The below reaction was studied using integrated rate kinetics2A 3BThe below graphs were generated. © CHEM1212 JB[A] vs. TimeIn[A] vs. Time12040214200100sime (sUme b)1/[A] vs. Time7000s.0004000cme (s)Which of the below mechanisms is most consistent with this data?[ALM 5.000400070000.000200tine (s)Which of the below mechanisms is most consistent with this data?a) step 1: A 2C (fast)step 2: 2C+ A→3B (slow)Ob step 1: A B+C (slow)step 2: C+A → 2B (fast)) step 1: A → B+C (slow)step 2: C+2A B (fast)di This is an elementary reaction as written 2A 3B

Interpretation: We have to determine the rate order for the reaction.

The below reaction was studied using integrated rate kinetics 2A 3B The below graphs were generated. © CHEM1212 JB [A] vs. Time In[A] vs. Time 12 02 00 200 400 500 1. 04 -10 0.4 1.2 0.2 14 100 200 400 500 ime (s) time (s) 1/[A] vs. Time 7.000 6.000 1.000 4.000 3.000 400 tme (s) Which of the bel w mechanisms is most concistent with this data? (AL M 1/(AL M

The below reaction was studied using integrated rate kinetics 2A 3B The below graphs were generated. © CHEM1212 JB [A] vs. Time In[A] vs. Time 12 02 00 200 400 500 1. 04 -10 0.4 1.2 0.2 14 100 200 400 500 ime (s) time (s) 1/[A] vs. Time 7.000 6.000 1.000 4.000 3.000 400 tme (s) Which of the bel w mechanisms is most concistent with this data? (AL M 1/(AL M

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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Consider the following chemical reaction involving hydrogen gas and NO. The value of the specific rate constant at this temperature is H2(g) + 2 NO(g) → N20(g) + H2O(g) (MTS 2/17/2018) Experiment Initial [NO] (M) Initial [H2]_(M). Initial Rate (M•s-1) 1 0.30 0.35 2.835 x 10-3 2 0.60 0.35 5.670 x 10-3 3 0.60 0.70 2.268 x 10-2
Consider the initial-rate data at a certain temperature in the table for the reaction described by 2 NO₂ (g) + 03 (g) N₂05(g) + O₂(g) Determine the value and units of the rate constant, k. k= [NO2], (M) 0.650 1.10 1.76 Units: [03], (M) 0.800 0.800 1.40 Initial rate (M/s) 3.12 x 104 5.28 × 104 14.78 x 104
Reaction Conc. Na2S2O3 Conc. HCI A Abs. A Time (s) Rate (Δ Abs./jΔ Time) 1 0.10 M .30 М 1.3686611 1.007568 1.358380874 0.300349 |0.01870913 0.10 M .15 M 1.5360817 5.114311671 3 0.050 M .30 M 1.2267196 65.56796601 4 0.025 M .30 М 0.9563164 0.02870913 11.3085840 POSTLAB QUESTIONS 1. Compare the rates of reactions 1, 3 and 4. What is the effect on the reaction rate of halving the thiosulfate concentration? What is the order of the reaction in sodium thiosulfate?
Consider the reaction A+2B⇌CA+2B⇌C whose rate at 25 ∘C∘C was measured using three different sets of initial concentrations as listed in the following table: Trial [A][A](MM) [B][B](MM) Rate(M/sM/s) 1 0.20 0.010 4.8×10−4 2 0.20 0.020 9.6×10−4 3 0.40 0.010 1.9×10−3 Calculate the initial rate for the formation of CC at 25 ∘C∘C, if [A]=0.50M[A]=0.50M and [B]=0.075M[B]=0.075M. Express your answer numerically in molar per second using two significant figures.
The initial Rate of a chemical reaction is the instantaneous rate at t=1s true of false
In Experiment M you studied the reaction: S2Og²- + 2l¯ → 2SO42- + 12 The reaction time was monitored by the "iodine clock reaction": 2S2032- + 12→ 21¯ + S406²- When the above reaction was carried at 22°C (using the same concentrations) with a trace of copper sulfate, the time for the reaction decreased because: The rate constant decreases due to the presence of the copper ions The rate constant decreases due to the presence of the sulfate ions The copper ions provide an alternative path for the reaction of S20g²- + 2I° The copper ions increase AH so more molecules of S2032- could react OThe copper ions provide an alternative path for the reaction of S2O3²- with I2
Consider the mechanism. Step 1: A+B Step 2: A+C Overall: 2 A+B D Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate= esc ! # 1 Te @ 2 W # 3 C E C D $ 4 R slow fast G Search or type URL % 5 MacBook Pro T 6 Y & 7 M U * 00 8 + 1 ( 9 O P
Analyze the following reaction mechanism: H2O + O → CIÓ + CF2CI CI + 202 4. Cl + CF2CI –→ CF2CI2 1. H2O2 2. O + CF2CI2 3. CIO + Oз -> Identify the reaction intermediates in this reaction. A) O, CIO, CI B) CI, CF;CI, CF2CI2 C) O, CIO, O, H20 D) O, CIO, CI, CF2CI E) O, CIO, CI, CF;CI2
Attem Using the data in the table, determine the rate constant of Trial [A] (M) [B] (M) Rate (M/s) the reaction and select the appropriate units. 1 0.300 0.400 0.0112 2 0.300 0.800 0.0112 A + 2B C+D 3 0.600 0.400 0.0448 Units k =|| %D TOOLS M-'s-1 x10 |help terms of use contact us careers privacy policy about us prime video W
For the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C 2 H202(aq)2 H20(1) + O2(g) the following data have been obtained: [H2O2], M 4.17x10-2 11.4 8.86x10-2 9.24x10-3 1.96×102 22.8 time, min 34.2 The average rate of disappearance of H,02 over the time period from t= 0 min to t= 11.4 min 1s M min-1.
For the gas phase decomposition of hydrogen peroxide at 400 °C 2 H2O2 2 H2O + O2 the following data have been obtained: [H,O2], M 9.35x10-2 3.54x10-2 2.18×10-2 1.56x10-2 time, s 27.0 54.0 81.0 The average rate of disappearance of H,O2 over the time period from t = 27.0 s to t = 54.0 s is |Ms-!.