The following initial rate data are for the reaction of nitrogen dioxide withfluorine:2 NO2+ F2 → 2 NO₂F.-1Experiment [NO2]0, M [F2]o, M Initial Rate, M s•4.632.081.24 × 10-34.634.169.262.089.264.161234Rate =k=2.48 x 107M-¹.s-¹2.48 x 107-3Complete the rate law for this reaction in the box below.Use the form k[A] [B]", where '1' is understood for m or n andconcentrations taken to the zero power do not appear. Don't enter 1 for m or n.-3-34.97 × 107

Answer:Power of the concentration term of a reactant in rate law is equal to the order of reaction…

The following initial rate data are for the reaction of nitrogen dioxide with fluorine: Experiment [NO2]0, M 4.63 4.63 9.26 9.26 1 2 3 2 NO2+ F2 → 2 NO₂ F Rate k = M-¹. S -1 [F2]o, M Initial Rate, M. s-¹ 2.08 4.16 2.08 4.16 -1 1.24 x 10 2.48 × 10 -3 -3 2.48 x 107 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 -3 -3 4.97 x 107

The following initial rate data are for the reaction of nitrogen dioxide with fluorine: Experiment [NO2]0, M 4.63 4.63 9.26 9.26 1 2 3 2 NO2+ F2 → 2 NO₂ F Rate k = M-¹. S -1 [F2]o, M Initial Rate, M. s-¹ 2.08 4.16 2.08 4.16 -1 1.24 x 10 2.48 × 10 -3 -3 2.48 x 107 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 -3 -3 4.97 x 107

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...

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2) 2 NO₂ (g) +2 NO(g) + O₂(g) (W) [ZON] 2.5 2 1.5 1 0.5 0 10 20 Reaction Data 30 40 50 60 70 Time (s) 80 Use the experimental data for the above reaction to answer. a) What is the average rate of reaction between 50 and 70 seconds? b) Estimate the instantaneous rate of reaction at 20 seconds. 90 100 c) Estimate the instantaneous rate of formation of O₂ at 30 seconds. d) If the initial concentration of NO₂ is 2.0M how much O₂ is produced in the first 40 seconds of reaction?
5. The reaction A →B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, min [A], M 5.00 x 10-2 4.30 x 10-2 5 10 3.70 x 10-2 2.74 x 10-2 1.51 x 10-2 20 40 1.12 x 10-2 8.26 x 10-3 50 60 (a) What is the average rate of reaction between 5 and 20 min? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 40 min. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.
The following initial rate data are for the gas phase reaction of hydrogen with iodine: H₂+I₂ → 2 HI Experiment [H₂0, M120, M Initial Rate, M.s¹ 0.0212 0.0180 7.17 x 10-22 0.0212 0.0360 1.43 x 10-21 0.0424 0.0180 1.43 x 10-21 0.0424 0.0360 2.87 x 10-21 1 2 4 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 71. Rate = k= M-1
Chemistry please i need the answer of any two of them thanks.
Hydrogen gas reduces NO to N2 in the following reaction: 2H, (g) + 2NO(g) 2H,0(g) + N, (g) The initial reaction rates of four mixtures of H, and NO were measured at 1500°C with the following results: Experiment [H2]o (M) [NO]o (M) Initial Rate (M/s) 0.212 0.136 0.0393 2 0.212 0.272 0.0789 0.424 0.544 0.624 0.848 0.544 2.50 4.
The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C: NO + 03- NO2 + 02 Initial Rate, Experiment [NO]o, M [03]o, M Ms-1 0.292 7.88x10-2 7.88x10-2 3.70x10-2 7.40x10-2 0.583 0.158 3.70x10-2 0.585 4 0.158 7.40x10-2 1.17 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 following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C: NO + 03 NO₂ + O₂ Experiment [NO]o, M [03]o, M Initial Rate, M-s1 0.192 0.0497 0.928 0.192 0.0994 1.86 0.384 0.0497 1.86 0.384 0.0994 3.71 1 2 3 4 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 71. Rate = k= M
QUESTION 1 The thermal decomposition of an oxide produced the following data: time (5) 120 180 240 300 560 680 [oxide] (M) 1.2 0.53 0.41 0.34 0.29 0.17 0.15 0.00 Determine: a) The order of the reaction. Explain your reasoning. b) The rate constant of the reaction. Be sure to include units and explain how you arrived at this answer.
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 ICl with hydrogen:2 ICl + H2I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.438 0.105 9.37×10-3 2 0.876 0.105 1.87×10-2 3 0.438 0.209 3.71×10-2 4 0.876 0.209 7.42×10-2 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 = _______ From these data, the rate constant is __________M-2s-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.
3. Initial rates shown below were measured for the following reaction: CO(g) + Cl2(g) → COCl2(g) Experiment 1234 2 3 Initial [CO], M 1.00 0.100 0.100 0.100 a) What is the rate law for this reaction? Initial [Cl₂], M 0.100 0.100 1.00 0.0100 Initial rate, M/min 1.29 x 10-29 1.33 x 10-30 1.30 x 10-29 1.32 x 10-31 b) What is the value of the rate constant for this reaction? Be sure to include units with your answer.