Half lives, Arrhenius theory, activation energy, collision theory for bimolecular gaseous reactions - Question Bank
1. 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?
2. In collision theory, the steric factor (p) accounts for:
3. The Arrhenius equation is most useful for determining the effect of which factor on the reaction rate?
4. 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:
5. 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?
6. 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?
7. Which of the following is NOT a factor that influences the rate of a chemical reaction according to collision theory?
8. 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:
9. 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:
10. In the context of activation energy, the 'activated complex' or 'transition state' has:
11. What is the relationship between the rate constant (k) and temperature (T) as described by Arrhenius equation?
12. The half-life of a reaction is the time required for the concentration of a reactant to reduce to:
13. For a zero-order reaction, the rate constant has the same units as:
14. According to collision theory, increasing the concentration of reactants leads to:
15. 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:
16. If the half-life of a reaction is 't', then after 2t, the remaining amount of reactant for a first-order reaction will be:
17. The 'effective collisions' in collision theory refer to collisions that have:
18. For a reaction A + B -> Products, if the rate law is Rate = k[A][B], what is the order of the reaction?
19. The rate of a reaction is independent of temperature if:
20. What is the effect of increasing temperature on the collision frequency of gas molecules?
21. If the initial concentration of a first-order reaction is halved, its half-life will:
22. In collision theory for bimolecular gaseous reactions, 'Zab' represents:
23. The Arrhenius equation can be written in logarithmic form as:
24. Which of the following statements is true about activation energy?
25. 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:
26. If the activation energy (Ea) is zero, the rate constant 'k' according to Arrhenius equation becomes:
27. The probability that a collision between reactant molecules leads to a reaction is known as the:
28. The collision theory is most applicable to which type of reactions?
29. What is the half-life of a reaction if its rate is constant and does not depend on the concentration of reactants?
30. If the temperature is increased by 10°C, the rate of a reaction approximately doubles. This is a general observation for reactions with:
31. What does the term 'RT' in the exponent of the Arrhenius equation represent?
32. For a bimolecular reaction, the rate law is generally expressed as:
33. The pre-exponential factor 'A' in the Arrhenius equation has the same units as:
34. If the activation energy of a reaction is very high, the rate constant 'k' at a given temperature will be:
35. Which of the following factors affects the rate of a chemical reaction according to collision theory?
36. A catalyst increases the rate of a reaction by:
37. What is the unit of the rate constant for a second-order reaction?
38. For a second-order reaction, the half-life (t1/2) is related to the initial concentration ([A]0) as:
39. The fraction of collisions that have energy equal to or greater than the activation energy is represented by which term in the Arrhenius equation?
40. In collision theory, for a reaction to occur, the colliding molecules must possess:
41. Which theory explains the rate of bimolecular reactions based on the frequency of collisions between reactant molecules?
42. What is the minimum energy required for reactant molecules to undergo a chemical reaction called?
43. According to the Arrhenius theory, what happens to the rate constant 'k' as temperature (T) increases?
44. The term 'Ea' in the Arrhenius equation stands for:
45. In the Arrhenius equation, k = A * e^(-Ea/RT), what does 'A' represent?
46. The Arrhenius equation relates the rate constant (k) of a reaction to:
47. 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?
48. For a zero-order reaction, the half-life is:
49. What is the half-life of a first-order reaction?