The following data were obtained from a study of the decomposition of CHEM at 320 °C: t, second S 0.00 200 400 Concentration of CHEM, mole/L 1.16 0.86 0.65 Plot the data using the first- and second-order equations. A. What is the correlation coefficient (r) for each plot? A1. r for first-order? choose your answer... A2. r for second-order? choose your answer... B. What is the order for this reaction? choose your answer... C. What is the rate constant? choose your answer... D. What is the CHEM concentration (in mol/L) at 300 s? choose your answer... V V

The following data were obtained from a study of the decomposition of CHEM at 320 °C: t, second S 0.00 200 400 Concentration of CHEM, mole/L 1.16 0.86 0.65 Plot the data using the first- and second-order equations. A. What is the correlation coefficient (r) for each plot? A1. r for first-order? choose your answer... A2. r for second-order? choose your answer... B. What is the order for this reaction? choose your answer... C. What is the rate constant? choose your answer... D. What is the CHEM concentration (in mol/L) at 300 s? choose your answer... V V

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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P 12:41 A docs.google.com 100% @ * ZAIN IQ Iı. إجابنك Q1) Calculate the quantity adsorbed at equilibrium according to first and second order equations for the adsorption of methylene blue dye on charcoal surface at 250C, if the quantity adsorbed at time 15 min. are equal to 19.32 mg/g. The values of first and second order constants are 0.176 min-1 and 0.013 g.mg-1.min-1. Respectively.
The data below were obtained for the decomposition of oxygen difluoride 20F2 → 02 + 2F2 at 298 K. t/s [OF;]/10³ mol dm Verify that this is second order reaction find a value for the rate constant at 298 K. 60 120 180 3.8 240 300 7.2 5.5 4.6 3.3 2.9
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C blackboard.sc.edu Content Blackboard Lea... > Recitation W3... J Late Model Ca... rate = k[N₂01² Question 3 Worksheet 13.6 #2 X Consider the two-step mechanism below that has been proposed for the reaction of nitrous oxide to form nitrogen and oxygen gas to answer the following questi Step 1: N₂0 (g) → N2 (9) + O (g) (slow) (fast) Step 2: N₂O(g) + O (g) → N2 (g) + O2 (9) Net: 2 N₂O (g) → 2 N2 (9) + O2 (9) Part B: Based on the proposed rate law for the net overall reaction, what is the overall order of the reaction? Selected Answer: 1/2 order Worksheet 13.6 #2 Consider the two-step mechanism below that has been proposed for the reaction of nitrous oxide to form nitrogen and oxygen gas to answer the following questi Step 1: N₂O (g) → N₂ (g) + O (9) (slow) (fast) Step 2: N₂O(g) + O (g) → N₂ (9) + 02 (9) Net: 2 N₂0 (g) → 2 N2 (9) + 02 (9) Part C: What intermediates/catalysts are present in this mechanism? Selected Answer: N₂O is a catalyst; there are no intermediates Wednesday, April 6,…
3-chem The gas phase reaction of hydrogen with iodine H2 + I22 HI is first order in H2 and first order in I,. Complete the rate law for this reaction in the box below. Use the form k[A]™[B]"... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 1.98×10-18 M's. Using this value for the rate constant, the rate of the reaction when [H2] = 2.20×10² M and [I,] = 1.42×102 M would be Ms-1.
The first-order degradation of a drug was monitored under three different conditions (I, ii, and iii), which resulted in half-lives (in no particular order) of 4 hours, 8 hours, and 10 hours: а. i. at 37 °C. ii. at 37 °C, in the presence of a catalyst. iii. at 21 °C. Identify which half life goes with which set of conditions. For condition i., draw and label a graph of Concentration (mmol/L) vs Time (hr). Start with an initial concentration of 10 mmol/L and show the decay over 40 hours. You may use the grid below or draw your graph by hand. 10 9.5 8.5 7.5 2 6.5 E 5.5 4.5 4 3.5 2.5 1.5 0.5 4 8 10 12 14 16 18 20 22 24 26 28 30 32 34 36 38 40 Time (hours) -1 Another reaction is found to have an activation energy of 80.3 kJmol. The reaction is very slow at 25°c. Which will be the more effective way of speeding up the reaction, b. -1 i. adding a catalyst which lowers the activation energy to 30.0 kJ mol or ii. raising the temperature from 25°C to 50°C ? Show all calculations and explain…
... cvg.cengagenow.com The gas phase decomposition of sulfuryl chloride at 600 K SO₂Cl₂(g) SO₂(g) + Cl₂(g) is first order in SO₂Cl₂. 0.000657 M after 503.0 min had passed. + OWLV2 | Online teaching and learning resource from Cengage Learning During one experiment it was found that when the initial concentration of SO₂Cl₂ was 0.00494 M, the concentration of SO₂Cl₂ dropped to Based on this experiment, the rate constant for the reaction is min-¹. 99% 00 00
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.
A certain first-order reaction is 62% complete in 55 s. What are the values of the rate constant and the half-life for this process? a. k = -1 S b. t₁/2 = Submit Answer S Try Another Version 1 item attempt remaining
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a. What is the average rate of NO₂ appearance in the range between 300-400 sec? b. Estimate the instantaneous rate of N₂Os decomposition at t = 200 sec. c. Estimate the initial rate of N₂Os decomposition.
4.2 * 10 - 4s - 1 . What is the half- life 4. The rate constantk for a first-order reaction is equal to for the reaction?