For the gas phase decomposition of trichloromethyl chloroformate, CICOOCC13 → 2 COC1₂ -1 the rate constant in s has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.09 × 104 K and a y-intercept of 30.3. The value of the rate constant for the gas phase decomposition of trichloromethyl chloroformate at 556 K is S-¹.

For the gas phase decomposition of trichloromethyl chloroformate, CICOOCC13 → 2 COC1₂ -1 the rate constant in s has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.09 × 104 K and a y-intercept of 30.3. The value of the rate constant for the gas phase decomposition of trichloromethyl chloroformate at 556 K is S-¹.

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

Concentration-Time Relationships (See Section 15.4 and Examples 15.5-15.7.) 15. The rate equation for the hydrolysis of sucrose to fruc- tose and glucose CRH2O1(aq) + H¿O(€) → 2 C,H12O6(aq) is -A[sucrose]/At = k[C¡2H2O1]. After 27 minutes %3D at 27 °C, the sucrose concentration decreased from 0.0146 M to 0.0132 M. Find the rate constant, k.
For the gas phase decomposition of nitrogen dioxide at 383 °C 2 NO2 2 NO +02 the following data have been obtained: [NO2], M time, s 6.85x10 2 3.25x102 2.13x102 0 30.0 60.0 1.55x10-2 90.0 The average rate of disappearance of NO2 over the time period from t = 30.0 s to t = 60.0 s is Submit Answer Retry Entire Group 8 more group attempts remaining Ms.
For the gas phase decomposition of bromoethane, CH;CH,Br >C,H4 + HBr -1 the rate constant in s has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of-2.63x104 K and a y-intercept of 29.6. The value of the rate constant for the gas phase decomposition of bromoethane at 703 K is -1 (Enter your answer to one significant figure.)
24
For the gas phase decomposition of t-butyl acetate, CH3COOC(CH,))3– 3/3 (CH,)2C=CH, + CH,COOH 3/2 the rate constant has been determined at several temperatures. When In k in s is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.04×104 K and a y-intercept of 30.7. The activation energy for the gas phase decomposition of t-butyl acetate is kJ/mol.
For the gas phase decomposition of ethyl acetate, CH;COOC,H,–CH,COOH + C2H4 the rate constant has been determined at several temperatures. When In k -1 in s is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.41x10* K and a y-intercept of 28.8. The activation energy for the gas phase decomposition of ethyl acetate is kJ/mol.
The rate constant of a chemical reaction increased from 0.100 s−1 to 3.20 s−1 upon raising the temperature from 25.0 ∘C to 55.0 ∘C . Calculate the value of (1T2−1T1) where T1 is the initial temperature and T2 is the final temperature. Express your answer numerically.
to access important values if needed for this question. For the gas phase decomposition of ethyl chloroformate, CICOOC₂H5 C₂H5Cl + CO₂ the rate constant in s¹ has been determined at several temperatures. When Ink is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -1.48 x 104 K and a y-intercept of 24.6. The value of the rate constant for the gas phase decomposition of ethyl chloroformate at 465 K is s-1
The rate constant of a chemical reaction increased from 0.100 s−1 to 3.10 s−1 upon raising the temperature from 25.0 ∘C to 55.0 ∘C . Part A: Calculate the value of (1/T2−1/T1) where T1 is the initial temperature and T2 is the final temperature. Part B: Calculate the value of ln(k1/k2) where k1 and k2 correspond to the rate constants at the initial and the final temperatures as defined in part A. Part C: What is the activation energy of the reaction?