Given the following proposed mechanism:(1) 02(g)2 O(g)(slow)(2) 12(g) +2O(g) 2 10(g)(slow) Under what conditions is the reaction most likely to be pseudo-first order?When the pressure of O2(g) is equal to the pressure of I2(g).When the pressure of I2(g) is large.When the pressure of O2(g) is large.When the pressure of O2(g) is small.When the pressure of I2(g) is small.

Pseudo first-order reaction is the type of reaction that appears to be a second-order reaction but…

Answered: Under what conditions is the reaction…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 12Q: The plot below shows the number of collisions with a particular energy for two different...

See similar textbooks

Similar questions

What would be the rate law for the mechanism below? Step 1 NO(g) + Cl2(g) ↔ NOCl2(g) slow Step 2 NOCl2(g) + NO(g) → 2 NOCl(g) fast kobs[NOCl2][NO] kobs[NO][Cl2] kobs[Cl2][NO]2 kobs[NO]2
This table provides rate data for the hypothetical rxn, 2A + B ® C. What is its rate law? Rate = k[A][B] Rate = k[A]2[B] Rate = k[A][B]2 Rate = k[A]2[B]2 Rate = k[B]2
Q3. Find the value of the rate constant at 600 K
What is the molecularity of the rate limiting step for the mechanism below? Step 1: H2O2 (aq) + I–(aq) → H2O(l) + OI–(aq) (slow)Step 2: H2O2 (aq) + OI–(aq) → H2O(l) + O2 (g) + I–(aq) (fast)
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
rate=k[CH3Cl][Cl2]^(1/2) Calculate the value of the rate constant, k.
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?
How is ΔG related to the forward (k1) and reverse(k-1) rates of a reversible first order reaction? ΔG = -RTln(k1/k-1) (k-1/k1) = e(-ΔG/RT) k1/k-1) = -e(ΔG/RT) ΔG = RTln(k1/k-1)
rate law is r=k[ClO2][OH-]
Determine the rate law for the overall reaction below using the mechanisms listed: F2 + CHF3 → HF + CF4 (overall) Step #1: F2 ⇌ 2 F (fast) Step #2: F + CHF3 → HF + CF3 (slow) Step #3: F + CF3 → CF4 (fast) rate = k [F2]½[CHF3] rate = k [F]2 rate = k [F][CHF3] rate = k [F2]½ rate = k [F2][CHF3]
What would be the rate law for the mechanism below? Step 1 I2 → 2 I fast Step 2 2 I + H2 ↔ 2 HI slow

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS