4. The reaction of pentene with ozone was studied in CCL, at 25°C. CSH10 + O3 → C3H100 The reaction was observed, and the following data was collected: Trial Rate (M/s) [C3H10]; [O]; 1 2.2 0.0100 0.0028 1.1 0.0050 0.0028 3 4.4 0.0100 0.0056 What is the rate law expression for this reaction? а. b. What is the value of k for this reaction from the data? c. Why isn't the concentration of the CC14 given in the data table? С. 2.

4. The reaction of pentene with ozone was studied in CCL, at 25°C. CSH10 + O3 → C3H100 The reaction was observed, and the following data was collected: Trial Rate (M/s) [C3H10]; [O]; 1 2.2 0.0100 0.0028 1.1 0.0050 0.0028 3 4.4 0.0100 0.0056 What is the rate law expression for this reaction? а. b. What is the value of k for this reaction from the data? c. Why isn't the concentration of the CC14 given in the data table? С. 2.

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

Given: 2NO2 --> 2NO + O2 [NO2]o (M) Rate (M/s) 0.01 7.1 x 10-5 0.02 28.1 x 10-5 a) Give the rate law and overall order. b) What is [NO2] at 125 s if [NO2]o = 0.015 M?
Answer all the parts please
In the general rate law rate=k[I2]X[H+]Y[CH3COCH3]Z what are the values of X, Y, and Z? Drag each item to the appropriate bin -1 0 1 2
Give typed full explanation not a single word hand written otherwise leave it CH3SCH3(g) + OH(g) → Products For a constant O2 concentration of 150 torr, it has an activation energy of -15880 J/mol and a rate constant at 270.0 K of 1.33 x 10-11 cm3/molecule/s. Determine the rate constant at 27 °C (cm3/molecule/s).
19. The initial rate of decomposition of acetaldehyde at 600°C was measured at a series of concentrations with the following results. Solve for the rate law expression of this reaction. Note: Include all rough notes, show all calculations, follow the rules of significant figures, and box your final answer. ( CH;CHO(g) → CH,(g) + CO(g) Trial Number Trial #1 Trial #2 Trial #3 Trial #4 [CH,CHO] 0.10 M 0.20 M 0.30 M 0.40 M Initial rate 0.085 0.34 0.76 1.4 (mol/L-s)
This is your graph. The rate of reaction at any point in time is given by the gradient of the concentration-time graph. Annotate your graph to show how you could determine the rate of reaction at 6 hours by drawing a tangent to the curve. Include your annotated graph in the answer and use the values from it to calculate the rate of reaction at 6 hours. Show your calculation in full.
Only #2. I circled the correct answer.
An unknown inorganic phosphate undergoes first-order dehydration in a drying oven. Initially, the excess water content is measured to be 1.13 mg. After 2.10 days the water content is reduced to 0.488 mg. After 4.40 days, water content is only 0.194 mg. Determine the half-life of hydration under these conditions.
Please use the values in the resources listed below instead of the textbook values. The rate of the electron-exchange reaction between naphthalene (C10H8) and its anion radical (C10H8¯) in an organic solvent is diffusion controlled. C10H8 + C10H8 = C10H8 + C10H8 The reaction is bimolecular and second order. The rate constants are as follows. T/K 305 295 291 275 k/109 M-1.s-1 2.64 2.21 2.05 1.49 Calculate the values of Ea, AHº†, ASº† and AG°† at 295 K for the reaction. [Hint: Rearrange the equation below and plot In(k/T) versus 1/T.] KBT eASot/R@¬AH°†/RT(M1 – m) k = h Ea X kJ•mol-1 2993.386 AHo* X kJ•mol-1 2991.1 ASo# = X J:K-1.mol-1 -28069.52 AG°# X kJ•mol-1 107010.2
The activation energy for the gas phase decomposition of acetic anhydride is 144 k). (CH3CO)20→CH2=C=0 + CH3COOH The rate constant at 502 K is 9.94x10 4/s. The rate constant will be 9.74x10 3/s at K.
A reaction between substances A and B has been found to give the following data: 3A + 2B --> 2C + D [A] (mol/L) [B] (mol/L) rate of appearence of C (mol/L-hr) 0.01 1.0 3.00 x 10-6 0.01 3.0 8.10 x 10-6 0.02 3.0 3.24 x 10-5 0.02 1.0 1.20 x 10-6 0.03 3.0 7.30 x 10-5 Using the above data, determine the order of the reaction with respect to A and B, the rate law, and calculate the specific rate constant.