TirIn a particular experiment, it was found that the concentration of N₂O5 in liquid brewith time as follows:2 N₂O5(g)4 NO2(g) + O2(g)1[N₂05] 0.110Time (s)a 2.2073Calculate the value of the rate constant (k)b. 0.0623C.0.0962d 9E-05e. 1.8502f. 0.0021For the reaction,2N₂O5(g)Time0100300600900The following data were obtained:T = 339 K[N₂O), Ma. 45.8 kJ/mol0b. 120.6 kJ/molC.112.5 kJ/mold. 95.7 kJ/mole. 68.5 kJ/mol200 400 60010000.073 0.048 0.032 0.014f.89.7 kJ/mol4NO2(g)1.00 × 106.14 102.33 1075.41- 10¹1.26 × 10+Find the Ea using the best-fit straight line of the three rate constants at the three temperaturevalues.O2(g)T = 310 K[N₂O.]. M1.00 × 109.54 × 108.6310²7.43 106.39 × 10T = 304 K[N₂O₁]. M1.00 × 109.69 × 109.15 108.40 - 107,70 10-

Answer: From drawn graph it has been confirmed, the reaction is of first order. Reacion rate…

In a particular experiment, it was found that the concentration of N O; in liquid bre Tir with time as follows: 2 N₂O5(g) 4 NO2(g) + O2(g) Time (s) [N₂O5] a. 2.2073 b. 0.0623 Calculate the value of the rate constant (k) C. 0.0962 d. 9E-05 e. 1.8502 |0.110 f. 0.0021 200 400 600 0.110 0.073 1000 0.048 0.032 0.014

In a particular experiment, it was found that the concentration of N O; in liquid bre Tir with time as follows: 2 N₂O5(g) 4 NO2(g) + O2(g) Time (s) [N₂O5] a. 2.2073 b. 0.0623 Calculate the value of the rate constant (k) C. 0.0962 d. 9E-05 e. 1.8502 |0.110 f. 0.0021 200 400 600 0.110 0.073 1000 0.048 0.032 0.014

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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Nn.77. Subject :- Chemistry
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T
Please provide the step by step solution for the question attached. Graphics must be included. Please make sure the graphics are visible.
A. Determine the order of the reaction and the value of the rate constant (must be done graphically, drawgraph in the space next to the table) B. For the data in number 1, Predict the concentration of N2O5 at 250 s.
The activation energy for the reaction of 2NO2(g) 2NO(g) + O2(g) has been determined to be 111 kJ∙mol–1. The rate constant at 300°C is 0.54 M–1∙s–1. What is the rate constant when the temperature is increased to 310°C? a. 0.00050 M –1∙s –1 b. 2.3 M –1∙s –1 c. 0.81 M –1∙s –1 d. 0.54 M –1∙s –1
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AMoving to another question will save this res Question 20 A graph that displays a straight line when the reciprocal of the concentration is plotted as a function of time. The graph has a slope of 0.482 and a y- intercept of 0.756. What is the rate constant? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation-examples include 1.23 and 12.3 and 120. and -123) Question 20 of 29 AMoving to another question will save this response PIL esc %23 %24 4 & 7. 8 delete R T. Y TO tab enter D. F K return caps lock C V elt control option command option
Chem q 5
23. The rate constant for decomposition of azomethane at 425°C is 0.68 s~', CH,N=NCH,(g) N;(g) + C,H(g) a) Based on the units of the rate constant, is the reaction zeroth-, first-, or second-order? b) If2.0 g azomethane is placed in a 2.0-L flask and heated to 425°C, what mass of azomethane remains after 5.0 s? c) How long does it take for the mass of azomethane to drop to 0.24 g? d) What mass of nitrogen would be found in the flask after 0.50 s of reaction?
The reaction of 2 N2O5(g) → 4 NO2(g) + O2(g) is experimentally determined to be fırst oder. What experimental data would support this conclusion? I. Plotting 1/[N2O5] vs. time would be linear. II. The half-life is independent of the initial concentration. III. Doubling the initial concentration of N205 would yield a quadrupled initial rate. Only I. Only II. II. and III. I. and III.
A particular reactant decomposes with a half‑life of 117 s117 s when its initial concentration is 0.376 M.0.376 M. The same reactant decomposes with a half‑life of 221 s221 s when its initial concentration is 0.199 M.0.199 M. Determine the reaction order. 2 1 0 What is the value and units of the rate constant for this reaction? ?=k= Units
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