A reaction is followed and found to have a rate constant of 3.36 times 10^4 M^-1

Question

A reaction is followed and found to have a rate constant of 3.36 times 10^4 M^-1s^-1 at 344 K and a rate constant of 7.69 M^-1 s^-1 at 219 K. Determine the activation energy for this reaction. 23.8 kJ/mol. 42.0 KJ/mol. 11.5 kJ/mol. 12.5 KJ/mol. 58.2 KJ/mol. Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H^+ + H_2O_2 H_2O^+ -OH (rapid equilibrium) H_2O^+ -OH + Br^- rightarrow HOBr + H_2O (slow) HOBr + H^+ + Br^- rightarrow Br_2 + H_2O (fast) What is the overall reaction equation for this process? 2H_2O^+ -OH + 2Br^- rightarrow H_2O_2 + Br_2 + 2H_2O 2H^+ + 2Br^- + H_2O_2 rightarrow Br_2 + 2H_2O 2H^+ + H_2O_2 + Br^- + HOBr rightarrow H_2O^+ -OH + Br_2 + H_2O H_2O^+ -OH + Br^- + H^+ rightarrow Br_2 + H_2O Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H^+ + H_2O_2 H_2O^+ -OH (rapid equilibrium) H_2O^+ -OH + Br^- rightarrow HOBr + H_2O (slow) HOBr + H^+ + Br^- rightarrow Br_2 + H_2O (fast) Which of the following rate laws is consistent with the mechanism? Ratc = k[H_2O_2][H^+]^2[Br^+] Rate = k [H_2O^+ -OH][Br^-] Rate = k[H_2O_2][H^+][Br^-] Rate = k[Br^-] Rate = k[HOBr][H^+][Br^-][H_2O_2] The reaction CH_3NC(g) rightarrow CH_3CN(g) is first-order with respect to methyl isocyanides, CH_3NC. If it takes 10.3 minutes for exactly one quarter of the initial amount of methyl isocyanides to react, what is the rate constant in units of min^-1? -0.135 min^-1 0.0279 min^-1 0.089 min^-1 0.135 min^-1 35.8 min^-1

Explanation / Answer

7. B

8. B

9. C

10. D

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