age 1:1.8140 14.001120 --4.25100 --4.50-80 -Page 2:4.75-0.8600.6-S.0012234 S2 346Time (s) X 10Time (s) x 10Time (s) X10Page 3:Which of the following graphs, 1st. 2nd, or 3rd shows a correctly graphed data set3for a second order reaction?Page 4:3rd41stnone of these2nd01 x (W) PH5

From the graph we can get the idea about the order of the reaction .

4.00 140 1.6 120 -4.25 1.4 100 1.2 -4 50 80 1.0 4.75 0.8 60 0.6 -5.00 o1 2 3 Time (s x10 2. 3. 15 6. Time (s) X 10' Time (sx to Which of the following graphs, 1st. 2nd, or 3rd shows a correctly graphed data set for a second order reaction? 3rd 1st none of these O2nd

4.00 140 1.6 120 -4.25 1.4 100 1.2 -4 50 80 1.0 4.75 0.8 60 0.6 -5.00 o1 2 3 Time (s x10 2. 3. 15 6. Time (s) X 10' Time (sx to Which of the following graphs, 1st. 2nd, or 3rd shows a correctly graphed data set for a second order reaction? 3rd 1st none of these O2nd

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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For the reaction: 4NH3 (g) + 7O2 (g) → 4NO2 (g) + 6H2 (g), if H2 is produced at a rate of 3.5 x 10-3 M/s, O2 is consumed at a rate of... A. -2.5 x 10-2 M/s B. -4.1 x 10-3 M/s C. -2.1 x 10-2 M/s D. -3.0 x 10-3 M/s E. -5.8 x 10-4 M/s
Assignment 1. The reaction 2NO (g) t CL (g) 2NOCI (g) was studied at- 10 C. The following results were obtained where Rate =- A[CI1 At [2NO], (mol / L) (Ch], (mol/L) Initial Rate (mol /L min) 0.18 0.10 0.10 0.10 0.20 0.36 0.20 0.20 145 a) What is the rate law b) What is the value of the rate constant
For the reaction A products, concentration and time data were collected. t (s) [A] (M) > 0.0 3.40 Enter these data into the graphing tool to determine the reaction order. 25.0 2.28 50.0 1.53 75.0 1.02 Graphing Tool Clear All Data [A] vs. t In[A] vs. t 1/[A] vs. t t [A] In[A] 1/[A] [V]
The kinetic reaction data of the decomposition of substance S is given below. Keep the values in 4 decimal places. Time (s) 60 120 180 240 300 360 420 Concentration [S] (M) 2.2464 x 10-3 2.0185 x 10-3 1.8138 x 10-3 1.6299 x 10-3 1.4646 x 10-3 1.3160 x 10-3 1.1826 x 10-3 a. Identify the order of reaction. b. Identify the rate law governing the reaction.
ConstaEIThe taIDTE OT data collected for the reaction A → Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately. Time (s) [A] (M) 0.00 0.600 0.50 0.325 1.00 0.178 1.50 0.095 2.00 0.050 2.50 0.028 3.00 0.015 3.50 0.008 4.00 0.004
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Q1
The following data were obtained for the reaction below at 25.0 °C. 2 NO(g) + O2(g) → 2 NO2(g) Trial 1 2 3 Initial Reactant Concentration (M) [NO] 0.030 0.030 0.060 [0₂] 0.0055 0.0110 0.0055 Initial Rate (M/s) 8.55 x 10-3 1.71 x 10-² 3.42 x 10-² Using the rate law you determined previously, calculate the initial rate for an experiment in which the initial concentration of NO is 0.100 M and O₂ is 0.050 M. Round your answer to 2 sig figs and include your units in your answer.
Consider the following reaction. 4 A + B + 3 C →→ 4 D + E The following data was collected on the reaction. Trial [A]0 [B]0 [C]0 Rate (M/s) 1 0.67 0.5 0.67 8.096 2 1.34 0.5 0.67 32.384 3 0.67 1 0.67 16.192 4 0.67 0.5 1.34 8.096 Two mechanisms are proposed: Mechanism 1: A + C →→ D + Y Y + C →→ X X +2 A + B →→ D + Z Z + A →→ E Mechanism 2: B + C →→ D + Y Y + B + C →→ X + D X + A + C →→ E Which mechanism best fits the data? Select an answer Mechanism 1 or Mechanism 2 Which is most likely the rate-determining step? Select an answer Step 1 or Step 2 or Step 3 or Step 4
4.
A kinetics experiment was conducted based on the reaction: 2NO + H2 - N20 + H20 Use the following data from the experiment to determine the rate law for the reaction. Expt. # Initial rate 1.46 M/min INO]. [H:]0 1 0.021 0.065 2 0.021 0.260 1.46 M/min 3 0.042 0.065 5.84 M/min rate = k[NO] 2[H 2) 2 rate = k[NO] rate = k[NO] 2[H 2] rate = k[NO][H 2] rate = k[NO] 2
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