The dithionite is formed by the reduction reaction of sulphur oxide. This proceeds according to the following equation:2,502 + H2» S204H2The following rate data were collected at 510 K for the rate of consumption of SO2:Initial concentrationExperimentSO2 (mol L-1)H2 (mol L-1)Initial Rate (mol L-s1)12.31 x 10-19.64 x 10-14.82 x 10-14.82 x 10-12.28 x 10-46.93 x 10-12.07 x 10-32.33 x 10-432.31 x 10-1Deduce the experimental rate law for this reaction including the order with respect to each reactant and then determine the rate constant.Show your working clearly, paying attention to significant figures and units.

Answered: Image /qna-images/answer/12d890fd-f725-490e-b7f8-84eff37b53b8.jpg

The dithionite is formed by the reduction reaction of sulphur oxide. This proceeds according to the following equation: 2,502 + H2- S204H2 The following rate data were collected at 510K for the rate of consumption of SO2: Initial concentration Experiment SO2 (mol L-1) H2 (mol L-1) Initial Rate (mol L-1s-1) 2.31 x 10-1 9.64 x 10-1 4.82 x 10-1 4.82 x 10-1 2.28 x 10-4 2.07 x 10-3 2.33 x 10-4 2 6.93 x 10-1 2.31 x 10-1 3 Deduce the experimental rate law for this reaction including the order with respect to each reactant and then determine the rate constant. Show your working clearly, paying attention to significant figures and units.

The dithionite is formed by the reduction reaction of sulphur oxide. This proceeds according to the following equation: 2,502 + H2- S204H2 The following rate data were collected at 510K for the rate of consumption of SO2: Initial concentration Experiment SO2 (mol L-1) H2 (mol L-1) Initial Rate (mol L-1s-1) 2.31 x 10-1 9.64 x 10-1 4.82 x 10-1 4.82 x 10-1 2.28 x 10-4 2.07 x 10-3 2.33 x 10-4 2 6.93 x 10-1 2.31 x 10-1 3 Deduce the experimental rate law for this reaction including the order with respect to each reactant and then determine the rate constant. Show your working clearly, paying attention to significant figures and units.

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

Pls help ASAP.
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,…
show work please
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…
None
solve using excel and explain please 6. The rate constant of the following second-order reaction of hydroxyl radical with 1,2- dichloroethane: OH (g) + CICH,CH2(g) → H20(g) + ClIchCH;CI(g) was investigated experimentally and the following table was obtained TPC k/s a. What is the reaction order, why? b. Determine the Arrhenius parameters for this reactions c. Calculate the enthalpy, entropy, and free energy of activation at 298 K using Eyring equation for the transition complex (See page 338-343 Chapter 18 for part b and c 10.0 2.08 15.7 4.57 21.5 27.5 15.80 33.2 28.40 38.5 46.10 45.7 8.24 93.50
5 ScAc4590506f/General?threadld-19:9597603ecb3f40b5ab24e8aee75e899c@thread.tacv28tcbx-channel Posts Files Class Notebook Moodle 2 more v O Meet versity of Technology and Applied Sciences - Ibri Course search Mazin Al Hinaai Consider the following reaction, A-B, the rate of reaction is 7.5 x 10-6 moldm 3s1. The time taken for the reaction is 9.5 minutes. What is the concentration? ion O a. 4275 x 10 -3 moldm 3 O b. 427.5 x 10 3 moldm 3 OC. 42.75 x 10 -3 moldm 3 Activate Windows Go to Settings to actvate Wdow O d. 4275 x 10 -3 moldm 1:35 PM A D A 4) ENG 4/12/202 Cop
D. Pls answer asap . Pls provide accurate answer. Help me thank uuu. Handwritten thank u.
Now consider the following reaction and data: H₂+2IF→2HF + I₂ Time S Part B 15 15 I, concentration (M) 1.50 1.73 4 What is the average rate of formation of I₂? Express your answer to three decimal places and include the appropriate units.
Hw.139.
The reaction between bromate ions and bromide ions in acidic aqueous solution is given by the following equation: BrO3- (aq) + 5Br- (aq) + 6H+ (aq) --> 3Br2 (l) + 3H2O (l) The experimental results are given below. Experiment Initial [BrO3-] Initial [Br-] Initial [H+] Initial Rate (M s-1) 1 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.20 0.20 0.10 3.2 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 Using these data, determine the orders for all reactants, the overall reaction order, and the value of the rate constant.
Use the References to access important values if needed for this question. The following initial rate data are for the reaction of UO2+ with hydrogen ion in aqueous solution: 2UO2+4HU++ UO22++ 2H2O Experiment [UO2] M [H] M Initial Rate, M. s¹ 0' 1 0.000748 0.664 0.0000628 2 0.00150 0.664 0.000252 3 0.000748 1.33 0.000126 4 0.00150 1.33 0.000506 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for mor n and concentrations taken to the zero power do not appear. Don't enter 1 for mor n. Rate= k= M-2 -1 S Submit Answer Retry Entire Group 1 more group attempt remaining