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−(aq) 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?

So, according to the balanced equation, it can be seen that rate of formation of [tex]Cl^{-}[/tex] will be twice the rate of disappearance of [tex]H_{2}S[/tex] .

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 [tex]H_{2}S[/tex]

= [tex]k[H_{2}S][Cl_{2}][/tex]

= [tex](3.5 \times 10^{-2}) \times (2 \times 10^{-4}) \times (2.8 x 10^{-2})[/tex]

= [tex]1.96 \times 10^{-7}[/tex] M/s

Therefore, calculate the rate of formation of [tex]Cl^{-}[/tex] as follows.

Rate of formation of [tex]Cl^{-}[/tex] = [tex]2 \times 1.96 \times 10^{-7}[/tex]

= [tex]3.92 \times 10^{-7}[/tex] M/s

Thus, we can conclude that the rate of formation of [tex]Cl^{-}[/tex] is [tex]3.92 \times 10^{-7}[/tex] M/s.

throwdolbeau throwdolbeau · Answer 2 · 2022-02-01T13:17:44+01:00

The rate of formation of [tex]Cl^-[/tex] [tex]3.92*10^{-7}M/s[/tex].

Let's write the balanced chemical reaction first:

[tex]H_2S_{(aq)}+ Cl_2_{(aq)}---->S_{(s)}+2H^+_{(aq)}+2Cl^-{(aq)}[/tex]

From the given reaction, we can infer that the rate of formation of [tex]Cl^-[/tex] will be twice the rate of disappearance of [tex]H_2S[/tex] .

Let's solve the question:

Rate of disappearance:

For reactants the rate of disappearance is a positive (+) number. For products the (-) rate of disappearance is a negative number because they are being formed and not disappearing.

This means that,

Rate of the reaction = -Rate of disappearance of [tex]H_2S[/tex]

[tex]=k[H_2S][Cl_2]\\\\=3.5*10^{-2}*2*10^{-4}*2.8*10^{-2}\\\\=1.96*10^{-7}M/s[/tex]

Rate of appearance:

The rate of appearance of a product is equal to the rate of disappearance of a reactant.

Therefore, calculation for the rate of formation of [tex]Cl^-[/tex] is as follows.

Rate of formation of [tex]Cl^-[/tex]

[tex]=2*1.96*10^{-7}\\\\=3.92*10^{-7}M/s[/tex]

Therefore, the rate of formation of [tex]Cl^-[/tex] is [tex]3.92*10^{-7}M/s[/tex].

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