Iodine `(I_2)` and bromine `(Br_2)` are added to a solution containing iodide `(I^-)` and bromide `(Br^-)` ions. What reaction would occur if the concentration of each species is 1M? The electrode potentials for the reactions are:
`I_2+2barerarr2I^-`, E^@=+0.54V`

Complete the reaction : I_2+ S_2O_3^(2-) rarr

Tarnished silver contains Ag_2S . Can this tranish be removed by placing tranished silver articels in an aluminium pan containing an inert electrolyte solution such as NaCl? The standard electrode potentials for the half cell reactions are: Ag_2S(s)+2barerarr2Ag(s)+S^(2-)(aq) , E^@=-0.71V and Al^(3+)+3barerarrAl(s) , E^@=-1.66V .

Complete the following reaction: NaClO_3+ I_2 rarr

For the reaction , 2HI hArr H_(2) + I_(2)

What will happen when bromine (Br2) is added to ethene in the presence of CCl4?

What will happen when bromine (Br2) is added to propene in the presence of CCl4?

The rate law for a reaction is found to be : Rate = k [NO_2^(-) [I^(-)] [H^+]^2 How would the rate of reaction change when concentration of I^- is halved ?

The rate of a reaction of Br^- ions with BrO_3^- ions in the acidic medium is rate= k[Br^-][BrO_3^-][H^+]^2 The order of reaction