Hydrogen sulfide (H2S) is a common and troublesome pollutant in industrial wastewaters. One way to remove H2S is to treat the water with chlorine, in which case the following reaction occurs:
H2S(aq) + CI2(aq) --→ S(s) + 2 H+ (aq) + 2 CIˉ (aq)
The rate of this reaction is first order in each reactant. The rate constant for the disappearance of H2S at 28 oC is 3.5 × 10-2 M-1 s-1. If at a given time the concentration of H2S is 2.0 × 10-4 M and that of Cl2 is 0.025 M, what is the rate of formation of CIˉ?