The chemical reaction between Hydrogen sulphide and iodine to give Hydrogen iodide and sulphur is given below:H2S + I2 → 2HI + S.The reducing and oxidising agents involved in this redox reaction are:Iodine and sulphur, respectivelyIodine and hydrogen sulphide, respectivelySulphur and iodine, respectivelyHydrogen sulphide and sulphur, respectively

Iodine reacts with ClO−3ClO3- under acidic conditions according to the reaction shown below.5 ClO−3+3 I2+3 H2O ⟶ 5 Cl−+6 IO−3+6 H+5 ClO3-+3 I2+3 H2O ⟶ 5 Cl-+6 IO3-+6 H+Does I2I2 act as the oxidizing agent or reducing agent in the reaction?A.Oxidizing agent, because I2I2 is reducedB.Reducing agent, because I2I2 is oxidizedC.Oxidizing agent, because ClO−3ClO3- is reducedD.Reducing agent, because ClO−3ClO3- is oxidized

Which of the following reaction produces SO2 gas?Burning of sulphur in oxygenReaction of copper with H2SO4Roasting of sulphide oresBurning of H2S

Suppose the formation of iodine proceeds by the following mechanism:step elementary reaction rate constant1 H2(g) + ICl(g) → HI(g) + HCl(g) k12 HI(g) + ICl(g) → I2(g) + HCl(g) k2Suppose also k1≫k2. That is, the first step is much faster than the second.Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction. =ratek Note: your answer should not contain the concentrations of any intermediates.Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism. =k

Deduce the balanced chemical equation for the reaction between sodium and sulfur. State the electron arrangements of the reactants and product, and explain whether sulfur is oxidized or reduced.

H2O2(aq) + 2I-(aq) + 2H3O+(aq) → I2(aq) + 4H2O(l) (Reaction 1) I2(aq) + 2S2O32-(aq) → S4O62-(aq) + 2I-(aq) (Reaction 2) I2(aq) + I-(aq) + Starch(aq) → (I3- -Starch)complex (aq) (Reaction 3) Now consider the moment when the blue colour change is about to occur (i.e. when there is no more thiosulfate remaining in solution).Based on the initial experiment and initial concentrations of reagents, calculate the concentrations of the reagents present in the flask at the moment just before the blue colour change begins (ignore the starch, and the S4O62- which is formed as the other by-product in this reaction).Does Reaction (1) continue beyond this point? Multiple choice 2 Question 10a. yesb. no Based on what you have calculated, which reagent in Reaction (1) is the limiting reagent?Multiple choice 3 Question 10a. H+b. H2O2c. I-d. S2O32-