The process in which methylisonitrile is converted to acetonitrile was found to follow first order kinetics. What do the y-intercepts in the graphs below represent for this reaction? 160 5.2 140 120 100 80 60 40 20 0 0 0 10,000 20,000 30,000 Time (s) 10,000 20,000 Time (s) The natural logarithm of the initial pressure of CH3NC The initial rate of reaction The initial concentration of CH3NC The initial concentration of products Pressure, CH₂NC (torr) In pressure, CH₂NC 5445 80 80 1544- 5.0 4.8 4.6 4.4 4.2 4.0 3.8 3.6 3.4 so so c i do 30,000

The process in which methylisonitrile is converted to acetonitrile was found to follow first order kinetics. What do the y-intercepts in the graphs below represent for this reaction? 160 5.2 140 120 100 80 60 40 20 0 0 0 10,000 20,000 30,000 Time (s) 10,000 20,000 Time (s) The natural logarithm of the initial pressure of CH3NC The initial rate of reaction The initial concentration of CH3NC The initial concentration of products Pressure, CH₂NC (torr) In pressure, CH₂NC 5445 80 80 1544- 5.0 4.8 4.6 4.4 4.2 4.0 3.8 3.6 3.4 so so c i do 30,000

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

For the following reaction: 2N2O5(g) ---> 4 NO2(g) + O2(g) The rate law is first order with respect to N2O5 and has a rate constant of 4.82 x 10-3 sec-1 . Calculate the rate of reaction when the [N2O5] = 0.25M.
A first-order reaction has a rate constant of 3.6 x 10-3s-1. How many seconds does it take for the reaction to be 31.3% complete? (Report an integer)
What are the correct units for the rate constant in a zeroth order overall reaction rate? O M-1s1 O Ms1 s1 O None of these are correct.
The rate at which a certain drug is eliminated by the body follows first-order kinetics, with a half life of 73 minutes. Suppose in a particular patient the concentration of this drug in the bloodstream immediately after injection is 1.1 ug/mL. What will the concentration be 365 minutes later? Round your answer to 2 significant digits. ug x10 mL ?
The gas phase decomposition of sulfuryl chloride at 600 K SO₂ Cl₂ (g) → SO₂ (g)+ Cl₂ (g) is first order in SO₂ Cl2 with a rate constant of 2.80 × 10-³ min-¹. If the initial concentration of SO₂ Cl2 is 0.00164 M, the concentration of SO₂ Cl2 will be 0.000364 M after min have passed.
Determine the rate order and rate constant for dinitrogen pentoxide. Time (minutes) [N2O5] 0 0.0165 10.0 0.0124 20.0 0.00930 30.0 0.00710 40.0 0.00530 50.0 0.00390 60.0 0.00290 Group of answer choices First-order, k = 0.0289 minute-1 First-order, k = 0.0126 M-1⋅minute-1 Second-order, k = 4.59 M-1⋅minute-1 Zero-order, k = 0.000200 M/minute Zero-order, k = 0.0148 M/minute Second-order, k = 30.8 M-1⋅minute-1
Given that the rate constant for the decomposition of hypothetical compound XX from part A is 1.60 M−1⋅min−1�−1⋅min−1, calculate the concentration of XX after 13.0 minmin .
The first-order reaction, SO2C12 → SO2 + Cl2, has a rate constant equal to 2.20 × 10-5 s-1 at 593 K. What percentage of the initial amount of SO2C12 will remain after 9.2 hours? 100% 99.9% 3.88% 48.3% 2.20%