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)+cl2(aq)→s(s)+2h+(aq)+2cl−(a q) the rate of this reaction is first order in each reactant. the rate constant for the disappearance of h2s at 28 ∘c is 3.5×10−2 m−1s−1.if at a given time the concentration of h2s is 2.0×10-4 m and that of cl2 is 2.8×10-2 m , what is the rate of formation of cl?

Explanation:

As the given reaction is as follows.

So, according to the balanced equation, it can be seen that rate of formation of will be twice the rate of disappearance of .

And, it is known that rate of disappearance of reactant will be negative and rate of formation of products will be positive value.

This means that,

Rate of the reaction = -Rate of disappearance of

                 =

                 =

                 = M/s

Therefore, calculate the rate of formation of as follows.

Rate of formation of =

                                        = M/s

Thus, we can conclude that the rate of formation of is M/s.

po-215 i got it right on the quiz