Loading presentation...

Present Remotely

Send the link below via email or IM

Copy

Present to your audience

Start remote presentation

  • Invited audience members will follow you as you navigate and present
  • People invited to a presentation do not need a Prezi account
  • This link expires 10 minutes after you close the presentation
  • A maximum of 30 users can follow your presentation
  • Learn more about this feature in our knowledge base article

Do you really want to delete this prezi?

Neither you, nor the coeditors you shared it with will be able to recover it again.

DeleteCancel

Make your likes visible on Facebook?

Connect your Facebook account to Prezi and let your likes appear on your timeline.
You can change this under Settings & Account at any time.

No, thanks

Chemical Kinetics Lab

No description
by

Kyle Harvey

on 10 October 2012

Comments (0)

Please log in to add your comment.

Report abuse

Transcript of Chemical Kinetics Lab

The rate expression for this experiment was found to be 1.23 L/mol s. This low value indicates a slow reaction rate. The rate expression was found to be: and the overall order of the reaction is second order. This expression indicates that the rate of the reaction is proportional to the concentration of hydrogen peroxide and potassium iodide. If their concentration is doubled, so is the rate. Conclusion There are a couple of errors that occurred in the lab. The first is the stopwatch. It was started before the reactants were mixed together. This created a systematic error. This can be fixed by starting the stopwatch as soon as the reactants have all been mixed together. Another error that occurred was the stopping of the stopwatch. It was difficult to tell which shade of yellow was the right shade. This caused the stopwatch to be stopped early or late. This created a random error. This can be fixed by performing several trials to cancel out the error. Errors Graphical Representation of Reaction The rate expression shows that the rate of the reaction is proportional to the concentration of hydrogen peroxide and potassium iodide. If the concentration of hydrogen peroxide or potassium iodide is doubled, then so is the concentration. Rate Expression Rate Order with respect to HCl Rate Order with respect to H2O2 Table 2 Reaction 4 Rate of Formation Reaction 2 Rate of Formation Reaction 1 Rate of Formation Reaction Mixture 3

H2O2


KI


HCl Solving for Concentration Reaction Mixture 1

H2O2



KI




HCl Solving for Concentration Table 1 The mixture began transparent

The mixture turned yellow- it gradually went from a pale yellow to a dark yellow

The mixture turned brown after being dark yellow

The time taken was based on which combination of volumes was used Observations The purpose of this lab is to derive a rate expression and calculate the value of the rate constant. Purpose The rate of a reaction between two reactants, A and B, can be calculated experimentally. The rate of a reaction will be proportional to the concentration of A raised to a power and also to the concentration of B raised to a power. The rate of a reaction can be expressed as rate= k[A]^x[B]^y . K is the constant of proportionality and is known as the rate constant. X is known as the order of the reaction with respect to A and y is known as the order of reaction with respect to B. The overall order of the reaction is x + y. The order of the reaction and the rate expression can only be determined experimentally. Introduction By Kyle Harvey Chemical Kinetics Lab Calculating the Rate Constant Rate Order with respect to KI Reaction 3 Rate of Formation Reaction Mixture 4

H2O2


KI


HCl Solving for Concentration Reaction Mixture 2

H2O2


KI


HCl Solving for Concentration
Full transcript