Complete the table below: Reaction: A + B +C - ABc[A][B][C]RateTrial 10.5 M1.5 M1.0 M0.10 M/sTrial 20.5 M1.5 M2.0 M0.10 M/sTrial 30.5 M0.75 M1.0 M0.025 M/sTrial 42.0 M1.5 M3.0 M0.40 M/sTrial 51.0 M1.5 M1.5 MRate LawRate Constant

Solution : The rate law shows the relation between the rate of reaction and the concentration…

Answered: Reaction: A + B+C → ABC [A] [B] Rate…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.33PAE: The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution....

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The reaction below has rate constant 2.50 x 10 -1 min -1 and obeys the rate law: rate = k [A]. At what time will 61.9 % of A have reacted? A --> B The reaction below has rate constant 2.50 x 10 -1min -1 and obeys the rate law: rate = k [A]. At what time will 61.9 % of A have reacted? A --> B 80.8 min 16.9 min 0.00114 min 0.567 min 0.0601 min 3.85 min 19.8 min 495 min
Is the proposed mechanism below valid or invalid? Justify your answer.Overall reaction: 2NO2(g) + F2(g) → 2NO2F(g) ________________________________________________Step 1: NO2(g) + F2(g) →NO2F(g) + F(g) slow Step 2: F(g) + NO2(g) → NO2F(g) fast
Find DG° for this reaction: CH4 (g) + 2O2(g)+ ---> CO2 (g)+ 2H2O (l) Substance DGfdegree (kJ/mol) CH4(g) -50.66 O2(g) 0 CO2(g) -394.4 H2O(l) -237.4 A –682.5 kJ B 131.1 kJ C –581.1 kJ D -919.9 kJ E -818.5 kJ
6 I- + BrO3-  + 6 H+ ----- 3 I2 + Br-  + 3 H2O Rate= k[I-]m[BrO3-]n[H+]p rate= (∆[I2])/(3*∆time) Trial [I-] (M) [BrO3-] (M) [H+] (M) 1 1.67*10-3 6.67*10-3 1.67*10-2 2 3.33*10-3 6.67*10-3 1.67*10-2 3 1.67*10-3 1.33*10-2 1.67*10-2 4 1.67*10-3 6.67*10-3 3.33*10-2 Reaction time: Trial 1 - 301.90 secs Trial 2 - 213.28 secs Trial 3 - 214.92 secs Trial 4 - 86.45 secs Calculate the rate for each trial and Using the information above determine the rate law (m, n and p) for the reaction. m_____________ n_________________ p ____________ Rate= k[I-]m[BrO3-]n[H+]p
Rate information was obtained for the following reaction at 25°C and 33°C; Cr(H2O)6 3+ + SCN¯ ---> Cr(H2O)5NCS2+ + H2O(l)                 Initial Rate             [Cr(H2O)6 3+]                         [SCN-] @ 25°C    2.0x10-11                     1.0x10-4                                0.10                  2.0x10-10                     1.0x10-3                                0.10                  9.0x10-10                     2.0x10-3                                0.15                  2.4x10-9                      3.0x10-3                                0.20 @ 33°C    1.4x10-10                     1.0x10-4                                0.20 Can a 4th order reaction occur?
Rate information was obtained for the following reaction at 25°C and 33°C; Cr(H2O)6 3+ + SCN¯ ---> Cr(H2O)5NCS2+ + H2O(l)                 Initial Rate             [Cr(H2O)6 3+]                       [SCN-] @ 25°C   2.0x10-11                     1.0x10-4                                0.10                  2.0x10-10                     1.0x10-3                                0.10                  9.0x10-10                     2.0x10-3                                0.15                  2.4x10-9                      3.0x10-3                                0.20 @ 33°C   1.4x10-10                     1.0x10-4                                0.20 a) Write a rate law consistent with the experimental data. b) What is the value of the rate constant at 25°C? c) What is the value of the rate constant at 33°C? d) What is the activation energy for this reaction? e) Can a 4th order reaction occur?
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
Calculate the full rate law using the information below: 2 NACHOS (g) → 12 CHIPS (g) + 3 CHEESE (g) [NACHOS]0 (M) Initial Rate (M–1s–1) 0.101 0.00484 0.0910 0.00437 Group of answer choices Rate = 5.61 × 10–2 M–1 s–1 [NACHOS]2 Rate = 6.03 × 10–1 M–2 s–1 [NACHOS]3 Rate = 4.79 × 10–2 s–1 [NACHOS] Rate = 1.66 × 10–3 M1/2 s–1 [NACHOS]2/3 Rate = 1.78 × 10–2 M–1/2 s–1 [NACHOS]3/2
10 Degrees Below16 ° C Room Temperature 26 ° C 10 Degrees Above36 ° C 20 Degrees Above46 ° C 30 Degrees Above56 ° C Depth of H2O2 Solution (d) 2.1 cm 2.1 cm 2.1 cm 2.1 cm 2.1 cm Time (t) 56.30 sec 67.81 sec 23.75 sec 18.50sec e 21.30 sec Rate of the Reaction(R = d/t) 0.04 cm/sec 0.031cm/sec 0.09 cm/sec 0.114 cm/sec 0. 1 cm / sec graph the rate of the reaction on the y-axis and temperature on the x-axis. Based on the information in the data table and your graph, is there an optimum temperature for catalase that makes it the most productive in terms of reaction rate? If so, what is the temperature? At what temperature, does the rate of the reaction decrease? Explain why.
Reaction rate for the chemical reaction 2A + B → A2B Select one: a. V = KCA .CB b. V = KCB c. V = KCA2 d. V = KCA2 .CB
Consider the following reaction. Calculate the value of the rate constant.. 3 A + B → 2 C Trial [A]0 [B]0 [C]0 Rate (M/s) 1 0.61 0.15 0.071 3.013 2 1.22 0.15 0.071 12.052 3 0.61 0.3 0.071 12.052 4 0.18 0.78 0.071 ?
The rate law of the elementary reversible reaction CO + 2H2 < - > CH3OH is k [ Cco CH2 - K CcH3OH ) is True or False Multiple choise

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Reaction: A + B+C → ABC [A] [B] Rate Trial 1 0.5 M 1.5 M 1.0 M 0.10 M/s Trial 2 0.5 M 1.5 M 2.0 M 0.10 M/s Trial 3 0.5 M 0.75 M 1.0 M 0.025 M/s Trial 4 2.0 M 1.5 M 3.0 M 0.40 M/s Trial 5 1.0 M 1.5 M 1.5 M Rate Law Rate Constant