Question

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 O B. The reaction is first order in each of H2O2 and H2SO3, but of order -1 in H+ O C. The reaction is first order in H2O2 and of order -1 in H+ OD. The reaction is first order in each of H2O2 and H+ O E. The reaction is first order in each of H2O2 and H2SO3 and H+ Reset Selection

Answer 1

H₂SO3(g) + H22(g) → H₂SO4 (g) + H₂O(g) Step 1: H₂ SO 3 ² H SO3 +H+ ... Kl -- [1503] [H+] [hasaz] :: [1503] = k'[H2 Soz] -0) [H +1 (k'z eonstant) step 2; H202 +++ 3H3027. 1 k = [#39]+ (kl= constant) [H222][H+]" -- [H30, +7 – K"[H203][41] –61) Step 3% H₂O2 + + HSO3 H₂SO4+H₂O; slow As it is slow step, So the rate determining step Ý this. The rate Law for overall Reaction - a=k [H30₂ t] [HSO 3 ] (K= constant) putting the value of [#3024] & [ HS03] &K.K" [H202] [44] K'. [H2 S03] CH? Tee = K [H202] [H₂ 503] [kklk's constant ... The Ans ý - # The reaction is first order . in each of H2O2 and H2SO3 but cs Scapped würder o in Ht.