11. An experiment followed the decomposition of nitrogen dioxyde te nitrogen monoxide & oxygen gas. Given the following data, what order is the reaction for nitrogen dioxide? Given an initial concentration of nitrogen dioxide of 0.0400 M, what's the concentration of this reactant after a half hour? show all grapers & calcs to determine answers. (sec) Time |CN0₂] (M) 0,0 50.0 100.0 200.0 300.0 0.01000 0.00787 0.00649 0.00481 0.00380 M A(9) # *#I(9)

11. An experiment followed the decomposition of nitrogen dioxyde te nitrogen monoxide & oxygen gas. Given the following data, what order is the reaction for nitrogen dioxide? Given an initial concentration of nitrogen dioxide of 0.0400 M, what's the concentration of this reactant after a half hour? show all grapers & calcs to determine answers. (sec) Time |CN0₂] (M) 0,0 50.0 100.0 200.0 300.0 0.01000 0.00787 0.00649 0.00481 0.00380 M A(9) # *#I(9)

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

Use this data for the following four (4) questions: The relative initial rates of the reaction A2 + B2-products in vessels (a)-(d) are 1:1:4:4. The spheres represent the number of molecules of present at the beginning of the reaction. [Unshaded spheres = A2 molecules; shaded spheres = B2 molecules] %3D For example, vessel (a) contains 2 A2 molecules and 2 B2 at the beginning of the reaction. Rate = 1 Rate 1 Rate = 4 Rate = 4 %3D 2. 8. 80 (c) (a) 11) What is the order of reaction with respect to A2? (b) (d) BA 11) A))0 B) 1 C) 2 D) 3 12) What is the order of reaction with respect to B2? 12) C A) 0 B) 1 D) 3 13) o c 13) What is the overall order of reaction? A) 0 B) 1 D) B 14) 14) What is the rate law for this reaction? B) Rate k[B2]2 D) Rate = k[A2]2[B2]² A) Rate = k[A2]² %3D C) Rate = k[A2][B2] %3D %3D nation below: 15) 8. 8.
Please show all steps
Pleas don't handwritten solution ...
1 of 1 Assignment 3 (NCHE312) The total pressure of the following system is used to monitor the progress of the chemical reaction. SO₂Cl₂(g) → SO2(g) + Cl₂(g) The reaction is initiated, and the following data are obtained: Time (h) PTotal (kPa) Pso₂cl₂ Ps0₂ Pclz 0 11.07 3 6 14.79 17.26 9 18.90 12 19.99 15 20.71 Additional information: As the reaction proceeds, stoichiometry dictates that for every mole of SO₂Cl₂ that dissociates one mole of each of SO₂ and Cl₂ is produced. Defining the extent of dissociation/reaction as E, and the initial pressure as Po, the total pressure is given by: Ptotal = Pso₂Cl₂ + Pso₂+ Pcl₂ = (Po-5)+5+5 Convert your work into a single PDF file and upload it into your eFundi Dropbox folder. Deadline for submission: 26/05/2023 at 12pm a) Calculate the pressure of each component at each time interval, i.e. complete the above table. b) Use a graphical method and determine what the order of the reaction is with respect to SO₂Cl₂? (i) Show the plot as well as the…
Consider the hypothetical reaction 4A + 3B – 2C + D A certain amount of A and B was placed in a container and the reaction was allowed to proceed. The initial concentration of the products is zero. Over an interval of 1.5 s the average rate of change of the concentration of B was measured to be -0.0800 M/s. What is the concentration of D at the end of this same interval. 0.10 M 0.04 M 0.02 M 0.12M O O O
Consider this reaction: →H2CO3aq+H2OaqCO2aq At a certain temperature it obeys this rate law.rate =·0.0579M−1s−1H2CO32 Suppose a vessel contains H2CO3 at a concentration of 0.820M. Calculate the concentration of H2CO3 in the vessel 280.seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. =___M
The reaction described by the equation 0,(g) + NO(g) - O2(g) + NO, (g) > has, at 310 K, the rate law rate of reaction k[O,][NO] k = 3.0 x 106 M-1.s-1 Given that [O,] = 2.0 × 10-4 M and [NO] = 4.0 × 10-³ M at t = 0, calculate the rate of the reaction at t = 0. rate: M/s What is the overall order of this reaction? 2 3 1
General Chemistry II- Ara Sinavi 13 According to the data given below calculate k and t1/2. For the hypothetical aqueous reaction: A B, the concentration change of A was monitored and several derived data were tabulated and two different plots were obtained. Based on these given plots and data: time(min) [A] (M) In[A] V [A] -0.2 0.65 -0.43 1.5 --0.4 10 0.51 -0.67 2.0 -0.6 S -0.8 20 0.42 -0.87 2.4 -1.0 30 0.36 -1.02 2.8 Карat
Subject-advance chemistry
Please and thank you ?
For the simple decomposition reaction: AB(g) A(g) + B(g), the rate = k{AB}? ({ = [) and k = 0.78 1/M•s. How long (in seconds) will it take for the concentration of AB to reach one-third of its initial concentration of 1.07? Enter to 2 decimal places.