To this is added a solution containing potassium iodidesodium thiosulfateand starch. There are two reactions occurring in the solution.
Next Chemistry Investigation Questions. I'm currently doing A2 chemistry, Salters B course. Within this course there is a large piece of coursework called an 'individual investigation that is completed over about a month. My investigation is on the kinetics of the reaction between potassium bromate, potassium bromide and hydrogen ions.
This reaction is commonly called a bromine clock. I am using a small known quantity of phenol solution in my reaction so that the time taken for the bromide ions to decolourise is proportional to the rate of the reaction.
But I'm having a few issues. I have found a mechanism, in the form of equations, but I can't find the types of intermediate reactions nucleophilic substitution etc. The steps I have are: So hopefully someone can shed some light on how each this reacts, so that I can draw it.
The experiments I have done so far is: Now I am changing the catalyst, and investigating the effects. The reaction originally uses sulfuric acid as a catalyst to supply the hydrogen ions. I tried today using the same concentration 0. All conditions, concentrations and volumes were kept the same in both reactions, however, the sulfuric acid reaction took 22 seconds to decolourise, but the HCl reaction took only 3 seconds.
I can't explain this. Sulfuric acid and hydrochloric acid are both strong acids, but sulfuric acid is a diprotic acid, so I expected the sulfuric acid reaction to be faster, not the other way around.
My chemistry teacher couldn't explain this either. So there are my two main issues. What is the mechanism for this reaction? Hope you can help, please only answer if you know what you're talking about, I have to use this information in my report.The kinetics of the reaction between bromate(V), bromide and hydrogen ions Bromate(V), bromide and hydrogen ions react according to the following equation: 5Br– + BrO3– + 6H+ → 3Br2 + 3H2O As bromate and bromide react, they produce Br2, which then reacts with methyl orange to dissipate the colour of the solution and show completion of the reaction.
Reaction step 2: ·The iodide formed is oxidized by the iodate excess under formation of iodine. Iodine reacts with starch to form a blue iodine-starch complex. The reaction proceeds fast. Reaction step 3: ·Iodine liberated is instantaneously retransformed by bisulfite to iodide.
This is . Bromine Clock Reaction Free Essays - StudyMode Bromine Clock Reaction. PLAN Introduction: After having built up knowledge about the kinetics of reactions I decided to do an investigation in this area. The bromate-ferroin clock reaction is studied experimentally and the dependence of the clock or induction timet cl on the initial concentration of various reactants determined.
Particular attention is paid to the dependence of t cl cl on the initial bromide ion concentration [Br − ] 0.
Core practical Determine the activation energy for the reaction between bromide and bromate(V) ions Objective To use the Arrhenius equation to determine the activation energy of a reaction Safety Wear a lab coat and gloves, and use eye protection.
Phenol is . Iodine Clock Reaction Kinetics Introduction: This experiment is designed to study the kinetics of a chemical reaction. The reaction involves the oxidation of iodide ions by bromate ions in the presence of acid. The objective of this lab is to determine the rate law for the redox reaction between the iodide ion, bromate ion, and hydrogen ion in.