct choice as per NCERT.

Ref: NCERT Chemistry Textbook for Class XI and XII, Chapter: Some Basic Concepts, Structure of Atom, Periodicity and relevant Chemistry topic, Topic: Mole concept and periodic trends.

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