The reaction rate of a reaction at 60 °C will be greater than at 30°C because _____

A) the higher temperature leads to greater surface area on solid or liquid reactants.

B) the reactants at 60°C will be moving with too great of a speed to collide effectively.

C) the activation energy will be lower at 60°C.

D) there is a greater proportion of reactants with the necessary kinetic energy to react.

E) there is a greater likelihood that the reactants will have the correct orientation to collide effectively.

2. Which of the following will decrease the rate of a reaction?

A) Removing a catalyst from the reaction.

B) Decreasing the temperature.

C) Decreasing the surface area of a solid reactant.

D) Decreasing the concentration of the reactants.

E) All of these will decrease the rate of a reaction.

3. For the reaction 2 A + 4 B → 2 C + 4 D, what is the absolute magnitude of the rate of change for [B] when [C] is increasing at 7.9 M/s?

4. What is the rate at which Br⁻(aq) disappears in the reaction below if the rate of disappearance of BrO₃⁻(aq) is 0.037 M/s?BrO₃⁻ + 5 Br⁻ + 6 H⁺ → 3 Br₂ + 3H₂O

5. What is the absolute magnitude of the rate of change for [NH₃] if the rate of change for [H₂] is 8.70 M/s in the reaction 2 NH₃(g) → N₂(g) + 3 H₂(g)?

6. For the reaction A(g) → B(g) + 4 C(g), what is the rate of pressure change for C if the pressure change for A is -0.200 atm/s?

7.The reaction A + 2B + C → Products has a rate law of Rate = k[A]²[B]. By what factor would the reaction rate change if [A] is tripled?

8. What is the rate for the second order reaction A → Products when [A] = 0.379 M? (k = 0.761 M⁻¹s⁻¹).

9. What is the rate for the zero order reaction A → Products when [A] = 0.200 M? (k = 7.83 M/min)

10. Using the information in the table, the rate law for the reaction 2 A(g) + B(g) → C(g) + D(g) is

A) Rate = k[A][B]

B) Rate = k[A]

C) Rate = k[A]²[B]

D) Rate = k[A][B]²

11. Consider the table of data collected for the reaction A → Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately.

12 Using the information in the table, the value of the rate constant for the reaction A(g) + 3 B(g) → C(g) + 2 D(g) is

A) 0.106 M⁻¹s⁻¹

B) 6.80 M⁻¹s⁻¹

C) 0.362 s⁻¹

D) 68 M⁻³ s⁻¹

E) 1.36 s⁻¹

13. Which one of the following changes could double the rate of the reaction 2 A(g) + B(g) + 3 C(g) → 3 D(g) + E(g) with the rate law Rate = k[A]²[C]?

A) double [A]

B) double [B]

C) double [C]

D) cut [A] in half

14. What is the rate law for the reaction A + B → C + D given the experimental data for four trials of initial rate?

A) Rate = k[A][B]

B) Rate = k[A]²[B]

C) Rate = k[A][B]²

D) Rate = k[A]³[B]²

E) Rate = k[A]²[B]³

15. What is the rate law for the reaction A → B if the rate constant, k, is 0.25 M⁻¹ s⁻¹ at 75°C?

A) Rate = 0.25 M⁻¹ s⁻¹[A]

B) Rate = 0.25 M⁻¹ s⁻¹[A]²

C) Rate = 4.0 M⁻¹ s⁻¹[A]²

D) Rate = 0.25 M⁻¹ s⁻¹[B]

E) Rate = 0.25 M⁻¹ s⁻¹[B]²

16. What is the overall reaction order for the following rate law:Rate = k[A][B][C]²

17. The reaction A + 2 B → C has the rate law rate = k[A][B]. By what factor does the rate of reaction increase when both [A] and [B] are doubled?

18. How long will it take for the concentration of A to decrease from 0.850 M to 0.263 for the reaction A → Products? (k = 0.0882 M⁻¹s⁻¹)

19. How long will it take for the concentration of A to decrease from 1.25 M to 0.215 for the second order reaction A → Products? (k = 1.52 M⁻¹min⁻¹)

20. The second order reaction A → Products takes 13.5 s for the concentration of A to decrease from 0.740 M to 0.213 M. What is the value of k for this reaction?

21. The zero order reaction A → Products takes 63.5 minutes for the concentration of A to decrease from 0.970 M to 0.223 M. What is the value of k for this reaction?

22. What is the concentration of A after 11.5 minutes for the reaction A → Products when the initial concentration of A is 0.750 M? (k = 0.0451 M⁻¹min⁻¹)

23. If a reaction is first order with a rate constant of 0.0450 s⁻¹, how much time is required for 55% of the initial quantity of reactant to be consumed?

24. What is the concentration of A after 50.9 minutes for the second order reaction A → Products when the initial concentration of A is 0.250 M? (k = 0.117 M⁻¹min⁻¹)

25. What is the rate constant of a first-order reaction if the half-life is 5.20 min?

26. What is the half-life for a particular reaction if the rate law is rate = (951 M⁻¹*min⁻¹)[A]² and the initial concentration of A is 0.250 M?

27. A first order reaction initially contains 3.70 × 10²⁰ molecules. If the reaction has a half-life of 20.0 minutes, how many molecules remain unreacted after 80.0 minutes?

28. If the first-order half-life of tritium (³H) is 12.26 years, what amount of time is necessary for it to lose 75% of its radioactivity?

29. The half-life for the second order reaction A → Products is 4.57 min. What is the value of the rate constant for the reaction if the initial concentration of A is 0.217?

30. The half-life for the zero order reaction A → Products is 276 s. What is the value of the rate constant for the reaction if the initial concentration of A is 0.847?

31. The initial concentration of a reactant in a first order reaction is 0.860 M. What will be its concentration after 3 half-lives have passed?