In a study of the decomposition of ammonia on a platinum surface at 856 °CNH31/2 N2 + 3/2 H2the following data were obtained:NH3], M2.39x10-31.20×1039976.00x1041.50x1033.00x10-41.75x103secondsHint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 2.39x10-3 M iss and when the starting concentration is 1.20×10-3 M iss.(2)The average rate of disappearance of NH3 from t= 0 s to t= 997 s isMs!.(3)The average rate of disappearance of NH3 from t= 997 s to t= 1.50×103 s isMs-l.(4)Based on these data, the rate constant for this| order reaction isMs-1.

In a study of the decomposition of ammonia on a platinum surface at 856 °C NH31/2 N2 + 3/2 H2 the following data were obtained: NH3). M 1.20x10-3 997 3.00x104 1.75x103 2.39x10-3 6.00x104 1.50x103 seconds Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 2.39×10-3 M is s and when the starting concentration is 1.20x103 M is | (2) The average rate of disappearance of NH3 from t= 0s to t= 997 s is Ms! (3) The average rate of disappearance of NH3 from t= 997 s to t= 1.50×103 s is s!. (4) Based on these data, the rate constant for this | order reaction is

In a study of the decomposition of ammonia on a platinum surface at 856 °C NH31/2 N2 + 3/2 H2 the following data were obtained: NH3). M 1.20x10-3 997 3.00x104 1.75x103 2.39x10-3 6.00x104 1.50x103 seconds Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 2.39×10-3 M is s and when the starting concentration is 1.20x103 M is | (2) The average rate of disappearance of NH3 from t= 0s to t= 997 s is Ms! (3) The average rate of disappearance of NH3 from t= 997 s to t= 1.50×103 s is s!. (4) Based on these data, the rate constant for this | order reaction is

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

In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g) →½ H2(g) + ½ I2(g) the following data were obtained: HI], M seconds 1.01 0.505 0.253 0.127 1.05x103 3.15x103 7.32x103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.01 M is s and when the starting concentration is 0.505 M is S. (2) The average A(1/[HI]) / At from t= 0 s to t= 1.05x103 s is The average A(1/[HI]) / At from t= 1.05×103 s to t= 3.15×103 s is Ms!. (3) Based on these data, the rate constant for this order reaction is
For the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C 2 H202(aq)2 H20(1) + O2(g) the following data have been obtained: [H2O2], M 4.17x10-2 11.4 8.86x10-2 9.24x10-3 1.96×102 22.8 time, min 34.2 The average rate of disappearance of H,02 over the time period from t= 0 min to t= 11.4 min 1s M min-1.
In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H,(g) + % »(9) the following data were obtained: HI], M seconds 0.274 0.137 6.85×10-2 3.43x10-2 521 782 912 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.274 M is s and when the starting concentration is 0.137 M is (2) The average rate of disappearance of HI from t= 0s to t= 521 s is| Ms!. (3) The average rate of disappearance of HI from t= 521 s to t= 782 s is| Ms! (4) Based on these data, the rate constant for this | | order reaction is Ms!.
or the decomposition of nitrous oxide at 565 °C2 N2O2 N2 + O2the following data have been obtained: [N2O], M 1.48 0.463 0.274 0.195 time, s 0 22.5 45.0 67.5 The average rate of disappearance of N2O over the time period from t = 22.5 s to t = 45.0 s is M s-1.
The gas phase decomposition of dinitrogen pentoxide at 335 K 2 N205 →4 NO2+02 has the following relationship between rate and concentration, where the bracket around the formula indicates concentration and k is a constant called the rate constant. Rate = k[N2O5l %3D If the value of k is 7.38×10~$ s', what is the rate of the reaction when [N2O5] = 0.180 M? Ms-
For the decomposition of nitramide in aqueous solution at 25 °C NH,NO,(aq)N,0(g) + H2O(1) the following data have been obtained: NH,NO2], M 9.12x10-2 217 2.69x10-2 651 0.168 4.95x10-2 434 time, min The average rate of disappearance of NH,NO, over the time period from t = 0 min to t= 217 min is M min!.
The following data were obtained on the initial rates of a reaction of a d-metal complex in aqueous solution. What is (a) the order of reaction with respect to the complex and the reactant Y. (b) the rate constant? For the experiments (a) [Y] = 2. 7 mmol dm-3 and for experiments (b) ]Y] = 6.1 mmol dm-3[complex]/(mmol dm-3) 8.01 9.22 12.11v/(mol dm-3 s-1) (a) 125 144 190 (b) 640 730 960
Please ? and thank you ?
The following data are for the gas phase decomposition of sulfuryl chloride at 600 K. sO,C2(g)- - SO2(g) + Cl2(g) [ SO;Clz ], M 2.89x103 1.45x103 7.25x104 3.63x104 time, min 168 336 504 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is | min. (2) Based on these data, the rate constant for this order reaction is min
In a study of the decomposition of nitrous oxide at 565 °C N2₂O(g) N₂(g) + ½ O₂(g) the following data were obtained: [N₂0], M seconds 0.750 0 0.375 1.50x10³ 0.188 4.47x10³ Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.750 M is concentration is 0.375 M is S. (2) The average A(1/[N₂0])/ At from t = 0 s to t = 1.50x10³ s is The average A(1/[N₂0])/ At from t = 1.50x10³ s to t = 4.47x103 s is (3) Based on these data, the rate constant for this 9.40×10-2 1.04x104 M-1 S-1. order reaction is M-1 S-1. M-¹ S-1. s and when the starting
A 1st order reaction takes place with k = 0.00528 s-1. If the initial [A] is 0.455 M, what is a) the half-life of the reaction; b) [A] after 215 seconds? O t1/2 = 131 s; [A] = 0.299 M %3D t1/2 = 189 s; [A] = 0.146 M %3D t1/2 = 95 s; [A] = 0.401 M %3D O t1/2 = 131 s; [A] = 0.146 M. = 131 s; [A] = 0.033 M
Please don't provide handwritten solution ....