3. Chlorineoxide(CIO),whichplaysanimportantrole in the depletion of ozone decays rapidly at room temperature according to the equation 2CI0(g) > Cl2(g) + 02(g) From the following data, determine the reaction order and calculate the rate constant of the reaction TIME (s) [CIO] 0.12 x 10-3 8.49 x 10-6 0.96 x 10-3 7.10 x 10-6 5.79 x 10-6 5.20 x 10-6 4.77 x 10-6 2.24 x 10-3 3.20 x 10-3 4.00 x 10-3

3. Chlorineoxide(CIO),whichplaysanimportantrole in the depletion of ozone decays rapidly at room temperature according to the equation 2CI0(g) > Cl2(g) + 02(g) From the following data, determine the reaction order and calculate the rate constant of the reaction TIME (s) [CIO] 0.12 x 10-3 8.49 x 10-6 0.96 x 10-3 7.10 x 10-6 5.79 x 10-6 5.20 x 10-6 4.77 x 10-6 2.24 x 10-3 3.20 x 10-3 4.00 x 10-3

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

Cyclobutane, C4H8, consisting of molecules in which four carbon atoms for a ring, decomposes when heated to give ethylene. C4H8(g) → 2C2H4(g) The reaction is first order. In an experiment, the initial concentration of cyclobutane was (3.500x10^-3) M. After heating at 450 °C, for (5.55x10^2) s, this was reduced to (2.6090x10^-3) M. What was the concentration of cyclobutane after a total of (1.008x10^3) s? Express your answer to three significant figures. Just enter the number (e.g. 2.48x10^-4) and the unit.
For the reaction: NO2(g) → 1/2 O2(g) + NO (g) The following data were obtained: Time (s) 0 50 100 [NO₂] (M) 0.01 Concentration NO2 0.00787 -4.844697217 127.064803 200 0.00481 -5.337058195 0.00649 -5.037492748 154.0832049 300 0.0038 -5.572754212 0.012 0.01 0.008 Natural Log [NO2] (M) Determine the rate law of this reaction and the value of k, the rate constant. The graphs of the data appear below. 0.006 0.004 -4.605170186 100 0.002 0 0 1/[NO2] 100 200 Time (s) 207.9002079 1/[NO2] 263.1578947 y = -1.97E-05x + 9.15E-03 R² = 9.27E-01 300 250 200 150 100 50 0 300 0 50 400 100 Natural Log [NO2] 150 -4.5 -4.7 -4.9 -5.1 -5.3 -5.5 -5.7 0 200 Time (s) y = 0.5431x + 99.833 R² = 1 100 250 300 200 Time (s) 350 y = -0.0032x - 4.6679 R² = 0.9824 300 400
What is the half life of the following reaction, given the following set of conditions (Hint: observe the units for the rate constant to determine the order of the reaction!): 2 HI (g) → H2 (g) + I2 (g) Initial concentration of HI = 1.00 M k = 1.2 x 10-3 M-1 s-1
The following initial rate data are for the reaction for the formation of phosgene from carbon monoxide and chlorine: со + Clz → COCI2 Initial Rate, Ms-1 Experiment [CO]o, M [CIz]o, M 2.45 0.399 1.43x10-28 2 2.45 0.798 |2.85х10-28 3 4.90 0.399 2.85x10-28 4 4.90 0.798 5.71x10-28 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-1s-1.
The reaction described by the equation 0,(g) + NO(g) → 0,(g) + NO,(g) has, at 310 K, the rate law rate of reaction = k[O,][NO] k = 3.0 × 106 M-!·s-! Given that [O,] = 4.0 × 10-4 M and [NO] = 2.0 × 10-³ M at t = 0, calculate the rate of the reaction at t = 0. %3D rate: M/s What is the overall order of this reaction? 3
The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H,(g) + % »(9) is zero order in HI with a rate constant of 1.20×104M s!. If the initial concentration of HI is 0.103 M, the concentration of HI will be 1.33×10-2 M after seconds have passed.
The reaction 2 NO (g) + O2 (g) → 2 NO2 (g) occurs when automobile exhaust releases NO into the atmosphere. Use the following data to determine the order with respect to NO for this reaction. Trial [NO] (M) [O2] (M) Initial Rate (M/s) 1 0.012 0.020 1.02 x 10-4 2 0.024 0.020 4.08 x 10-4 3 0.024 0.040 8.16 x 10-4 Enter the answer as a single digit, not the word.
How do you find the order for [O2]?
6) For the reaction 3A + 2B2C + D + E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Rate (M/s) 1.9 x 108 [A] (M) [B] (M) 1.0 x 10¹2 1.0 x 10¹1 9.5 x 108 5.0 x 10¹2 1.0 x 1011 3 5.7 x 108 1.0 x 10¹2 3.0 x 10¹1 a) Write the rate law for this reaction. rate=[A]*[B]Y 3 3.0 x 10" 1.0 x10¹2 y = ²/ 5.0×10 1.0x1010 X = = 1 1.0x10" 1.0 ×1010 5 3=1 b) What is the overall order of the reaction? c) Calculate the rate law constant, k (including units). x = = 1.0x10" 1.0 x 10" 1 lom C²
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. k = A + 2B → C + D Trial [A] (M) [B] (M) Rate (M/s) 1 0.260 0.260 2 0.260 0.520 3 0.520 0.260 Units 0.0199 0.0199 0.0796
Given the information based on time and concentration, determine the order of the reaction and the rate constant k when graphing the following data: A--> C+D Time (s) (A] M 10 0.1000 50 0.0856 100 0.0749 200 0.0598 350 0.0460 500 0.0373 800 0,0271
13.102 Chlorine oxide (CIO), which plays an important role in the depletion of ozone (see Problem 13.101), decays rapidly at room temperature according to the equation 2C10(g) Cl₂(g) + O₂(g) From the following data, determine the reaction order and calculate the rate constant of the reaction. Time (s) 0.12 x 10-³ 0.96 x 10-³ 2.24 x 10-³ 3.20 x 10-³ 4.00 x 10-³ [CIO] (M) 8.49 x 10-6 7.10 x 10-6 5.79 x 10-6 5.20 x 10-6 4.77 x 10-6