The thiosulfate ion (s2o32-) is oxidized by iodine as follows: 2s2o32-(aq) + i2(aq) → s4o62-(aq) + 2i-(aq)

in a certain experiment, 4.56×10-3 mol/l of s2o32- is consumed in the first 11.0 seconds of the reaction.

calculate the rate of production of iodide ion.

4.16 × 10⁻⁴ M/s

Explanation:

The rate of appearance of a product is the change in its concentration divided by the time elapsed.

The rate of disappearance of a reactant is minus the change in its concentration divided by the time elapsed.

The rate of the reaction is equal to the rates of appearance or disappearance divided by its stoichiometric coefficient.

Let's consider the following reaction.

2 S₂O₃²⁻(aq) + I₂(aq) → S₄O₆²⁻(aq) + 2 I⁻(aq)

The rate of dissapearance of thiosulfate is:

The rate of the reaction with respect to thiosulfate is:

The rate of the reaction with respect to the iodide ion is: