The first-order rate constant for the thermaldecomposition of 3-methylcyclobutanone has the valuesT/K k/1045-! T/K k/104s!552.24 0.4259589.05 6.459561.81 0.8936596.96 11.201570.41 1.707606.14 20.83579.35 3.207a. Find the value of the activation energy and the valueof the preexponential factor.b. Find the value of the rate constant at 600.0 K.c. Find the time for 80.0% of the reactant to react at600.0 K.

Arrhenius equation is the equation that gives the effect of change in temperature on rate constant…

Answered: The first-order rate constant for the…

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...

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Initial-rate data at a certain temperature is given in the table for the reaction SO₂Cl₂(g) → SO₂(g) + Cl₂ (g) [SO₂Cl₂], (M) k = 0.100 0.200 0.300 Initial rate (M/s) 2.40 x 10-6 4.80 x 10-6 7.20 x 10-6 Determine the value and units of the rate constant. units:
38. Time and concentration data were collected for the reaction A → B. t (s) [A] (M) 0.600 30.0 0.484 60.0 0.405 90.0 0.349 a. Determine the reaction order with respect to A. b. Calculate the rate constant for the reaction. 0.00
Determine half-life, order, and k from concentration-time data. The following data were collected for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g)-CH₂(g) + H₂(g) + CO(g) [CH3OCH 3], M 7.02x10-² time, min 0 3.51x10-2 22.20 K 1.76x10-² 44.40 8.80×10-3 66.60 (a) What is the half-life for the reaction when [CH3OCH3] = 7.02x10-² M? (b) What is the half-life for the reaction when [CH3OCH3] = 3.51x10-² M? (c) Is the reaction first order? If so, what is the rate constant for the reaction? (If not first order leave blank). min min min-1
5. The reaction A →B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, min [A], M 5.00 x 10-2 4.30 x 10-2 5 10 3.70 x 10-2 2.74 x 10-2 1.51 x 10-2 20 40 1.12 x 10-2 8.26 x 10-3 50 60 (a) What is the average rate of reaction between 5 and 20 min? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 40 min. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.
The table shows the variation of the rate constant with temperature for the first-order reaction. 2N₂O5 (g) 2N₂O₂(g) + O₂(g) Determine graphically the activation energy for the reaction. Be sure your answer has the correct number of significant digits. T(K)|*(--) S 298. 1.74 x 10 308. 6.61 × 10 318. 2.52 × 10 328. 7.59 × 10 338. 2.40 × 10 - 5 -5 -4 -4 3 Note: Reference the Fundamental constants table for additional information.
The rate of a certain reaction was studied at various T(K) k (s-1) temperatures. The table shows temperature (T) and rate 400 0.000108 constant (k) data collected during the experiments. Plot the 420 0.000626 data to answer the questions. 440 0.00310 What is the value of the activation energy, E, for 460 0.0134 this reaction? 480 0.0511 500 0.175 520 0.547 E, = kJ - mol- 1108.79 540 1.57 560 4.18 Incorrect 580 10.4 What is the value of the pre-exponential factor (sometimes called the frequency factor), A, for this reaction? A = 140 6.79 x10 Incorrect
The first-order rate constant for the decomposition of C2H5Cl, C2H5Cl(g) C2H4(g) + HCl(g) at 27 oC is k = 7.27e-30 s-1. Suppose we start with 0.0845 mol of C2H5Cl in a volume of 4.9 L. How many moles of C2H5Cl will remain after 1.24e+27 min?
The values of the rate constant for the A→Products reaction are given in the table below with the change of temperature. Find the activation energy for this reaction. k 0.027 0.040 0.059 0.085 0.12 0.17 0.24 t (oC) 1 6 11 16 21 26 31
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Initial-rate data at a certain temperature is given in the table for the reaction SO₂Cl₂(g) SO₂(g) + Cl₂(g) [SO₂Cl₂], (M) k= 0.100 0.200 0.300 Initial rate (M/s) 2.00 x 10-6 4.00 x 10-6 6.00 x 10-6 Determine the value and units of the rate constant. units:
The temperature dependence of the rate constant for the gas-phase reaction are as follows 2 N₂Os(g) Temperature (°C) K(s¹) 2.0 × 10 7.3 × 10-' 2.7 × 10 - 9.1 × 10 2.9 × 10-¹ Determine the values of activation energy (Ea) and frequency factor (A) for this reaction 20 30 40 50 60 4NO2(g) + O2(g) a. Activation energy = 1.22 kJ/mol and frequency factor = 2.14E+13 b. Activation energy = 101.21 kJ/mol and frequency factor = 30.70 c. Activation energy = 101.21 kJ/mol and frequency factor = 2.14E+13 d. Activation energy = 1.22 kJ/mol and frequency factor = 30.70 What is the volume at the equivalence point volume? a. 50.001 b. 50.000 IC 50.011 49.932 le 49.861 Clear my choice Liptoad YOUR eacel für showing all work
2 YO2 (g) + X2 (g) → 2 YO₂X (g) = -218 kJ/mol reaction AH rxn The reaction is first-order with respect to YO2 and first-order with respect to X₂. What is the relationship between the rate constant and activation energy of a chemical reaction?|

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