The half-life for the reaction below was determined to be 2.14 x 104 s at 800. K. The value of the half-life is independentN₂O present. The activation energy of the reaction is 248.0 kJ/mol.N₂O(g) →→→→ N₂(g) + O(g)1st attemptWhat would be the half-life at 1050.1 K?SSee Periodic TableSUBMIT ANSWE

Answered: Image /qna-images/answer/899273e7-7364-41dd-b4c3-9fb5b5738ee0.jpg

The half-life for the reaction below was determined to be 2.14 x 104 s at 800. K. The value of the half-life is independent U N₂O present. The activation energy of the reaction is 248.0 kJ/mol. N₂O(g) →→→ N₂(g) +0(g) 1st attempt What would be the half-life at 1050.1 K? See Periodic Table

The half-life for the reaction below was determined to be 2.14 x 104 s at 800. K. The value of the half-life is independent U N₂O present. The activation energy of the reaction is 248.0 kJ/mol. N₂O(g) →→→ N₂(g) +0(g) 1st attempt What would be the half-life at 1050.1 K? See Periodic Table

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 following data were collected for the reaction between hydrogen and nitric oxide at 700°C. 2 H2(g) + 2 NO(g) - 2 H20(g) + N2(g) Experiment [H2]/M [NO]/M Initial rate/M-s-1 0.012 0.031 4.5x10-6 0.0060 0.031 2.2x10-6 3 0.012 0.0155 1.1x10-6 (a) What is the rate law for the reaction? (Rate expressions take the general form: rate = k. [A]ª . [B]b.) chemPad Help Greek - (b) Calculate the rate constant for the reaction. 4.0 (c) Suggest a plausible reaction mechanism that is consistent with the rate law. (Hint: Assume that the oxygen atom is the intermediate. Omit states-of-matter from your answer.) First step: chemPad Help Greek - Second step: chemPad Help Greek
3. The rate equation for the decomposition of N,Os(g) (forming NO2(g)) is: A[NO2]/At = k[N;Os]. The value of k is 5.0 × 104 s-1 for the reaction at a particular temperature. a) Calculate the half-life of N2O5(g) at that temperature. b) How long does it take for [N½O5] to decrease to one tenth of its original value?
Suppose you are studying the kinetics of the reaction between nitrogen monoxide and hydrogen gas. You perform the reaction multiple times with different starting concentrations and measure the initial rate for each, resulting in this table. Experiment [NO] (M) [H2] (M) Initial Rate (M/s) 1 0.0050 0.0020 1.25 x 10–5 2 0.010 0.0020 5.00 x 10–5 3 0.0050 0.0040 2.50 x 10–5 Based on the data, choose the correct exponents to complete the rate law. rate=k[NO]x[H2]y x=? y=?
The reaction A → B + C is known to be zero order in A with a rate constant of 5.2 × 10–2 mol/L • s at 25° C. An experiment was run at 25°C where [A]0 = 3.2 × 10–3 M. What is the half-life for the reaction? A) 1.3× 101 s B) 2.6× 10–2 s C) 8.3× 10–2 s D) 6.0× 104 s E) 3.1× 10–2 s
See attached image for question A.) What is the order of the reaction in A? B.) What is the rate of reaction when the initial concentrations are [A]= 0 M and [B]= 4.4x 10-2M?
Dinitrogen pentoxide decomposes via a first order reaction. Rate = K[N₂O5], k = 6.93 x 10°3 s-1 The concentration of N₂O5 is initially 0.500 mol/L. After 100 s it has dropped to 0.250 mol/L and after 200 s it has dropped to 0.125 mol/L. What is the concentration after 150 s? HOW DO WE GET THERE? Use the first order concentration-time equation to determine [N₂O5] remaining after 150 s. [N₂05]t = 150 X mol/L
17. SHOW ALL YOUR WORK OGiven the following data, determine the order of the reaction with respect to NO(g). 2 NO(g) + Cl2(g)→ 2 NOCI(g) Experiment 1 [C2] (M) 0.0100 [NO] (M) Rate (M/s) 3.4 x 104 1.36 x 103 3.4 x 104 0.0300 0.0150 0.0150 0.0100 3 0.0400
The reaction 2 NO (g) + O2 (g) → 2 NO2 (g) occurs when automobile exhaust releases NO into the atmosphere. Use the following data to determine the order with respect to NO for this reaction. Trial [NO] (M) [O2] (M) Initial Rate (M/s) 1 0.012 0.020 1.02 x 10-4 2 0.024 0.020 4.08 x 10-4 3 0.024 0.040 8.16 x 10-4 Enter the answer as a single digit, not the word.
Nitesh
A particular reactant decomposes with a half-life of 103 s when its initial concentration is 0.275 M. The same reactant decomposes with a half-life of 211 s when its initial concentration is 0.134 M. Determine the reaction order. 1 What is the value and units of the rate constant for this reaction? Units k = M-1.s-1 M·s-1 M-2.s-1
The given first-order reaction A → B, has a rate constant of 1.60 x 10-2 s-1 at 165oC and 6.54 x 10-1 s-1 at 295oC. What is the activation energy for the reaction? 59.0 kJ/mol 650. kJ/mol 11.5 kJ/mol 0.582 kJ/mol
Molecular iodine, I2 (g), dissociates into iodine atoms at 652 K, with a first order rate constant of 0.452 s-1. I2(g) -----> 2I a. What is the half life for this reaction? b. If you start with 0.35 M I2 at this temperature, how long will it take for the concentration of I2 to reach 0.12 M?