Use the References to access important values if needed for this question. The following initial rate data are for the reaction of UO2+ with hydrogen ion in aqueous solution: 2UO2+4HU++ UO22++ 2H2O Experiment [UO2] M [H] M Initial Rate, M. s¹ 0' 1 0.000748 0.664 0.0000628 2 0.00150 0.664 0.000252 3 0.000748 1.33 0.000126 4 0.00150 1.33 0.000506 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for mor n and concentrations taken to the zero power do not appear. Don't enter 1 for mor n. Rate= k= M-2 -1 S Submit Answer Retry Entire Group 1 more group attempt remaining

what is the activation energy? rate = r = k [I-]^1 [S2O82-]^1 Mixtures:             Temperatures (celsius):        Initial Rates: 1                                      21.9                               6.45 * 10-4 2                                     38.9                              3.54 * 10-4 3                                      2.4                               4.35 * 10-4

The initial rates listed in the following table were measured in methanol solution for the reactionC2H4Br2+3I−→C2H4+2Br−+I3−C2H4Br2+3I−→C2H4+2Br−+I3−   Experiment Initial [C2H4Br2][C2H4Br2] Initial [I−][I−] Initial Rate (M/s)(M/s) 1 0.127 0.102 6.45×10−56.45×10−5 2 0.343 0.102 1.74×10−41.74×10−4 3 0.203 0.125 1.26×10−41.26×10−4 What is the value of the rate constant and its units?

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.

Kinetic data were obtained on the aqueous reaction of hydrogen peroxide with iodide ion and H+. H2O2(aq) + 3 l-(aq) + 2 H+(aq) → 13-(aq) + 2 H2O(1) Exp. 1 [H₂0₂], M 0.010 [I], M 0.010 [H+], M 0.00050 Initial Rate, M/s 1.15 x 10-6 2 0.020 0.010 0.00050 4.60 x 10-6 3 0.010 0.020 0.00050 1.15 x 10-6 4 0.010 0.010 0.00100 2.30 x 10-6 Determine the rate law for the reaction: none of the answers are correct R = 2.3 M-2 S-1 [H2O2]2 [H+] R = 1.15 x 10-2 M-1 S-1 [H2O2]2 R = 0.0115 M-1 S-1 [H2O2] [-]

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

Use the previous example for the chemical reaction 2 HgCl₂(aq) + C₂O4²-(aq)→ 2 Cl(aq) + 2 CO₂ (g) + Hg₂Cl₂ (s) The following initial rates of reactions were determined for the reactant concentrations given: Experiment #[HgCl₂] 0.100 0.100 0.050 1 2 3 [C₂O4²-] 0.20 0.40 1.2 x 10-4 0.40 6.2 x 10-5 Initial rate (M/sec) 3.1 x 10-5 (a) Find the order of the reaction with respect to HgCl2₂. (b)Find the order of the reaction with respect to C₂04² (c)Write the rate law for this reaction. (d)Calculate the value for the rate constant based on the data for experiment #1 and provide the proper units.

O None of the above Question 13 Consider the table below: The reaction is: 2FCI + Hz F2 + 2HCI Which gives the following data: Trial Initial Concentration of Initial Concentration of Instantaneous FCI (M) H2 (M) Reaction Rate (M/s) 1 2.0 2.0 0.222 2. 2.0 4.0 0.888 3. 4.0 4.0 1.776 What would be the generalized rate equation for this reaction? OR-k(FCI (H2 OR=K[F2[HCJ* OR-K FCI[Hal3 OR=k(FCI[Ha] OR-k(F2 THCIY Question 14

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.