### Kinetics Study of a Chemical ReactionThe rate of a certain reaction was studied at various temperatures. The table shows temperature (\(T\)) and rate constant (\(k\)) data collected during the experiments. Plot the data to answer the questions.| \(T\) (K) | \(k\) (s\(^{-1}\)) ||-----------|---------------------|| 400 | 0.000108 || 420 | 0.000626 || 440 | 0.00310 || 460 | 0.0134 || 480 | 0.0511 || 500 | 0.175 || 520 | 0.547 || 540 | 1.57 || 560 | 4.18 || 580 | 10.4 |#### Questions:1. **What is the value of the activation energy, \( E_a \), for this reaction?** \[ E_a = 1108.79 \text{ kJ} \cdot \text{mol}^{-1} \] *Incorrect*2. **What is the value of the pre-exponential factor (sometimes called the frequency factor), \( A \), for this reaction?** \[ A = 6.79 \times 10^{140} \text{ s}^{-1} \] *Incorrect*

Arrhenius Equation based Numerical

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 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

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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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- 0.36 20 20 0.43 0.32 40 40 0.35 0.28 60 60 0.29 0.24 88 80 0.23 0.20. 0.16. 100 0.19 The blue curve is the plot of the data. The straight orange line is tangent to the blue curve at t = 40 s. Approximate the instantaneous rate of this reaction at time t = 40 s. instantaneous rate: M/s 0 10 20 30 40 50 60 70 80 90 100 t(s)
use/make a graph since there is 5 data points
1. In the Rates of Chemical Reactions lab you measured the experimental rate of the following reaction: S208 +212 +2 SO4² Given a graph of moles S₂Og 2 consumed versus time (s) with a best fit linear line and a total volume of 325 mL for the reaction, explain how would you determine the rate of reaction? 2. The initial rates listed in the following table were determined for the reaction: H2PO3 (aq) + OH (aq) →HPO3²¯ (aq) + H2O (1) Trial Initial [H₂PO3¯], (M) Initial [OH], (M) Initial Rate of Consumption (M/s) 1 0.025 0.030 0.432 2 0.100 0.030 1.728 3 0.100 0.015 0.864 a) What is the rate law? b) What is the value of the rate constant, k? c) What is the initial rate when the initial concentrations of both reactants are 0.12 M? 3. The following experimental data was obtained for the bromination of acetone at 30°C. 21 +2 H+H2O2 → I2 + 2 H₂O Trial Initial [I] (M) Initial [H+] Initial [H2O2] (M) Rate (M/sec) (M) 1 0.001 0.005 0.001 2.0 x 104 2 0.002 0.005 0.001 4.0 x 10+ 3 0.006 0.002 0.001…
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General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning Initial-rate data at a certain temperature is given in the table for the reaction N,0,(g) NO(g) + NO,(g) [N,O,], (M) Initial rate (M/s) 0.100 0.480 0.200 0.9600 0.300 1.440 Determine the value and units of the rate constant. units: k =