NEET UG · Chemistry

Chemical Kinetics

18 practice questions, each with the answer and an explanation.

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Random questions from this topic, one at a time. You see the answer and the explanation straight after each one.

All 18 questions

  1. For the gas-phase chemical reaction: N2(g) + 3 H2(g) -> 2 NH3(g), how is the rate of formation of ammonia (d[NH3]/dt) stoichiometrically related to the rate of disappearance of hydrogen (-d[H2]/dt)?
  2. What are the dimensional units of the rate constant (k) for a chemical reaction of overall order n = 0 (zero-order reaction)?
  3. How does the half-life (t1/2) of a zero-order reaction depend on the initial concentration of the reactant ([A]0)?
  4. A first-order chemical reaction has a rate constant k = 6.93 * 10^-3 s^-1. What time is required for the reaction to reach 99.9 percent completion?
  5. Why is the acid-catalyzed hydrolysis of ethyl acetate (CH3COOC2H5 + H2O -> CH3COOH + C2H5OH) classified as a pseudo-first-order reaction?
  6. In the Arrhenius equation, k = A * e^(-Ea / RT), what does the slope of a linear plot of ln k versus 1/T represent?
  7. For a chemical reaction, the rate constant at 310 K is exactly double the rate constant at 300 K (k310 / k300 = 2). Given R = 8.314 J K^-1 mol^-1 and ln 2 = 0.693, what is the approximate activation e…
  8. How does a positive chemical catalyst accelerate the rate of a chemical reaction according to transition state theory?
  9. In collision theory of chemical reactions, what two fundamental criteria must molecular collisions satisfy to produce a successful chemical transformation?
  10. For the multi-step reaction: 2 NO2(g) + F2(g) -> 2 NO2F(g), the proposed mechanism is:
    Step 1: NO2 + F2 -> NO2F + F (slow)
    Step 2: NO2 + F -> NO2F (fast)
    What is the experimentally observed rate law f…
  11. What is the overall order of a reaction whose rate law is experimentally determined to be: Rate = k [A]^(1/2) [B]^(3/2)?
  12. Why cannot the molecularity of an elementary chemical reaction ever be zero or a fractional number?
  13. For an exothermic chemical reaction where the activation energy of the forward reaction is 50 kJ/mol and the enthalpy change (ΔH) is -30 kJ/mol, what is the activation energy of the reverse reaction?
  14. What happens to the rate of a chemical reaction when the temperature is raised from 300 K to 310 K, assuming a typical temperature coefficient of 2.0?
  15. Why does the catalytic decomposition of gaseous ammonia on a hot platinum metal surface follow zero-order kinetics at high ammonia pressures?
  16. If the half-life of a radioactive isotope is 14 days, what percentage of the original sample activity remains undecayed after 56 days?
  17. In a first-order chemical reaction A -> Products, if the initial concentration of reactant A is doubled from 0.1 M to 0.2 M, what happens to the half-life (t1/2) and the initial rate of the reaction?
  18. In chemical kinetics, when plotting ln k versus 1/T according to the Arrhenius relationship, what is the slope of the resulting straight line?

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