Half lives, Arrhenius theory, activation energy, collision theory for bimolecular gaseous reactions - One Line Questions

1. The activation energy of a reaction is 100 kJ/mol. At what temperature will the rate constant be approximately equal to the pre-exponential factor A? — Approx. 1200 K
2. The half-life of a reaction is 50 years. If it is a first-order reaction, what fraction of the substance will remain after 100 years? — 1/4
3. If the half-life of a reaction is 't', then after 2t, the remaining amount of reactant for a first-order reaction will be: — 1/4 of the initial amount
4. The half-life of a reaction is the time required for the concentration of a reactant to reduce to: — 1/2 of its initial value
5. For a second-order reaction where Rate = k[A]^2, if the initial concentration of A is doubled, the rate of reaction will increase by a factor of: — 4
6. For a bimolecular reaction, the rate law is Rate = k[A][B]. If the concentration of both A and B are doubled, the rate of reaction will increase by a factor of: — 4
7. If the half-life of a reaction is 10 minutes, and it is a first-order reaction, how much time will it take for the concentration to reduce to 1/8th of its initial value? — 30 minutes
8. If a reaction has a half-life of 20 minutes and is first order, how long will it take for 75% of the reactant to be consumed? — 40 minutes
9. The fraction of collisions that have energy equal to or greater than the activation energy is represented by which term in the Arrhenius equation? — e^(-Ea/RT)
10. In the Arrhenius equation, k = A * e^(-Ea/RT), what does 'A' represent? — Frequency factor or pre-exponential factor
11. In collision theory for bimolecular gaseous reactions, 'Zab' represents: — Collision frequency per unit volume
12. Which theory explains the rate of bimolecular reactions based on the frequency of collisions between reactant molecules? — Collision theory
13. Which of the following factors affects the rate of a chemical reaction according to collision theory? — All of the above
14. The probability that a collision between reactant molecules leads to a reaction is known as the: — Steric factor or orientation factor
15. The collision theory states that the rate of a reaction is proportional to the frequency of collisions and the fraction of effective collisions. The fraction of effective collisions depends on: — Activation energy and orientation factor
16. For a zero-order reaction, the rate constant has the same units as: — Rate of reaction
17. The Arrhenius equation is most useful for determining the effect of which factor on the reaction rate? — Temperature
18. Which of the following is NOT a factor that influences the rate of a chemical reaction according to collision theory? — Color of reactants
19. According to the Arrhenius theory, what happens to the rate constant 'k' as temperature (T) increases? — Increases
20. What is the effect of increasing temperature on the collision frequency of gas molecules? — Increases
21. What is the half-life of a reaction if its rate is constant and does not depend on the concentration of reactants? — Remains constant
22. The half-life of a second-order reaction A + B -> Products is given by t1/2 = 1 / (k[A]0) if [A]0 = [B]0. If the initial concentration is doubled, the new half-life will be: — Halved
23. The rate of a reaction is independent of temperature if: — Ea is zero
24. The term 'Ea' in the Arrhenius equation stands for: — Activation energy
25. If the initial concentration of a first-order reaction is halved, its half-life will: — Remain the same
26. If the activation energy of a reaction is very high, the rate constant 'k' at a given temperature will be: — Low
27. The 'effective collisions' in collision theory refer to collisions that have: — Both sufficient energy and proper orientation
28. According to collision theory, increasing the concentration of reactants leads to: — Increased collision frequency
29. A catalyst increases the rate of a reaction by: — Decreasing the activation energy
30. For a zero-order reaction, the half-life is: — Directly proportional to the initial concentration
31. What is the half-life of a first-order reaction? — Independent of the initial concentration
32. Which of the following statements is true about activation energy? — It is the minimum energy required for a reaction to occur.
33. What is the relationship between the rate constant (k) and temperature (T) as described by Arrhenius equation? — k increases exponentially with T
34. What is the minimum energy required for reactant molecules to undergo a chemical reaction called? — Activation energy
35. The Arrhenius equation can be written in logarithmic form as: — ln k = ln A - (Ea/RT)
36. If the temperature is increased by 10°C, the rate of a reaction approximately doubles. This is a general observation for reactions with: — High activation energy
37. In the context of activation energy, the 'activated complex' or 'transition state' has: — Higher energy than reactants
38. For a bimolecular reaction, the rate law is generally expressed as: — Rate = k[A][B]
39. What is the unit of the rate constant for a second-order reaction? — L mol^-1 s^-1
40. The Arrhenius equation is given by k = A * e^(-Ea/RT). If we plot log k versus 1/T, we get a straight line with: — Slope = -Ea/2.303R and intercept = log A
41. In collision theory, for a reaction to occur, the colliding molecules must possess: — Both sufficient kinetic energy and proper orientation
42. For a second-order reaction, the half-life (t1/2) is related to the initial concentration ([A]0) as: — t1/2 ∝ 1/[A]0
43. The Arrhenius equation relates the rate constant (k) of a reaction to: — Temperature and activation energy
44. What does the term 'RT' in the exponent of the Arrhenius equation represent? — The thermal energy available to molecules
45. In collision theory, the steric factor (p) accounts for: — The probability of effective orientation during collision
46. The pre-exponential factor 'A' in the Arrhenius equation has the same units as: — The rate constant 'k'
47. The collision theory is most applicable to which type of reactions? — Bimolecular reactions
48. If the activation energy (Ea) is zero, the rate constant 'k' according to Arrhenius equation becomes: — A
49. For a reaction A + B -> Products, if the rate law is Rate = k[A][B], what is the order of the reaction? — Second
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