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Which of the following statements are true about reaction mechanisms?I. A rate law can be written from the molecularity of the slowest elementary step.II. The final rate law can include intermediates.III. The rate of the reaction is dependent on the fastest step in the mechanism.IV. A mechanism can never be proven to be the correct pathway for a reaction.

In going from room temperature (25.0 °C) to 10 °C above room temperature, the rate of a reaction doubles. Calculate the activation energy for the reaction.

Iodine-123, used in thyroid therapy, has a half-life of 13.27 hours and follows first-order decay kinetics. How many half-lives are required for a 160 mg sample of iodine-123 to decay to 5.0 mg?

Which of the following statements are true about reaction mechanisms?I. A rate law can be written from the molecularity of the slowest elementary step.II. The final rate law can include intermediates.III. The rate of the reaction is dependent on the fastest step in the mechanism.IV. A mechanism can never be proven to be the correct pathway for a reaction.

Consider a reaction that occurs by the following mechanism:A + BC → AC + BAC + D → A + CDThe potential energy profile for this reaction is shown below. Intermediates occur at which reaction stages?

The following set of data was obtained by the method of initial rates for the reaction: 2 HgCl2(aq) + C2O42-(aq) → 2 Cl-(aq) + 2 CO2(g) + Hg2Cl2(s) What is the value of the rate constant, k?

Consider a reaction that occurs by the following one-step mechanism:A2 + B2 → 2 ABThe potential energy profile for this reaction is shown below. The energy of reaction, ΔE, is given by the difference in energy between which two reaction stages?

The following set of data was obtained by the method of initial rates for the reaction: 2 HgCl2(aq) + C2O42-(aq) → 2 Cl-(aq) + 2 CO2(g) + Hg2Cl2(s) What is the value of the rate constant, k?

Consider a reaction that occurs by the following one-step mechanism:A2 + B2 → 2 ABThe potential energy profile for this reaction is shown below. The energy of reaction, ΔE, is given by the difference in energy between which two reaction stages?

Consider the reactions of cadmium with the thiosulfate anion.                    Cd2+(aq) + S2O32–(aq)  ↔  Cd(S2O3)(aq)                           K1 = 8.3 x 103                   Cd(S2O3)(aq) + S2O32–(aq)  ↔  Cd(S2O3)22–(aq)          K2 = 2.5 x 102 What is the value for the equilibrium constant for the following reaction?                    Cd2+(aq) + 2S2O32–(aq)  ↔  Cd(S2O3) 22–(aq)