the mean time, the rate,[S₂O3] in the reactionmay label clear outliersthe mean) as such ande calculation.on mixturesNH4)2SO4 (NH4)2S2O8|(mL)(mL)1.500.501.500.501.001.001.001.00following reagents areum iodideium persulfatem thiosulfateum nitrateium sulfateodide in the solution in theAnswer: 0.050 M• Determination of the rate law follows the protocol in ref.(5). with one difference. A reactant order (rate lawexponent) will be calculated twice using two differentpairs of determinations (e.g. determinations 1 & 2 anddeterminations 3 & 4). Then the mean is taken of bothvalues and reported as order. This is done for eachreactant. This additional step allows us to include moredata and reduce experimental error.Practice Problem 2: The rate of a reactionCO(g) +3H₂(g)→ CH4(g) + H₂O(g)was determined at 25 °C. From the following data,determinea) the mean reaction order with respect to COb) the mean reaction order with respect to H₂c) the overall rate orderd) the rate law for the reaction ande) the mean rate constant.Det. [CO] (M) [H₂] (M)12340.1000.4000.1000.4000.2000.2000.6000.600Initial rate (M/s)1.12 x 10-44.75 x 10-43.45 x 10-41.34 x 10-3Answer: a) x = 1.01 1, b) y = 0.982 1, c) 2, d)rate = k[CO] [H₂], e) k = 5.72 x 10-3 M-¹S-¹.

The objective of the question is to calculate the-The mean reaction order with respect to The mean…

• Practice Problem 2: The rate of a reaction CO(g) +3H2(g)→→ CH4(g) + H₂O(g) was determined at 25 °C. From the following data, determine a) the mean reaction order with respect to CO b) the mean reaction order with respect to H₂ c) the overall rate order d) the rate law for the reaction and e) the mean rate constant. Det. [CO] (M) 1 2 3 4 0.100 0.400 0.100 0.400 [H₂] (M) 0.200 0.200 0.600 0.600 Initial rate (M/s) 1.12 x 10-4 4.75 x 10-4 3.45 x 10-4 1.34 x 10-3 Answer: a) x = 1.01 1, b) y = 0.982≈ 1, c) 2, d) rate = k[CO] [H₂], e) k = 5.72 x 10-³M-¹s-¹.

• Practice Problem 2: The rate of a reaction CO(g) +3H2(g)→→ CH4(g) + H₂O(g) was determined at 25 °C. From the following data, determine a) the mean reaction order with respect to CO b) the mean reaction order with respect to H₂ c) the overall rate order d) the rate law for the reaction and e) the mean rate constant. Det. [CO] (M) 1 2 3 4 0.100 0.400 0.100 0.400 [H₂] (M) 0.200 0.200 0.600 0.600 Initial rate (M/s) 1.12 x 10-4 4.75 x 10-4 3.45 x 10-4 1.34 x 10-3 Answer: a) x = 1.01 1, b) y = 0.982≈ 1, c) 2, d) rate = k[CO] [H₂], e) k = 5.72 x 10-³M-¹s-¹.

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter20: Rates Of Chemical Reactions, I. The Iodination Of Acetone

Section: Chapter Questions

Problem 3ASA

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