Lec 07 Jan 19 Mon - 1.20 6. Reaction Mechanisms (Sect...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
1.20 6. Reaction Mechanisms (Sect 14-10) = the series of steps by which an overall reaction occurs. Here is an overall reaction : NO 2 (g) + CO (g) NO (g) + CO 2 (g) Rate = k [NO 2 ] p [CO] q Using the method of initial rates, the rate law for this reaction was experimentally determined as : Rate = k[NO 2 ] 2 [CO] 0 = k[NO 2 ] 2 -- 2nd order in NO 2 -- 0th order in CO -- 2nd order overall The following mechanism is proposed for the above overall reaction : ( you will not need to propose a mechanism) Step 1 NO 2 (g) + NO 2 (g) NO 3 (g) + NO (g) (slow) Step 2 NO 3 (g) + CO (g) NO 2 (g) + CO 2 (g) (fast) NO 3 (g) : • is an INTERMEDIATE (neither a reactant nor a product) • it is formed and then consumed during the reaction • is NOT present in overall reaction rate • this is NOT an activated complex, as here NO 3 has fully formed bonds and can exist for a while (may be detected!) Let’s see if the above mechanism is possible : Things to do: look for the slowest elementary step
Background image of page 1

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

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 03/25/2009 for the course CHEM 102 taught by Professor Drk during the Spring '09 term at University of Alberta.

Page1 / 3

Lec 07 Jan 19 Mon - 1.20 6. Reaction Mechanisms (Sect...

This preview shows document pages 1 - 2. Sign up to view the full document.

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