kinetics informal lab - .033/[.075]^1[.14]^0= .44...

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

View Full Document Right Arrow Icon
Kinetics Theory Lab Olivia Downs 3/14/11 CHM 1046L/85606 The purpose of this experiment was to determine rates to calculate orders to find the rate constant “k”. Also, we found the activation energy. ˚C Temp ˚K 1/ Temp ˚K Rate constant, k Ln(k) 20 293.15 .0034 .44 -.821 28 301.15 .0033 .705 -.350 36 309.15 .0032 .928 -.075 Calculating order of [A] X= Calculating order of [B] X= Calculating rate constant “k” .0339/[.075]^1[.07]^0= .452 .0641/[.15]^1[.07]^0= .427
Background image of page 1

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

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

Unformatted text preview: .033/[.075]^1[.14]^0= .44 Calculating Activation energy Slope= -E(a)/R Slope × R= -Ea (8.314)(-3730)= -31022.22 E(a)= 31022.22 Calculating Frequency factor A= k/e^-E(a)/RT Take the average from all three trials 1) .44/e^-31022.22/(8.314)(293.15)= 147691.50 A 2) .705/e^-31022.22/(8.314)(301.15)= 168770.78 A 3) .928/e^-31022.22/(8.314)(309.15)= 161234.79 A Average A= 159232.36...
View Full Document

This note was uploaded on 11/03/2011 for the course CHM 1046L taught by Professor Simmons during the Spring '11 term at Tallahassee Community College.

Page1 / 2

kinetics informal lab - .033/[.075]^1[.14]^0= .44...

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