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1) the activation energy for the decomposition of HI(g) is 184 kJ/mole, what rate constant does simple collision theory predict at 300 degrees C? d=0.35nm (1nm=10^-9m) 2) the two second-order reactions have the same pre-exponential factors, and activation energies differing by 20 kJ/mol. what is the ratio of their rate constants at zero degrees C.

1) the activation energy for the decomposition of HI(g) is 184 kJ/mole, what rate constant does simple collision theory predict at 300 degrees C? d=0.35nm (1nm=10^-9m) 2) the two second-order reactions have the same pre-exponential factors, and activation energies differing by 20 kJ/mol. what is the ratio of their rate constants at zero degrees C.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section14.4: Concentration-time Relationships: Integrated Rate Laws
Problem 14.5CYU: Sucrose, a sugar, decomposes in acid solution to give glucose and fructose. The reaction is...
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1) the activation energy for the decomposition of HI(g) is 184 kJ/mole, what rate constant does simple collision theory predict at 300 degrees C? d=D.35nm (Inm=10^-9m) 2) the two second-order reactions have the same pre-exponential factors, and activation energies differing by 20 kJ/mol. what is the ratio of their rate constants at zero degrees C.
Transcribed Image Text:1) the activation energy for the decomposition of HI(g) is 184 kJ/mole, what rate constant does simple collision theory predict at 300 degrees C? d=D.35nm (Inm=10^-9m) 2) the two second-order reactions have the same pre-exponential factors, and activation energies differing by 20 kJ/mol. what is the ratio of their rate constants at zero degrees C.
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