The initial rate of the reaction: BrO3(aq) + 5 Br(aq) + 8 H(aq) → 3 Br2 + H₂O has been measured at the reactant concentrations shown below: [BrO3] mol dm3 Trial 1 2 3 4 0.10 0.20 0.10 0.10 [Br] mol dm 3 0.10 0.10 0.20 0.10 [H*] mol dm-3 0. 0.10 0.10 0.10 0.20 a. Determine the rate equation and the value of k, with units. b. Determine the initial rate if all three concentrations are 0.20 mol dm³. Initial Rate (mol dm³ s¹) 8.0 x104 1.6 x103 1.6 x10³ 3.2 x10³

The following initial rate data are for the reaction of ICl with hydrogen:2 ICl + H2I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.438 0.105 9.37×10-3 2 0.876 0.105 1.87×10-2 3 0.438 0.209 3.71×10-2 4 0.876 0.209 7.42×10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = _______    From these data, the rate constant is __________M-2s-1.

Using the data in the table, calculate the rate constant of Trial [A] (M) [B] (M) Rate (M/s) this reaction. 1 0.260 0.280 0.0119 A + B → C+ D 2 0.260 0.784 0.0933 3 0.312 0.280 0.0143 Units k = M-²s-1 M-'s-! M-s-!

7 11 The initial rate of the reaction has been measured at the reactant concentrations show: Trial [BrO3] [H*] (mol/L) (mol/L) 0.10 0.10 0.20 0.10 0.10 0.20 0.10 0.10 1 23 3. 4 The rate law expression will be: [Br] (mol/L) 0.10 0.10 0.10 0.20 Initial rate (mol/L.s) 8.0 16 16 32

The following initial rate data are for the reaction of mercury(II) chloride with oxalate ion: 2 HgCl, + C,0,–→2 Cr + Hg,Cl, + 2 Co, [C,0,?1, M [HgCl2lo. M S.53x10-2 Experiment Initial Rate, M s-! 0.378 1.26x10-4 2 0.171 0.378 2.52x104 3 S.53x10-2 0.756 5.02x10-4 4 0.171 0.756 1.01x103 Complete the rate law for this reaction in the box below. Use the form k[A]"|B}", where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is

Using the data in the table, calculate the rate constant of Trial [A] (M) [B] (M) Rate (M/s) this reaction. 0.210 0.320 0.0239 A + B → C + D 2 0.210 0.832 0.162 3 0.252 0.320 0.0287 Units k = м-2s-1

The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI + H Iz + 2 HCI Initial Rate, Ms! 1.57x10-2 3.13×10-2 6.24x10-2 0.125 Experiment [ICI]. M H), M 1 0.207 0.211 2 0.414 0.211 3 0.207 0.421 4 0.414 0.421 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is