011409 - 250 – 400 s Average Rate Δ[NO Δ t(M/s Time...

Info iconThis preview shows pages 1–13. Sign up to view the full content.

View Full Document Right Arrow Icon
CHEMICAL KINETICS Zumdahl Chapter 12
Background image of page 1

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

View Full DocumentRight Arrow Icon
What is a rate? y A change in something over time.
Background image of page 2
Definitions y Chemical Kinetics – the area of chemistry that concerns reaction rates and the steps through which a reaction occurs y Spontaneity – the inherent tendency for a process to occur, has nothing to do with the speed of the reaction y Reversibility – the ability of a reaction to go both forward and backward, it is often more favorable in one direction than in the other
Background image of page 3

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

View Full DocumentRight Arrow Icon
Definitions y Reaction Rate – change in concentration of a reactant or product per unit time y Average Rate – rate measured over a particular time period y Instantaneous Rate – rate measured at a specific time; determine instantaneous rate by taking the slope of the line tangent to the plot of [A] versus time
Background image of page 4
Reaction Rate
Background image of page 5

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

View Full DocumentRight Arrow Icon
Reaction Rate
Background image of page 6
Reaction Rate y What is happening when reaction is taking place?
Background image of page 7

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

View Full DocumentRight Arrow Icon
Average Rate - Δ [NO 2 ]/ Δ t (M/s) Time period (s) 0 – 50 s 50 – 100 s 100 – 150 s 150 – 200 s 200 – 250 s
Background image of page 8
Background image of page 9

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

View Full DocumentRight Arrow Icon
Background image of page 10
Background image of page 11

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

View Full DocumentRight Arrow Icon
Background image of page 12
Background image of page 13
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: 250 – 400 s Average Rate Δ [NO]/ Δ t (M/s) Time period (s) 0 – 50 s 50 – 100 s 100 – 150 s 150 – 200 s 200 – 250 s 250 – 400 s Average Rate Δ [O 2 ]/ Δ t (M/s) Time period (s) 0 – 50 s 50 – 100 s 100 – 150 s 150 – 200 s 200 – 250 s 250 – 400 s Average Rate 250 – 400 s 200 – 250 s 100 – 150 s 0 – 50 s ∆ [O 2 ]/ ∆ t (M/s) ∆ [NO]/ ∆ t (M/s) ∆ [NO 2 ]/ ∆ t (M/s) time period (s) Rate Law y Rate Law – an expression that shows how the rate of a reaction depends on the concentration of the reactants y Order – the exponent of the reactant concentrations, tells us how the rate depends on the concentrations of the reactants, has to be determined experimentally Rate Law y Differential Rate Law – rate law that expresses how a rate depends on concentration, often just called the rate law y Integrated Rate Law – rate law that expresses how concentration depends on time...
View Full Document

This note was uploaded on 02/09/2009 for the course CHEM 105BLG taught by Professor Parr during the Spring '08 term at USC.

Page1 / 13

011409 - 250 – 400 s Average Rate Δ[NO Δ t(M/s Time...

This preview shows document pages 1 - 13. Sign up to view the full document.

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