3.4 Chapter 14 Chemical Kinetics (inked 2)

3.4 Chapter 14 Chemical Kinetics (inked 2) - 14-5...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: 14-5 First-Order ReactionsH2O2(aq) →H2O(l) + ½ O2(g)= -k[H2O2] d[H2O2]dt= -kdt[H2O2] d[H2O2]∫[A][A]t∫t= -ktln[A]t[A]ln[A]t= -kt+ ln[A][k] = s-1Rate of reaction = k[H2O2]First-Order ReactionsHalf-Life•t½is the time taken for one-half of a reactant to be consumed.= -ktln[A]t[A]= -kt½ln½[A][A]- ln 2 = -kt½t½= ln 2k0.693k=Half-LifeButOOBut(g) →2 CH3CO(g) + C2H4(g)14-6 Second-Order Reactions• Rate law where sum of exponents m + n+…= 2.A →productsdt= -kd[A][A]2∫[A][A]t∫t= kt+1[A][A]t1dt= -k[A]2d[A][k] = M-1 s-1 = L mol-1 s-1Rate of Reaction = k[A]2Second-Order ReactionPseudo First-Order Reactions• A second order reaction can sometimes be made to behave like a first order reaction by holding one reactant concentration constant: pseudo first order reaction.CH3CO2C2H5+ H2O →CH3CO2H + C2H5OH• If the concentration of water does not change appreciably during the reaction.– Rate law appears to be first order.– Simplify the kinetics of complex reactions– Rate laws become easier to work with.ExamplePseudo First-Order Reactions• A second order reaction can sometimes be made to behave like a first order reaction by holding one reactant concentration constant: pseudo first order reaction....
View Full Document

Page1 / 4

3.4 Chapter 14 Chemical Kinetics (inked 2) - 14-5...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online