The following initial rate data are for the reaction of mercury(II) chloride with oxalate ion:  2 HgCl2 + C2 O4 -2 ----> 2Cl + Hg2 Cl2 + 2 CO2   Experiment [HgCl2]0, M [C2 O4 -2]0, M Initial Rate, M* s-1 1 0.211 0.539 0.000569 2 0.422 0.539 0.00114 3 0.211 1.08 0.00228 4 0.422 1.08 0.00457 Complete the rate law for this reaction in the box below. Use the form , k [A]m [B]m 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 =  k =  M-2 * s-1

Write the general formula for calculating the average rate based on the disappearance of thiosulfate (S2O32-) in the following reaction:                  I31-(aq) + 2 S2O32-(aq) ----> 3 I1-(aq) + S4O62-(aq)

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The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH4+NO₂ → N₂ + 2 H₂O Experiment [NH4+]o, M [NO₂ ]o, M Initial Rate, M. s-1 0.0358 1.45 x 10-6 0.0715 0.0358 0.0715 1 2 3 4 Rate = 0.128 0.128 0.255 0.255 Complete the rate law for this reaction in the box below. Use the form k[A]" [B]", 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. k = 2.89 x 10-6 2.88 x 10-6 5.76 x 10-6 M-1.s-1

Question number 2

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 0.113 3.10×10-2 1.81×10-4 2 0.226 3.10×10-2 3.63×10-4 3 0.113 6.20×10-2 7.25×10-4 4 0.226 6.20×10-2 1.45×10-3 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 =   k_____ From these data, the rate constant is ______M-2s-1.

The following initial rate data are for the reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution: OCr +I- OI + CI Experiment [OCI"]o, M , M Initial Rate, Ms™ -1 1.70×10-3 1.70×10-3 3.40x10-3 3.40x10-3 4.57×10-3 9.15×10-3 4.57x10-3 9.15×103 1 5.41x10-4 1.08×10-3 1.08×10-3 2.17x10-3 2 3 4 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]" , 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's.

The following initial rate data are for the reaction of UO,* with hydrogen ion in aqueous solution: 2 UO,* + 4 H*u* + UO,2* + 2 H,0 Experiment [UO,l,, M |[н"), м Initial Rate, M s! 2.43x10-3 9.70x10 3 4.85x10-3 1.94x10-2 4.36x10-3 8.72x103 0.886 0.886 4.36x10-3 1.77 14 8.72x103 1.77 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]", 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 м?1

A reaction is performed to study the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: AsO 3³ +2 Ce4+ + H₂OAsO4³- + 2 Ce³+ +2 H+ The following reaction rate data was obtained in four separate experiments. Experiment 1 2 3 4 [AsO 3³¹10, M 3.80×10-2 7.60×10-2 3.80×10-2 7.60×10-2 [Ce4+]o, M 0.590 0.590 1.18 1.18 Initial Rate, Ms-1 6.64x10-3 1.33x10-2 2.66x10-2 5.31-10-2 The reaction is zero order with respect to water a) What is the order with respect to AsO3³- and Ce4+ b) What is the value of k (include units) *Show all your work.

The reaction between bromate ions and bromide ions in acidic aqueous solution is given by the following equation: BrO3- (aq) + 5Br- (aq) + 6H+ (aq) --> 3Br2 (l) + 3H2O (l) The experimental results are given below. Experiment Initial  [BrO3-] Initial  [Br-] Initial  [H+] Initial Rate  (M s-1) 1 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.20 0.20 0.10 3.2 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 Using these data, determine the orders for all reactants, the overall reaction order, and the value of the rate constant.