Which equation best describes the average rate for the reaction shown? A(aq) + B(aq) → C(aq) + D(aq) Orate = +A[B]/At [A][B] rate= [CD] O rate = -A[A]/At O rate = [CD] AB O rate =A[C]/At

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Rate = k[HOOBr][HBr] Rate = k[HBr][O21 QUESTION 6 The following questions are based on the reaction and data below. Chlorine dioxide is a reddish yellow gas that dissolves in water. In basic solution this reaction takes place: 2CIO 2(aq) + 20H (aq) → CIO 2 (aq) + CIO 3 (aq) + H2O(). Based on the following data, determine the rate law and the value of the rate constant. Initial Concentrations Initial Rate [CIO2] [OH] (M/s 0.060 0.030 0.0248 0.020 0.030 0.00276 0.020 0.090 0.00828 What is the order of the reaction with respect to HO? Second order First order Zero order O Fourth order QUESTION 7

2 NO(g) + Br2 (g) → 2 NOB1(g) Initial Rate Experiment NO] (M) [Br2] (M) (mol/L's) 1 1.0 x 10-2 2.0 × 10-2 2.4 x 10-2 2 4.0 x 10-2 2.0 × 10-2 0.384 3 1.0 x 10-2 6.0 x 10-2 7.2 x 10-2 What is the order of the reaction with respect to [NO] and [Br2], and what is the overall order of the reaction? Order with respect to [NO] = Order with respect to [Br2] = Overall order

R=K [A] [B] ----; 2. The initial rate of the reaction: BrO3(aq) + 5 Br (aq) + 8 H*(aq) Has been measured at the reactant concentrations shown (in mol/L): Trial [BrO3] [Br] [H*] 1 0.10 0.10 0.10 2 0.20 0.10 0.10 3 0.10 0.20 0.10 4 0.10 0.10 0.20 A) Determine the rate law equation including the k value. Determine the order of reaction for BrO3, Br, and H* Rate law 3 Br₂(l) + H₂O(l) Initial rate (mol/Ls) 8.0 x 104 1.6 x 10³ 1.6 x 10°³ 3.2 x 10'³

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Write a balanced reaction for which the following rate relationships are true. Rate (A[NO]/At) = - (1/2)(A[HNO3]/At) = (A[H₂O]/At) = (1/3)(A[NO₂]/At) No +해 + + HNO3 H₂O 1 NO₂ 6 NO3HNO3 6H 20 + 2NO₂ If the rate of disappearance of NO in the reaction in #1 is 0.270 M s-1 at 150°C, the rate of appearance of NO3 is. What is the overall order of the reaction in #1, if given is the rate law? Rate = k[NO]2 [HNO3]³ Ms-1 Given the above rate law, how does the rate of reaction change if the concentration HNO3 is doubled? ANSWER:

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help w this question plz

Given the following balanced equation, determine the rate of reaction with respect to [NOCl]. 2 NO(g) + Cl2(g) → 2 NOCl(g) A) Rate = - 1∆[NO]/ 2∆t B) Rate = - 2∆[NOCl] / ∆t C) Rate = + 1∆[NOCl] / 2∆t D) Rate = - 1∆[NOCl] / 2∆t E) It is not possible to determine without more information