Chem_208_Lecture_7_Color

# Chem_208_Lecture_7_Color - PS3 due Friday at 2PM Today...

This preview shows pages 1–7. Sign up to view the full content.

PS3 due Friday at 2PM Today 14.4-14.7

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

View Full Document
Method of Initial Rates 1. Measure reaction rate for a known set of initial concentrations. BrO 3 - (aq) + 5Br - (aq) + 6H + (aq) 3Br 2 (l) + 3H 2 O (l) Expt. [BrO 3 - ][ B r - H + ] Init. Rate (M/s) ______________________________________________________ 1 0.10 0.10 0.10 8.0 x 10 -4 2. Carry out measurement again, using one different init. conc. 4. Continue by varying other initial concentrations to find order. 3 0.20 0.10 0.20 3.2 x 10 -3 2 0.20 0.10 0.10 1.6 x 10 -3 3. Determine the order of reaction with respect to that reactant. 4 0.10 0.20 0.10 3.2 x 10 -3 Rate = k [BrO 3 - ] a [Br - ] b [H + ] c
Zero-Order Reactions • Sum of exponents m + n +…. = 0 • Most common for unimolecular decomposition: A products Rate = k[A] 0 =k = constant Slope = -k k in units of M/s Integrated Rate Law: [A] t = [A] o -k ±t

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

View Full Document
First-Order Reactions • Sum of exponents m + n +…. = 1 • Most common for unimolecular decomposition and radioactive decay. A products Rate = k[A] 1 =k[A] Slope of [A] vs. t is not constant.
First-Order Reactions Rate = k[A] Integrated Rate Law: ln[A] t = ln[A] o -k±t Slope = -k k in units of s -1 [A] t =[A] o e -kt

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

View Full Document
Second-Order Reactions • Sum of exponents m + n +…. = 2
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

### Page1 / 12

Chem_208_Lecture_7_Color - PS3 due Friday at 2PM Today...

This preview shows document pages 1 - 7. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online