Help Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous...
Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+ + H202 = H207-OH (rapid equilibrium) H207-OH + Br- → HOBr + H20 (slow) HOBr + H+ + Br + Br2 + H20 (fast) What is the overall rate of reaction?
Consider the three step reaction mechanism for the atmospheric oxidation in clouds of sulfurous acid to sulfuric acid by hydrogen peroxide H2SO3(9)+ H2O2(9)- H2SO4(9)+ H20(9) Step 1: H2SO3 = HSO3+H* fast Step 2: H202 + H+ = H302 fast Step 3: H302* + HSO3 + H2SO4+H20 slow Which of the following is correct concerning the rate law for the overall reaction? O A. The reaction is first order in each of H2O2 and H2SO3, but of order 0 in H...