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![Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H + H2O2 H2O+-OH (rapid equilibrium) H2O+-OH + Br → HOBr + H2O (slow) HOBr + H+ + Br-→ Br2 + H2O (fast) Which of the following rate laws is consistent with the mechanism? A. Rate k[HO-OH][Br] B. Rate kHO2H ]Br] C. Rate kHOHTBr] D. Rate HOBr][H][Br][HO2] E. Rate K[Br] 5. At a particular temperature, N20s decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N205 is 1.0 × 1016 molecules cm3 what will be the concentration in molecules cm after 16.1 s? A) 2.4 × 1014 B) 3.3 × 10 C) 1.0 x 1016 D) 1.4 x 1014 E) 2.3 x 10-1 2NOBr→2N0+Br2 exhibits the rate law Rate-fNOBr]2=-A[NOBr] 6. The reaction where k = 1.0 × 10-5Mi s-1 at 25°C. This reaction is run where the initial concentration of NOBr (NOBrjo) is 0.11 M. What is one half-life for this experiment? B.9. 1x10s s C. 1.1 s D. 0.6×10-5s E. none of these A) 6.9 x10-4s](https://media.cheggcdn.com/media%2F379%2F37974718-54e7-44cf-b04d-d620e611a8ca%2Fimage)
Please answer but also explain all of them! Thank you!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? A. Rate = k[H_2O^+ – OH][Br^-] B. Rate = k[H_2O_2][H^+][Br^] C. Rate = k[H_2O_2][H^+]^2[Br^] D. Rate k[HOBr][H^+][Br^-][H_2O_2] E. Rate K[Br^] At a particular temperature, N_2O_5 decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N_2O_5 is 1.0 times 10^16 molecules/cm^3, what will be the concentration in molecules/cm^3 after 16.1 s? A) 2.4 times 10^14 B) 3.3 times 10^1 C) 1.0 times 10^16 D) 1.4 times 10^14 E) 2.3 times 10^-1 The reaction 2NOBr rightarrow 2NO + Br_2 exhibits the rate law Rate = k [NOBr]^2 = – Delta [NOBr]/Delta t where k = 1.0 times 10^-5 M^-1 s^-1 at 25 degree C. This reaction is run where the initial concentration of NOBr ([NOBr]o) is 0.11 M. What is one half-life for this experiment? A) 6.98 times 10^-4 s B.9. 1 times 10^5 s C. 1.1 s D. 0.6 times 10^-5s E. none of these
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