In a study of the decomposition of nitrous oxide at 565 °C N₂O(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 = 1.50×10³ s is The average A(1/[N₂0])/ At from t = 1.50x10³ s to t = 4.47×10³ s is (3) Based on these data, the rate constant for this 9.40x10-2 1.04x104 M-1 S-1 order reaction is M-1 S-1. M-1 S-1. s and when the starting

In a study of the decomposition of nitrous oxide at 565 °C N₂O(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 = 1.50×10³ s is The average A(1/[N₂0])/ At from t = 1.50x10³ s to t = 4.47×10³ s is (3) Based on these data, the rate constant for this 9.40x10-2 1.04x104 M-1 S-1 order reaction is M-1 S-1. M-1 S-1. s and when the starting

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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The rate constant for this first‑order reaction is 0.480 s−10.480 s−1 at 400 ∘C.400 ∘C. A⟶products How long, in seconds, would it take for the concentration of A to decrease from 0.690 M to 0.290 M?
6) The decomposition of reactant R was studied, and the data given below was obtained at 100.0 °C: R> products time (min) concentration (M) 0.120 35.6 5.83 17.8 25.6 0.0910 0.060 0.046 0.030 a) What is the half-life of the reaction in minutes? Explain. b) Various plots of the concentration of the reactant versus time are given below. What is the order of the reaction? Explain. ILD is 20 time (min) time (min) 05 -35 time (min) c) What is the value of the rate constant at 100.0 °C? d) Would you expect the half-life of the reaction to be longer, shorter, or the same at 60.0 °C? Explain. e) The activation energy in the forward direction is 95.0 kl/mol, and the enthalpy change for the forward reaction is 30.0 kl/mol. Sketch the reaction coordinate diagram for this reaction. ERER AR
At a certain temperature the rate of this reaction is first order in NH,OH with a rate constant of 0.00777 s : NH,OH (аq) — Nн; (ад) +н,о (аq) Suppose a vessel contains NH,OH at a concentration of 0.750M. Calculate the concentration of NH,OH in the vessel 87.0 seconds later. You may assume no other reaction is important. olo Round your answer to 2 significant digits. Ar | M x10
At a certain temperature the rate of this reaction is first order in N₂O5 with a rate constant of 0.0125 s¯¹: 2N₂O5 (g) → 2N₂O4 (8) + 0₂ (8) Suppose a vessel contains N₂O5 at a concentration of 1.14M. Calculate the concentration of N₂O5 in the vessel 88.0 seconds later. You may assume no of reaction is important. Round your answer to 2 significant digits.
The following data are for the decomposition of nitramide in aqueous solution at 25 °C. NH,NO2(aq) → N20(g) + H20(1) [ NH2NO2 ], 0.802 0.401 0.201 0.101 M time, min 175 350 525 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 O order reaction is min -1
Determine the order of the reaction and the value of the rate constant. Having trouble figuring out how to use the half life's to figure out the order of the reaction.
In a study of the decomposition of nitrosyl bromide at 10 °CNOBrNO + ½ Br2the following data were obtained: [NOBr], M 0.249 0.125 6.25×10-2 3.13×10-2 seconds 0 6.16 18.5 43.2 Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 0.249 M is s and when the starting concentration is 0.125 M is s.(2)The average (1/[NOBr]) / t from t = 0 s to t = 6.16 s is M-1 s-1.The average (1/[NOBr]) / t from t = 6.16 s to t = 18.5 s is M-1 s-1.(3)Based on these data, the rate constant for this order reaction is M-1 s-1.
Please provide the step by step solution for the question attached. Graphics must be included. Please make sure the graphics are visible.
In a study of the decomposition of hydrogen iodide on a gold surface at 150 °CHI(g)½ H2(g) + ½ I2(g)the following data were obtained: [HI], M 0.573 0.287 0.144 7.20×10-2 seconds 0 520 781 912 Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 0.573 M is s and when the starting concentration is 0.287 M is s.(2)The average rate of disappearance of HI from t = 0 s to t = 520 s is M s-1.(3)The average rate of disappearance of HI from t = 520 s to t = 781 s is M s-1.(4)Based on these data, the rate constant for this _______zerofirstsecond order reaction is M s-1.
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 1.48 0.740 0.370 0.185 750 2.25x103 5.25x103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.48 M is 750 s and when the starting concentration is 0.740 M is 1500 S. (2) The average A(1/[HI]) / At from t = 0 s to t = 750 s is M-1 s-1. The average A(1/[HI]) / At from t 750 s to t = 2.25×103 s is M-1 s-1. (3) Based on these data, the rate constant for this 0 order reaction is M-1 s-1.
Consider the following initial rate data (at 279 K) for the decomposition of a substrate (substrate 1) which decomposes to product 1 and product 2: [Substrate 1] Initial Rate 0.1 0.2 (M) (M/s) 0.00901 0.03604 0.6 0.32436 Determine the half-life for the decomposition of substrate 1 when the initial concentration of the substrate is 2.74 M.