CH 118 rate of chemical reactions

CH 118 rate of chemical reactions - Rates of Chemical...

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

View Full Document Right Arrow Icon
Rates of Chemical Reactions I. Purpose of the Experiment The purpose of the lab is to identify reaction rates using three different reagents: iodate, sulfurous acid, and water. By adding the reagents through series of orders, reactions show and data is used to identify the reaction rates through a formula, rate=k[HSO 3 - ] y [H + ] . This formula is then deduced to the following formulas: rate=k obs [IO 3 - ] x to k obs k[HSO 3 - ] y [H+] 2 . To convert this data into a linear graph, this formula is used: ln(rate)=xln[IO 3 - ]+ln(k obs ) ln(rate) being the y value, xln[IO 3 - ] being the slope, and ln(k obs ) being the y-intercept. Before so, this formula, M 1 V 1 =M 2 V 2 (M being the concentration in Molarity and V being the volume in drops), is used to identify the final concentrations for reaction rate equations. II. Summary of the Procedure Two pipets were stretched and cut at an angle to ensure consistent drop size. A five cm marking was placed on a third pipet. A stretched pipet was used to measure x drops of IO
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 06/15/2011 for the course CH 118 taught by Professor March during the Fall '09 term at University of Alabama at Birmingham.

Page1 / 2

CH 118 rate of chemical reactions - Rates of Chemical...

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