The rate of the reaction CH,COOC,H (ag) + оН (ад) — СH,COO "(аg) + Cән,ОН(ад) was measured at several temperatures, and the following data were collected: Temperature (°C) к(м+s-) 15 0.0521 25 0.101 35 0.184 45 0.332 Calculate the value of Eq by constructing an appropriate graph.

The rate of the reaction CH,COOC,H (ag) + оН (ад) — СH,COO "(аg) + Cән,ОН(ад) was measured at several temperatures, and the following data were collected: Temperature (°C) к(м+s-) 15 0.0521 25 0.101 35 0.184 45 0.332 Calculate the value of Eq by constructing an appropriate graph.

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

estion 3 of 3 Time and concentration data were collected for the reaction 0.52 A → products 0.48 0.44- t (s) [A] (M) 0. 0.52 0.40- 20 0.43 0.36- 40 0.35 0.32- 60 0.29 0.28 - 80 0.23 100 0.19 0.24 0.20. The blue curve is the plot of the data. The straight orange line is tangent to the blue curve at t = 40 s. 0.16. 0 10 20 30 40 50 60 70 80 90 t (s) Approximate the instantaneous rate of this reaction at time t = 40 s. instantaneous rate: M/s [A] (M)
но HO HO HO 0 + ½ O, → + H,0 H H но OH ascorbic acid dehydroascorbic acid Vitamin C is oxidized slowly to dehydroascorbic acid by the oxygen in air. It is catalyzed by ions such as Cu*2 and Fe*3. The reaction can be followed by measuring the ultraviolet absorbance at 243 nm. Time (hours) Absorbance (A) 1/A In A - In A 0.75 1.3 -0.29 0.29 1 0.38 2.6 -0.97 0.97 2 0.19 5.3 - 1.7 1.7 3 0.095 11 - 2.4 2.4 29. What is the hybridization of carbon 1 (far left) and carbon 2 (middle) in this hydrocarbon: CH3CH=CH2? (A) sp³, sp (B) sp?, sp? (C) sp³, sp? (D) sp, sp?
A student suspects that the nitrate ion (NO3−), rather than the Cu2+ ion, is the active species in the Cu(NO3)2 catalyst. He devises a second experiment to test his hypothesis, using KNO3 as a potential catalyst. If the student's hypothesis is correct, what should he observe when KNO3 is added to the reaction? Any changes are observed relative to an identical un-catalyzed reaction. a. The rate of the reaction will decrease b. The rate of the reaction will increase c. There will be no change in the rate of the reaction
Consider the following complex reaction: P + 2Q → Products whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [P](M) [Q](M) Rate(M/s) 1 0.100 0.050 2.25 × 10−3 2 0.100 0.150 6.75 × 10−3 3 0.200 0.050 9.00 × 10−3 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law (express your answer to three significant figures), and select the units for k.
Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H,(g) + 2 NO(g) → N,0(g) + H,0(g) k1 2 H2(9) + N,0(9) → N2(9) + H,O(g) Suppose also k, «k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k U Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k-2 for k = the reverse of the two elementary reactions in the mechanism.
Can my answers be checked please thank you .
The following kinetic data were collected at 298 K for the reaction of ozone with nitrite ion, producing nitrate and oxygen: NO, (aq) +O,(g) NO, (aq) +0,(g) > Experiment [NO2 lo (M) [O3lo (M) Initial Rate (M/s) 1 0.0100 0.0050 25.0 0.0150 0.0050 37.5 3 0.0200 0.0050 50.0 0.0200 0.0200 200.0
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=69.0 kJ/mol. If the а - 1 rate constant of this reaction is 5.7 × 10² M - 1 S. at 304.0 °C, what will the rate constant be at 256.0 °C? Round your answer to 2 significant digits. - 1 - 1 k = || M •S x10 ?
I rate Method: Explain how to get the rate law trom calculate the orders (step by step) and the value of k including units caction of A +B C D А. М 20 10 10 B, M 15 45 Rate, M/s 4.88 х 10- 7.37 x 10 2.45 x 10 Run 2 .15
Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction equation 2H,0, (aq) — 2н,00) + 0,(8) The activation energy for this reaction is 75 kJ-mol-1. In the presence of a metal catalyst, the activation energy is lowered to 49 kJ-mol-1. At what temperature would the non-catalyzed reaction need to be run to have a rate equal to that of the metal-catalyzed reaction at 25 °C? T = K