The following initial rate data are for the **reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution**:\[ \text{OCl}^- + \text{I}^- \rightarrow \text{OI}^- + \text{Cl}^- \]| Experiment | $[\text{OCl}^-]_0$, M | $[\text{I}^-]_0$, M | Initial Rate, Ms$^{-1}$ ||------------|-------------------------|----------------------|--------------------------|| 1 | $1.70 \times 10^{-3}$ | $4.57 \times 10^{-3}$ | $5.41 \times 10^{-4}$ || 2 | $1.70 \times 10^{-3}$ | $9.15 \times 10^{-3}$ | $1.08 \times 10^{-3}$ || 3 | $3.40 \times 10^{-3}$ | $4.57 \times 10^{-3}$ | $1.08 \times 10^{-3}$ || 4 | $3.40 \times 10^{-3}$ | $9.15 \times 10^{-3}$ | $2.17 \times 10^{-3}$ |**Complete the rate law for this reaction in the box below.** Use the form $ \text{k[A]}^m[\text{B}]^n $, where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n.Rate = \_\_\_\_**From these data, the rate constant is \_\_\_\_ M$^{-1}$s$^{-1}$.**

The rate law is used to express the relation between the rate of a reaction and the concentration of…

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 [ocr], M [1],, M Initial Rate, Ms 1 1.70x10-3 4.57×10-3 5.41x10-4 2 1.70×10-3 9.15x10-3 |1.08×10-3 3 3.40x10-3 4.57×10-3 1.08×10-3 4 3.40x10-3 9.15×10-3 2.17×10-3 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 M's1.

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 [ocr], M [1],, M Initial Rate, Ms 1 1.70x10-3 4.57×10-3 5.41x10-4 2 1.70×10-3 9.15x10-3 |1.08×10-3 3 3.40x10-3 4.57×10-3 1.08×10-3 4 3.40x10-3 9.15×10-3 2.17×10-3 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 M's1.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

consider the reaction of S20,- with I, in agne ons solution: 2. 2 At a given temp. the rate of disa ppearance of ' S,0? varies with reactnnt concentrafions in the following manner: experiment [S,0% (M) [I-](M) Rate (MIB) 0.034 2.6 0.018 0-027 0-03p 3.0 3 10- 10-6 0.034 0.054 7-8 Us 4. 0.050 0-072 l.4 10 5. Aenmime
The following initial rate data are for the reduction of nitric oxide with hydrogen: ... 2 NO + 2 HzN2 + 2 H2O Experiment NO],, M [H]o, M Initial Rate, M s 8.66x10-2 1 0.370 0.408 2 0.740 0.370 0.740 0.408 0.816 0.346 0.173 0.693 3 0.816 From these data, what is the rate constant in M?s1 (A) 2.55 B) 1.55 (c) 3.55 D) 4.55
alfa +O M 1.1 K/s & “l| 55 1 2:11 PM О 10 Which of the following units correspond (s) to the rate constant k of a second order reaction? (check all that apply) k (M-1 min-1) k (M-1 s-1) k (M-2 min-1) k (M-2) k (M-2 s-1)
Question 5 of 5 Macmillan Learning > For the reaction A-products, concentration and time data were collected. Insert these data into the graphing tool to determine the order of the reaction and the value of [A]o- Graphing Tool [A] In[A] Clear All Data 1/[A] M (A) Al vs. t (min) 5.0 10.0 15.0 20.0 25.0 In A) vs. 1/[A] vs. t [A] (M) 0.938 0.583 0.423 0.331 0.273
Please ? thank you ?
Pls help ASAP.
Pls help ASAP on all ASKED QUESTIONS PLS PLS
Determine the order with respect to DER
2. Consider the reaction A+2B C whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: [v] (M) (M) (M/s) [B] Rate Trial 1 0.10 0.050 6.0x10-4 0.10 0.100 1.2x10-3 3 0.20 0.050 2.4x10-3 Part B Provide
tab 11:36 AM Thu Feb 23 < aps lock Tap here or pull up for additional resources What is the half-life for a particular reaction if the rate law is rate= (1261 M-¹*min-¹) [A]² and the initial concentration of A is 0.250 M? ! 1 Q A N 2 W S X #3 E D $ 4 R TI F de 5 % V T G 6 ... Question 9 of 26 Y & 1% 7 H U : 8 00 J I ( 9 = K 1 4 7 +/- -0 0 V L P
please help
For a first-order reaction k A + B time t = 0 s 4.878 1.004 M time t = 19.84 s ? M when k = 0.030329 s-1 what is the concentration of B above in the question mark= _M? 3 sig. fig. normal format. Try to plot concentrations of A, B and rate over time in Excel.