The reaction, CO2(aq) + 2 OH "(aq) --> CO32- (aq) + H20(1), proceeds through the following mechanism: CO2(aq) + OH -(aq) -- --> HCO3 (aq) HCO3- (aq) + OH "(aq) --> CO32-(aq) + H20(1) > The first step of this mechanism is rate-determining (slow). What would the rate law for this reaction be if the second step were rate-determining? O a) Rate = k [OH ] [CO2]1/2 O b) Rate = k [OH - ]? [CO2] O c) Rate = k [OH-]1/2 [CO2] od) Rate = k [OH-] [CO2] e) Rate = k [OH-]? [CO2]1/2 The reaction, 2 NO(g) + 2 H2(g) --> N2(g) + 2 H2O(g), proceeds through the following mechanism: 2 NO(g) --> N2O2(g) N2O2(g) + H2(g) --> H2O(g) + N2O(g) N2O(g) + H2(g) --> N2(g) + H2O(g) The second step of this mechanism is rate-determining (slow). What would the rate law for this reaction be if the first step were rate-determining? a) Rate = k [NO]2 Ob) Rate = k [NO]1/2 [H2] O c) Rate = k [NO]2 [Hz]1/2 d) Rate = k [NO]2 [H2] Oe) Rate = k [NO] [H2]1/2 . The reaction, 4 HBr(g) + O2(g) --> 2 H2O(g) + 2 Br2(g), proceeds through the following mechanism: HBr(g) + O2(g) --> HOOBr(g) HOOBr(g) + HBr(g) --> 2 HOBr(g) HOBr(g) + HBr(g) --> Br2(g) + H2O(g) The first step of this mechanism is rate-determining (slow). What would the rate law for this reaction be if the third step were rate-determining? a) Rate = k [HBr]2 [02]1/2 b) Rate = k [HBr] [02] c) Rate = k [HBr]1/2 [02] d) Rate = k [HBr] [02]1/2 e) Rate = k [HBr]2