4. The following data were collected for the reaction of t-butyl bromide, (CH3)3CBr,with hydroxide ion at 55°C.Experiment12345(CH3)3CBr + OH → (CH3)3COH + BrInitial Concentration (M)Torony(CH3)3CBr0.100.200.300.100.10OH-0.100.100.100.200.30Initial Rateof Formation of(CH3)3COH (mol L-¹ s^¹)a) Calculate the order with respect to (CH3)3CBr and then with respect to OH-.What is the overall order of the reaction?b) Write the rate law.10.00100.00200.00300.00100.0010Department of ChemistryS1500X General Chemistry LaboratorySummer 2023c) What is the value of the rate constant for this reaction at 55°C? (Don't forget theunits!)d) If the activation energy for this reaction were 100 kJ/mol, what would the valueof the rate constant be at 75°C? (k = Ae -Ea/RT, R = 8.314 J/mol K) Hint: Youneed to use the information you calculated in step c in order to first calculatethe value of A.

Answered: Image /qna-images/answer/1115144a-1608-4da1-9ae7-938cb2aec514.jpg

4. The following data were collected for the reaction of t-butyl bromide, (CH3)3CBr, with hydroxide ion at 55°C. Experiment 1 2 3 4 5 Sony (CH3)3CBr + OH → (CH3)3COH + Br Initial Concentration (M) Initial Rate of Formation of (CH3)3COH (mol L-¹ s¹¹) Summer 2023 (CH3)3CBr 0.10 0.20 0.30 0.10 0.10 OH- 0.10 0.10 0.10 0.20 0.30 a) Calculate the order with respect to (CH3)3CBr and then with respect to OH". What is the overall order of the reaction? b) Write the rate law. 0.0010 0.0020 0.0030 0.0010 0.0010 Department of Chemistry S1500X General Chemistry Laboratory

4. The following data were collected for the reaction of t-butyl bromide, (CH3)3CBr, with hydroxide ion at 55°C. Experiment 1 2 3 4 5 Sony (CH3)3CBr + OH → (CH3)3COH + Br Initial Concentration (M) Initial Rate of Formation of (CH3)3COH (mol L-¹ s¹¹) Summer 2023 (CH3)3CBr 0.10 0.20 0.30 0.10 0.10 OH- 0.10 0.10 0.10 0.20 0.30 a) Calculate the order with respect to (CH3)3CBr and then with respect to OH". What is the overall order of the reaction? b) Write the rate law. 0.0010 0.0020 0.0030 0.0010 0.0010 Department of Chemistry S1500X General Chemistry Laboratory

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

The following mechanism has been proposed for the gas phase reaction of nitrogen monoxide with bromine. step 1 fast: NO + Br₂ step 2 slow: NOBr₂ + NO (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + NOBr2 2 NOBr Rate = + (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A][B]", where '1' is understood (so don't write it if it's a '1') for m, n etc.
Analyze the following reaction mechanism: H2O + O → CIÓ + CF2CI CI + 202 4. Cl + CF2CI –→ CF2CI2 1. H2O2 2. O + CF2CI2 3. CIO + Oз -> Identify the reaction intermediates in this reaction. A) O, CIO, CI B) CI, CF;CI, CF2CI2 C) O, CIO, O, H20 D) O, CIO, CI, CF2CI E) O, CIO, CI, CF;CI2
Chem 116 Spring 2020 recitation Week 5 Rate law 1. The following data were obtained for the reaction A + B+ C → products: Initial rate, Vo [A]o Experiment [B]o [C]o (mol L1s) 1.25x10-3 M 1.25x10-3 M 1.25x10-3 M 0.0087 2.50x10-3 M 1.25x10-3 M 1.25x10-3 M 0.0174 1.25x10-3 M 3 3.02x10-3 M 1.25x10-3 M 0.0508 1.25x10-3 M 4 3.02x10-3 M 3.75x10-3 M 0.457 3.01x10-3 M 1.00x10-3 M Find the rate law, reaction order, k, and the initial rate of the 5th experiment from the above data %23 1.15x10-3 M 1,
Use the following data to determine the rate law and the rate constant of the reaction 3A+B-->C+D
Need help 6 Use sig figs
10 tobio 15 2. The initial rate of the reaction: BrO3(aq) + 5 Br (aq) + 8 H*(aq) ----> 3 Br₂(l) + H₂O(l) Has been measured at the reactant concentrations shown (in mol/L): Trial [BrO3] [Br] [H*] Initial rate (mol/Ls) 1 0.10 0.10 0.10 8.0 x 104 2 0.20 0.10 0.10 1.6 x 10³ 3 0.10 0.20 0.10 1.6 x 10³ 4 0.10 0.10 0.20 er 3.2 x 10³ A) Determine the rate law equation including the k value. 1 Determine the order of reaction for BrO3, Br, and H* Rate law
#2 please
Hydrogen gas reduces NO to N2 in the following reaction:$$2H2(g)+2NO(g)2H2O(g)+N2(g)The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2]0 (M) [NO]0 (M) Initial Rate (M/s) 1 0.212 0.136 0.0387 2 0.212 0.272 0.0777 3 0.424 0.544 0.615 4 0.848 0.544 2.47 Determine the rate constant for the reaction at 1500°C. M-xs-1
1. The bromination of acetone is acid-catalyzed: CH3COCH3 + Br2 → CH3COCH2BR + H* + Br The rate of disappearance of bromine was measured for several different concentrations of acetone, bromine and H+ ions at a certain temperature: Rate of disappearance [CH3COCH3] [Br2] [H*] 0.050 of Br2 (M/s) (a) (b) (c) (d) (e) 5.7 x 105 5.7 x 105 1.2 x 104 3.1 x 104 7.6 x 105 0.30 0.050 0.30 0.10 0.050 0.30 0.050 0.10 0.40 0.050 0.20 0.40 0.050 0.050 A. What is the order of the reaction with respect to acetone? B. What is the order of the reaction with respect to bromine? C. What is the order of the reaction with respect to acid? D. Determine the average rate constant for the 5 reaction mixtures. E. Write the complete rate law for the reaction based on the experimental data given.
A mechanism for the gas phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is: step 1 slow: F2 + ClO2 FClO2 + F step 2 fast: F + ClO2 FClO2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + + (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]m[B]n... , where '1' is understood (so don't write it) for m, n etc.) Rate =
a and b please
Chemistry please i need the answer of any two of them thanks.