1 / 12

120 likes | 338 Views

Integrated rate laws. ln[ A ] = -k t + ln[ A ] 0. rate = k[ A ]. 1/[ A ] = k t + 1/[ A ] 0. rate = k[ A ] 2. Reaction mechanism. Elementary steps. reaction =. Molecularity. Elementary step. rate law. uni molecular . A product . k[ A ]. A + B product . bi molecular .

Download Presentation
## Integrated rate laws

**An Image/Link below is provided (as is) to download presentation**
Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.
Content is provided to you AS IS for your information and personal use only.
Download presentation by click this link.
While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.
During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

**Integrated rate laws**ln[A] = -kt + ln[A]0 rate = k[A] 1/[A] = kt + 1/[A]0 rate = k[A]2**Reaction mechanism** Elementary steps reaction = Molecularity Elementary step rate law unimolecular A product k[A] A+ B product bimolecular k[A][B] A+B+C product k[A][B][C] termolecular A+A+A product k[A]3 chemical reaction = sum of elementary steps rate law and stoichiometry**Reaction mechanism**2H2O2 (aq) 2H2O(l) + O2(g) Gorxn = [ 2(-237.9)] - [2(-131.67)] = -212.46 kJ spontaneous reaction experimentalrate law: rate = k[H2O2] [I-] I- = catalyst increase rate of reaction not consumed in the overall reaction reactant in early elementary step product in later elementary step**Reaction mechanism**2H2O2(aq) 2H2O(l) + O2(g) rate = k[H2O2] [I-] k1 step 1 H2O2 H2O + OI- + I- k2 step 2 H2O2 + OI- H2O + O2 +I- 2H2O2(aq) 2H2O(l) + O2(g) step 1 rate = k1 [H2O2] [I-]**Reaction mechanism**k1 H2O2 + I- H2O + OI- step 1 k2 H2O2+ OI- H2O + O2 +I- step 2 what about step 2 ? assume k2 >> k1 step 1 rate determining step I- catalyst consumed in rate determining step regenerated in later elementary step intermediate OI- formed in early step, consumed in later step**Rate determining step**on Labor Day weekend “Big Mac” bridge**Reaction Mechanism**H2(g) + I2(g) 2HI(g) rate = k [H2] [I2] reaction faster in light free radical unpaired electron**Reaction Mechanism**H2(g) + I2(g) 2HI(g) rate = k [H2] [I2] I2 2I. step 1 forward rate = kf [I2] kr [I.]2 reverse rate = kf[I2] = kr[I.]2 equilibrium = kf Keq= [I.]2 [I2] kr**** I22I. Reaction Mechanism H2(g) + I2(g) 2HI(g) rate = k [H2] [I2] step 1 step 2 H2+ 2I. 2HI 2HI H2 + I2 need H2in the rate determining step from step 2 rate = k [H2] [I.]2 I.= intermediate**** I22I. Reaction Mechanism H2(g) + I2(g) 2HI(g) rate = k [H2] [I2] step 1 step 2H2+ 2I. 2HI = kf rate = k [H2] [I.]2 [I.]2 Keq = [I2] kr Keq[I2] rate = k [H2] [I.]2 = Keq [I2] rate = k’ [H2] [I2]**2NO N2O2** Reaction Mechanism 2NO + O2 2NO2 rate = k[NO]2 step 1 N2O2 + O2 2NO2 step 2 2NO + O2 2NO2 overall reaction: intermediates: N2O2 relative rates of steps 1 and2**2NO N2O2** 2NO + O2 2NO2 rate = k[NO]2 step 1 N2O2 + O2 2NO2 step 2

More Related