The ozonization of pentene in carbon tetrachloride solution at 25 °C C3H10 + O3C3H10O3 is first order in C3H10 and first order in O3. 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 of the reaction was determined to be 250 Ms-1 when [C3H10] = 9.52×10-2 M and [O3] = 2.41×10-² M. From this experiment, the rate constant is

The ozonization of pentene in carbon tetrachloride solution at 25 °C C3H10 + O3C3H10O3 is first order in C3H10 and first order in O3. 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 of the reaction was determined to be 250 Ms-1 when [C3H10] = 9.52×10-2 M and [O3] = 2.41×10-² M. From this experiment, the rate constant is

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter20: Kinetics

Section: Chapter Questions

Problem 20.85E

See similar textbooks

Similar questions

The rate law for the hydrogenation (H) of ethylene (E) to form ethane (A) over a cobalt-molybdenum catalyst [Collection Czech. Chem. Commun.,51, 2760 (1988)] is (a)Suggest a mechanism and rate-limiting step consistent with the above rate law.(b)What was the most difficult part in finding the mechanism?
a) Briefly outline how you could determine the rate constant, k, of the reaction using this virtual experiment simulation. b) IO3- + 3 H3AsO3 → I- + 6 H+ + 3 HAsO42- . (Reaction 3) (catalysed by I-) This proceeds via two main reactions: 6 H+ + IO3- + 8 I- → 3 I3- + 3 H2O (Reaction 1) rate limiting step Followed by this rapid reaction: H3AsO3 + I3- + H2O → HAsO42- + 3 I- + 4 H+ (Reaction Over the course of the reaction (3), what would happen to the reaction rate if the pH was not maintained using acetic acid/sodium acetate buffers in the pH range 4 -5 but allowed to vary instead?
The variation in the partial pressure of azomethane (Azo) with time was followed at 600 K and the data obtained are reproduced in the table below.a) Confirm that the decomposition of CH3N2CH3(g)  C2H6(g) + N2(g) is first order with respect to azomethane and find the rate constant (reaction rate constant) at the temperature of the experiment. Interpret your answer. b) Fill in the table with the values and information you consider necessary to resolve the questions asked. c) What is the integrated form of the velocity law? (1.0 Pa ≈ 1.0 x 10-5 atm; 1.0 atm = 101.325 kPa); p = partial pressure).
Complete the rate law for this reaction in the box below. Use the form, where '1' is understood for or and concentrations taken to the zero power do not appear. Don't enter 1 for or. Rate = K=
Below is a proposed mechanism for ClO–(aq) reacting with I–(aq) in the presence of OH–(aq). ClO- +H2O --> HOCl +OH- (fast, reversible)I- +HOCl --> HOI +Cl- (slow)HOI + HO- --> IO- +H2O You are trying to show that the rate law for this proposed mechanism matches an experimentallydetermined one. What is the expression for koverall or k’ for the proposed mechanism?Note: When writing an expression, H2O is not involved (just don’t include it).
Complete the rate law for this reaction in the box below. Use the form, where '1' is understood for or and concentrations taken to the zero power do not appear. Don't enter 1 for or. Rate law = K=
The bromination of acetone is catalyzed by the acid CH2COCH3 (aq) + Br2(aq)+H2O →(acid catalyst) CH3COCH2 + H3O+(aq) + Br -(aq) The rate of dissappearance of bromine was measured for several different initial concentrations of acetone, bromine, and hydronium ion. (see image) A. Deduce the rate law for the reaction and give order with respect to each reactant B. What is the numerical value value of k, the rate constant C. If [H3O+] is maintained at 0.050 M, whereas both [CH3COCH3] and [Br2] are 0.10 M, what is the rate of reaction?
Explain the mechanism and potential energy surface of the reaction. N2O + hv → N2 + O Now choose an appropriate theory and describe how you would use it to determine the rate coefficient.
(i) In an iodine-clock involving peroxide: H2O2 (aq) +2I- (aq) + 2H+(aq) → 2H2O(l) + I2 (aq) The rate law has been determined to be: rate = k [H2O2][I-] with k= 0.658 L/Ms at 250C. If [I-] = 0.5, [H2O2]=0.25 and pH=5 what is the rate of reaction? (ii) In “peroxide clock” reaction above what is the rate of loss of I- ?
A solution of 100 g / L of acrylamide in methanol is polymerized at 25 ° C with 0.1 mol / Lof isobutyryl peroxide whose half-life is 9.0 h at this temperature and the efficiency inmethanol is 0.3. For acrylamide, kp2 / kt = 22 L / mol * s at 25 ° C and the termination is onlyby coupling. (a) What is the rate of polymerization, Rp? (b) How much polymer ishave you prepared in the first 10 minutes of reaction in 1 L of solution?
For a first order reaction, show that time required for 99% completion is twice the time required for the completion of 90% of reaction.
Give the reaction mechanism for the following subparts in clear handwritten!