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KCET Chemical Kinetics — practice questions

Explore 48 free Chemical Kinetics questions in KCET Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Chemical Kinetics questions and exercises with answers

Showing questions 1–30 of 48.

Rate of reaction is defined as:Read the answer and worked solution →Rate law: r = k [A]ᵐ [B]ⁿ. Sum m + n is called:Read the answer and worked solution →For a first-order reaction, rate ∝:Read the answer and worked solution →Units of rate constant k for a first-order reaction:Read the answer and worked solution →Arrhenius equation: k = A × e^(-Ea/RT). What is A?Read the answer and worked solution →For first-order reaction, half-life t₁/₂:Read the answer and worked solution →For zero-order reaction A → P, rate equals:Read the answer and worked solution →For first-order, integrated rate law:Read the answer and worked solution →For second-order reaction (single reactant), integrated rate law:Read the answer and worked solution →Catalyst affects:Read the answer and worked solution →Order of reaction CAN be determined from:Read the answer and worked solution →A first-order reaction is 25% complete in 20 min. Time for 75% completion:Read the answer and worked solution →For a reaction with Ea = 100 kJ/mol, find k₂/k₁ when T goes from 300 K to 350 K. (R = 8.314 J/mol K):Read the answer and worked solution →For a 2nd-order reaction with [A]₀ = 0.5 M and k = 0.1 L mol⁻¹ s⁻¹, half-life:Read the answer and worked solution →For complex reaction with rate-determining step that involves 2 molecules of A, the order in A is:Read the answer and worked solution →For Arrhenius plot of ln k vs 1/T, slope equals:Read the answer and worked solution →Threshold energy = Ea + average kinetic energy of reactants. If Ea = 50 kJ/mol and avg KE = 4 kJ/mol, threshold energy:Read the answer and worked solution →For reaction A → B with rate constant 10⁻³ s⁻¹ (first order), concentration after 1000 s if [A]₀ = 1 M:Read the answer and worked solution →A reaction has k = 0.05 s⁻¹. After how many seconds is 90% complete?Read the answer and worked solution →For radioactive decay (1st order), if 1/8 of initial nuclei remain, how many half-lives elapsed?Read the answer and worked solution →A catalyst lowers Ea from 100 kJ/mol to 75 kJ/mol at T = 300 K. Rate enhancement factor (R = 8.314 J/mol K):Read the answer and worked solution →For elementary bimolecular reaction 2 NO → products, rate law is:Read the answer and worked solution →Rule on these rate law claimsRead the answer and worked solution →Order or molecularity?Read the answer and worked solution →True or false: order and molecularityRead the answer and worked solution →Read the order off the rate lawRead the answer and worked solution →Complete the definition of orderRead the answer and worked solution →True or false: where a rate law comes fromRead the answer and worked solution →Instantaneous rate or average rate?Read the answer and worked solution →Match each symbol in the Arrhenius equation to its meaningRead the answer and worked solution →

Worked practice questions

Rate of reaction is defined as:

  1. Amount of product
  2. Change in concentration of reactant per unit time
  3. Total moles
  4. Velocity
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Correct answer: B. Change in concentration of reactant per unit time

Rate = -d[R]/dt = +d[P]/dt (concentration change per unit time). SI unit: mol L⁻¹ s⁻¹. Defined positive.

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Rate law: r = k [A]ᵐ [B]ⁿ. Sum m + n is called:

  1. Order of reaction
  2. Molecularity
  3. Stoichiometry
  4. Half-life
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Correct answer: A. Order of reaction

Order of reaction = sum of exponents of concentrations in the rate law. Determined experimentally, NOT from stoichiometry. Can be integer, fractional, or zero.

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For a first-order reaction, rate ∝:

  1. [A]⁰
  2. [A]¹
  3. [A]²
  4. [A]^0.5
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Correct answer: B. [A]¹

**First order:** rate = k[A]. **Examples:** radioactive decay, decomposition of H₂O₂. Half-life is constant (independent of initial concentration).

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More Chemistry topics

Chemical EquilibriumElectrochemistryCoordination CompoundsElectrochemical SeriesIdeal and Non-Ideal SolutionsIdeal SolutionsNon-Ideal SolutionsReactions in Aqueous Solution