Initial rates and the iodine clock

Tick tock goes the Iodine clock! Well not quite. Explore this video to find out how we can measure the initial rate from reactions and how we can use clock reactions to do the same too. Find out how we can use this to find out the order of the reaction.

[@MrHarun-dv6ee]

My word, these videos are absolute pieces of gem. I sincerely hope you are getting donations, because it'd be a shame if you had to delete this channel. All the best.

[@AlleryChemistry]

+Mamma Harun Thanks for your feedback. Thankfully for you this channel aint going anywhere. Plenty more content to be uploaded and more podcasts too. Revision summary sheets are on the agenda too! So much to do, so little time to do it in!

[@enlimyror9697]

Mr. Harun y

[@ausiliaquirighetti7596]

I’m watching this 9 years later and it’s better than any revision website. You are truly a legend thank you!!!

[@adlieneedun1061]

ik this is quite an old vidoe but please never stop doing these, because 9 years later this helped me understand so much more than save my exams and pmt :)

[@AlleryChemistry]

Thanks, surprisingly, the syllabus hasn't changed.

[@user-ms2bl4gg7h]

same, watching this the day of paper 2, i never thought 9 year old videos would be so useful. amazing guy he's literally walter white

[@i_love_dua_lipa1]

@@user-ms2bl4gg7h how did u find p1 and p2

[@imranramzan5042]

You need to explain that the thiosilphate is added to consume the iodine in the first reaction and when all the thiosulphate is used the iodine remains which then starch to a black colour. In your example the reaction will instantly go black.

[@darkmoon3646]

Mr allery u are an absolute blessing in my life

[@SH-tk9hy]

This actually helped me to understand the graphical method a lot better, my text book isn't very concise. However, I'm still a bit hazy on the iodine clock reaction, do you put the starch in at the same time as when you are mixing the reactants? My textbook says that the initial rate is proportional to 1/t. I'm not quite sure I understand.

[@AlleryChemistry]

Yes you do. The Iodine turns black in the presence of starch. Yes the 1/t bit is just the units other rate. E.g. s-1.

[@CookiieMonsterXxX]

You are amazing!

[@AlleryChemistry]

Thanks. Iodine clock is a tough one so I'm pleased it helped you.

[@zakkharsane3988]

Thank you, thank you, thank you very much, you have saved me

[@SuperStargazer666]

Surely thiosulphate must be added to the clock reaction? It’s a two step reaction and the second step involves thiosulphate

[@joehindley6185]

you are a complete legend, thanks so much

[@jasthakker648]

Fantastic Vid

[@aydahashraf8574]

Thank you for these videos!

[@rbc812]

Is the iodine clock experiment considered as initial rates method.

[@bleachbravesoul2542]

thank you for all the videos 😊😀

[@MeeraP07]

Hiya! Thanks for this fab video! Can you draw a tangent to the graph at t=0 and then measure the gradient of the tangent? That method has come up in Edexcel papers before.

[@AlleryChemistry]

MeeraP07 Thanks! Yes you should work out the gradient at t=0 in order to work out the initial rate. Please share the video and follow me on twitter @allerytutors for pre-release information on videos and future project news.

[@samcat4005]

Hey so I was just wondering, is it possible to measure the rate of reaction of an oscillatory reaction??? Like the briggs rauscher reaction??

[@samiultr]

yh

[@spadventuresworld7484]

I want to do a kinetic for a chemical reaction. Could you please how to calculate the intial rate of reaction?.

[@hassamurrehman1783]

Dude you're amazing

[@Sammy.a1287]

You're a cool dude

[@hudadahman2389]

In our book they added sodium thiosulfate can i know why was it added ??

[@physchemwithliz5879]

To convert the iodine back into iodide. If there was no thiosulfate, the solution would just turn black very quickly.

[@GallupJonas-z1x]

Rodriguez Joseph Lewis Steven Jackson Ronald