6.) The rate law for the reaction below is found experimentally to be Rate = k[N2O5] and the rate constant, k = 6.20 × 10s-. SHOW ALL WORK! %3D 2 N2O5 (g) → 4 NO2 (g) + O2 (g) a. Determine the time for the concentration of N2O5 to go from 0.400 M to 0.200 M. b. if [N2O5]o = 0.400 M, calculate [N2O5] at t = 60.0 min.

6.) The rate law for the reaction below is found experimentally to be Rate = k[N2O5] and the rate constant, k = 6.20 × 10s-. SHOW ALL WORK! %3D 2 N2O5 (g) → 4 NO2 (g) + O2 (g) a. Determine the time for the concentration of N2O5 to go from 0.400 M to 0.200 M. b. if [N2O5]o = 0.400 M, calculate [N2O5] at t = 60.0 min.

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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8. For the reaction: 2 N,O5 (g) → 4 NO2 (g) + O2 (g) the rate law is: Rate = k[N2O5] The activation energy of the reaction is 103.3 kJ mol-1. At 300 K, the half-life of the reaction is 2.50 × 104 seconds. At what temperature is the half-life 4.00 x 102 seconds? A) 278 K В) 333 K С) 3.04 K D) 304 K E) 296 K
Consider the following kinetic data for the reaction: 2NO + 2H2 --> N2 + 2H2O. [NO]0, M [H2]0, M Initial Rate (mol.L–1 ‧ s–1)___ 0.10 0.10 1.23 x 10–3 0.10 0.30 3.68 x 10–3 0.30 0.10 1.11 x 10–2 ——————————————————————————— What is the rate law for this reaction? (A) Rate = k[NO]2[H2]2 (B) Rate = k[NO]2[H2] (C) Rate = k[NO][H2] (D) Rate = k[NO][H2]2
O Name.p ane.CREE! 1. Dinitrogen pentoxide, N₂O5, decomposes via the following reaction: 2N₂O5(8) →→→ 4NO₂(g) + O₂(8) -1 Using to the data recorded in the table below for the reaction, determine the average rate of the decomposition of the reactant (in M s to two decimal places) during the first 200 s. In addition, determine the rate of change for [NO₂] (in M s -¹ to two decimal places) over the same time interval. -1 0.0200 0.0169 0.0142 0.0120 0.0101 Help Pag Time (s) N₂O5 (M) NO₂ (M) O₂ (M) 0 0 0 100 0.0063 0.0016 200 0.0115 0.0029 300 0.0160 0.0040 400 0.0197 0.0049 A: 2.90 × 10-5; 5.80 × 10-5
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k for some reaction is 1.21×10−4 s-1 at 26∘C and 0.227 s-1 at 79∘C A. What is the Ea for this reaction? (Express your answer in units of kilojoules per mole and with 3 significant figures. ) B. What is the value of the rate constant at 16∘C (Express your answer in units of inverse seconds (s−1) and with 3 significant figures.)
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I could use help with #2
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