The rate of the reaction N₂O5(g) →2 NO₂(g) + 1/2 0₂(g) is measured at different temperatures, with the following rate constants, k, determined: Temperature, K 298 328 358 378 Recheck k, s-1 1st attempt 3.46 x 10-5 1.5 x 10-3 3.34 x 10-2 0.21 Use the graphing tool above to make an appropriate plot and determine the activation energy, E, for this reaction in units of kilojoules_ X kJ/mol 4 Next) (1 of 1) Show Approach Select functions for the x-axis and the y-axis and create the plot that can be used to find the activation energy. The Arrhenius equatic Ea F/R (1) In k = In A - Inc y=b+mx

The rate of the reaction N₂O5(g) →2 NO₂(g) + 1/2 0₂(g) is measured at different temperatures, with the following rate constants, k, determined: Temperature, K 298 328 358 378 Recheck k, s-1 1st attempt 3.46 x 10-5 1.5 x 10-3 3.34 x 10-2 0.21 Use the graphing tool above to make an appropriate plot and determine the activation energy, E, for this reaction in units of kilojoules_ X kJ/mol 4 Next) (1 of 1) Show Approach Select functions for the x-axis and the y-axis and create the plot that can be used to find the activation energy. The Arrhenius equatic Ea F/R (1) In k = In A - Inc y=b+mx

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

The data given in the table below is for the following reaction (run at 25°C): 2 NO + O, 2(g) → 2 (g) 2(g) Initial Concentration (M) Initial rate Experiment NO 0, Mol/(L · s) 1 0.0010 0.0010 7 x 10-6 2 0.0010 0.0020 14 x 106 3 0.0010 0.0030 21 x 10-6 4 0.0020 0.0030 84 x 10-6 5 0.0030 0.0030 189 x 106 1. Determine the orders of the reaction with respect to NO and O, (show all work): NO
A reaction between substances A and B has been found to give the following data: 3A +2B 2C+D Al (mol/L) (mol/Rate of appearance of C 10 x 102 10 x 102 30 2.0 x 102 30 mol / L-hr) 0.300 x 100 810x 10 3 24 x 10-5 1.20 x 10-8 30 x 10-5 10 0 x 102 1.0 3.0 x 10- Using the above data, determine: a) the order of the reaction with respect to A and B - b) the rate law, and - c) calculate the specific rate constant
Some measurements of the initial rate of a certain reaction are given in the table below. [¹₂] 0.945M 1.74M 0.945 M 0.395M 0.458M 1.74M Use this information to write a rate law for this reaction, Round your value for the rate constant to 2 significant di rate = k H₂ initial rate of reaction 1.00 × 106 M/s 5.15 × 10¹ M/s 4.85 × 105 M/s [N₂] [H₂] k = 3.50 x 10 - 5 - 2 M S - 1 x10 • X 5 Be Careful Your answer should be a number followed by a unit. OK ol.
The progress of a reaction is tracked by following the concentration of one reactant as it is consumed. The table gives the concentration of that reactant at several times. Time (s) [R] (mol/L) 5.00 × 10-3 4.32 × 10-3 3.66 × 10-3 3.03 × 10-3 2.44 x 10-³ 1.90 x 10-³ 1.39 × 10-3 0 10.5 22.3 35.7 51.1 69.3 91.6 120.4 160.9 230.3 299.6 -4 9.27 x 107 5.26 x 10-4 1.99 x 10-4 7.54 x 10-5 a Use graphing software to plot the data as [R] versus time, and determine the average rate for the first 15 s and the average rate from t = 100 to t = 125 s. Enter the rates as positive values. Rate (from t = 0 tot = 15 s) = Rate (from t = 100 to t = 125 s) = M/s M/s Previous Next
Consider this reaction: H,CO, (ag) – H,0 (aq) + CO, (ag) At a certain temperature it obeys this rate law. rate = (9.70 x 10-4s)H,co,] Suppose a vessel contains H,CO, at a concentration of 0.470 M. Calculate the concentration of H,CO, in the vessel 680. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. x10
The kinetic data shown below were observed for the reaction: BF3 (g) + NH3 (g) ---------> F3B·NH3 (g) Trial # [BF3] (mol/L) [NH3] (mol/L) Rate (M/s) 1 0.250 0.250 0.2130 2 0.250 0.125 0.1065 3 0.200 0.100 0.0682 4 0.350 0.100 0.1193 5 0.175 0.100 0.0596 What is the rate constant for this experiment?
The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, k, of a particular gaseous reaction as 9.90 × 10-10 cm³ molecule-¹.s-¹ at 298 K. Convert the rate constant to units of M-¹.s-¹. k = k = Incorrect Convert the rate constant to units of Torr-¹.s-¹. 5.962 ×10¹7 Incorrect 2 3.208 ×10¹7 What is the order of this reaction? 0 M-¹.s Torr-g
Calculate the average rate of a reaction, given the following data: Reaction Data Time (s) Concentration (mol/L) 60 5.00 × 10-² 85 3.25 x 10-²
Some measurements of the initial rate of a certain reaction are given in the table below. H2||2| initial rate of reaction 0.554M| 1.43M 2.00 M/s 1.05 M 1.43 М 3.79 M/s 0.554M 4.76M 6.66 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate k I x10 k =
Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g) + O2(g) → 2 NO₂(g) [NO]i (M) [0₂]i (M) 0.030 0.030 0.060 A) Rate = 57 M-1s-1 [NO][0₂] B) Rate = 3.8 M-1/2-1[NO][0₂]¹/2 C) Rate = 3.1 x 105 M-³s-1 [NO]²[0₂]² D) Rate = 1.7 × 103 M-2s-1 [NO]²[0₂] E) Rate = 9.4 × 103 M-²s-1 [NO][0₂]² 0.0055 0.0110 0.0055 Initial Rate (M-1,-1) 8.55 × 10-3 1.71 × 10-2 3.42 × 10-2
Q1
O KINETICS AND EQUILIBRIUM Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. N2 H2 initial rate of reaction |2.44 М 0.652м 9.00 x 10°M/s 2.44 M 0.296 М 1.85 x 10°M/s 9.86 M 0.652м 3.64 x 10*M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k|| |• 0 k =