The Iodine Clock Investigation

Summary of iodine clock survey This is a survey on factors affecting reaction rate and reaction rate. By recording and analyzing raw data it is also possible to apply generally accepted scientific rules and test against results obtained from accurate experimental procedures. Objective The purpose of this experiment was to investigate the iodine formation rate when reactant concentration and temperature changed and to try to find order and activation energy.

Hydrogen iodide (IF) is unstable at room temperature and disproportionates with iodine and iodine pentafluoride very easily and irreversibly, so that no pure iodine is obtained. It can be reacted with iodine at -78 ° C. in trichlorofluoromethane at -78 ° C. at -78 ° C. or with silver fluoride at 0 ° C. On the other hand, iodine monochloride (ICl) and iodine bromide (IBr) are moderately stable. The former is a volatile red-brown compound discovered by Joseph Louis Gay-Lussac and Humphry Davy shortly after chlorine and iodine was discovered in 1813-4. Iodine monochloride iodide monochloride and iodine bromide can be easily prepared by reacting iodine with chlorine or bromine at room temperature and purifying by fractional crystallization.

Bromine is an intermediate of reactivity of chlorine and iodine, it is one of the most active elements. The binding energy to bromine is usually lower than the binding energy to chlorine, but higher than the binding energy to iodine, bromine is an oxidizing agent which is weaker than oxygen but stronger than iodine. This is done from the standard electrode potential of X 2 / X pair (F, + 2.866 V; Cl, ​​+1.395 V; Br, +1.087 V; I, + 0.615 V; Δt, about +0.3 V) You can see. Bromination typically results in a higher oxidation state than iodination, but the oxidation state is below chlorination. Bromine tends to react with compounds containing M - M, M - H or M - C bonds to form M - Br bonds.

Iodine oxide is the most stable among all halogen oxides. This is because the large difference in electronegativity between iodine and oxygen leads to strong I - O bonds and they are known for the longest. Since Gay-Lussac and Davy were founded in 1813, a stable white hygroscopic iodine pentoxide (I 2 O 5) has been known. It is most easily produced by dehydration of the acid anhydride iodic acid (HIO 3). It rapidly oxidizes carbon monoxide to carbon dioxide at room temperature and is a useful reagent for determining the concentration of carbon monoxide. It also oxidizes nitrogen oxides, ethylene and hydrogen sulphide. It reacts with sulfur trioxide and bifluorinated peroxodisulfide (S 2 O 6 F 2) to form the salt of the iodinated cation + and is reduced to the iodide salt containing + by concentrated sulfuric acid.