(a) Determine the order of the decomposition of N2O5 using the table below, and according to the following balanced chemical equation:2N2O5 (g) → 2N2O4 (g) + O2 (g)1Time (s)[N2O5] (M)In [N2O5][N2O5]0.1000-2.30310.0500.0707-2.6514.11000.0500-3.0020.02000.0250-3.6940.03000.0125-4.3880.04000.00625-5.08160.(b) How did you come to this conclusion?(c) Determine the rate constant for the reaction.(d) If this reaction is run in the laboratory under the same conditions, but the initial concentration of N2O5 is 0.375M, what will the concentration ofit be after 3 min (180) s?(e) What is the half-life of N2O5 in these reactions?(f) What is the half-life of N2O5 in its decomposition under different conditions, in which it has a rate constant (k = 7.8 × 10-³s)?B I U AAIxx X, E E12ptParagraphP fr

(a) The concentration on which the rate of reaction actually depends is known as order of…

a) Determine the order of the decomposition of N2O5 using the table below, and according to the following balanced chemical equation: → 2N2O4 (9) + O2 (g) In [N2O5] 2N2O5 (g) Time (s) [N2O5] (M) [N2O5] 0.1000 -2.303 10.0 50 0.0707 -2.65 14.1 100 0.0500 -3.00 20.0 200 0.0250 -3.69 40.0 300 0.0125 -4.38 80.0 400 0.00625 -5.08 160. Cb) How did you come to this conclusion? c) Determine the rate constant for the reaction.

a) Determine the order of the decomposition of N2O5 using the table below, and according to the following balanced chemical equation: → 2N2O4 (9) + O2 (g) In [N2O5] 2N2O5 (g) Time (s) [N2O5] (M) [N2O5] 0.1000 -2.303 10.0 50 0.0707 -2.65 14.1 100 0.0500 -3.00 20.0 200 0.0250 -3.69 40.0 300 0.0125 -4.38 80.0 400 0.00625 -5.08 160. Cb) How did you come to this conclusion? c) Determine the rate constant for the reaction.

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

Determine half-life, order, and k from concentration-time data. The following data were collected for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g)-CH₂(g) + H₂(g) + CO(g) [CH3OCH 3], M 7.02x10-² time, min 0 3.51x10-2 22.20 K 1.76x10-² 44.40 8.80×10-3 66.60 (a) What is the half-life for the reaction when [CH3OCH3] = 7.02x10-² M? (b) What is the half-life for the reaction when [CH3OCH3] = 3.51x10-² M? (c) Is the reaction first order? If so, what is the rate constant for the reaction? (If not first order leave blank). min min min-1
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
The reaction A(aq) → B(aq) is a reaction of order one with respect to A(aq). Theconcentration of A(aq) after 100.0 s of reaction is 0.477 M. The concentration of A(aq) afteranother 300.0 s (so 400.0 s in total) is 0.277 M. What was the initial concentration ofA(aq)? The temperature is always 25.0◦C
The decomposition of nitrosyl bromide is followed 2 NOBr → 2 NO + Br2 Time (s) [NOBr] (M) 0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00 0.0033 Determine the average rate over the entire experiment.
Consider the reaction and the information in the table provided. Calculate the average rate of formation of P2O5 between 20.0s and 40.0s. 2H3PO4 → P2O5 + 3H2O Time (s) 0.0 10.0 20.0 30.0 40.0 50.0 Conc P2O5 (M) 0 0.00120 0.00420 0.00600 0.00720 0.00780
The following kinetic data were collected at 298 K for the reaction of ozone with nitrite ion, producing nitrate and oxygen: NO, (aq) +O,(g) NO, (aq) +0,(g) > Experiment [NO2 lo (M) [O3lo (M) Initial Rate (M/s) 1 0.0100 0.0050 25.0 0.0150 0.0050 37.5 3 0.0200 0.0050 50.0 0.0200 0.0200 200.0
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.
The following data were obtained for the reaction 2A → B: Time, min TA], mol/L 0.0962 0.0398 0.0156 10 20 40 60 80 0.0059 0.000428 0.000061 0.000009 (i) By plotting a suitable graph, determine the order of this reaction. (i) Calculate the rate constant of the reaction.
The following mechanism has been proposed for the atmospheric destruction of ozone, O3 (g):O3 (g) + NO (g) --> O2 (g) + NO2 (g) (slow)NO2 (g) + O (g) --> NO (g) + O2 (g) (fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.
The overall reaction of ozone reacting to form oxygen has been proposed to occur in a reaction mechanism of: Step 1: O3(g)-→O2(g) + O(g) Step 2: O3(g) + O(g) →202(g) What is the role of O(g) and what is the overall balanced equation? Periodic Table and Datasheet Select one: O a. O(g) is an intermediate; 203(g) + O(g) →302(g) + O(g) O b. O(g) is a catalyst; 203(g) + O(g)→302(g) + O(g) O c. O(g) is an intermediate; 203(g) → 302(g) O d. O(g) is a catalyst; 203(g)→302(g) Which statement best describes general equilibrium?
The following mechanism has been proposed for the reaction of H2 (g) and NO (g): H2 (g) + NO (g) → H2O (g) + N (g) (Slow)N (g) + NO (g) → N2 (g) + O (g) (Fast)H2 (g) + O (g) → H2O (g) (Fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.
c) Calculate its half-life 2. The following data were obtained for the gas-phase decomposition of dinitrogen pentaoxide 2N,O, (g) 4NO, (g) +0; () IN,OJ, (mol / L.) Initial Rate (mol /Ls) 0.0750 8.90 x 104 0.190 2.26 x 10 0.275 3.26 x 10 0.410 4.85 x 10 Defining the rate as -A [N;OJ/A write the rate law and caiculate the value of the rate constant