Question

The proposed mechanism for a reaction is

Cl₂ => Cl⁺ + Cl^- Slow

Cl^- + H₂S => HCl + HS^- Fast

Cl⁺ + HS^- => HCl + S Fast

Which of the following would be a rate law for the reaction?

	A.	rate = k[Cl2]
	B.	rate = k[Cl2][H2S]
	C.	rate = k[Cl2]1/2[H2S]
	D.	rate = k[Cl-][H2S]
	E.	rate = [Cl+][Cl-]

Answer 1

cette slow ce the S HU THs fast cettus Hut s fast. Always slow step is the late determining step. In the above reaction only one step is slow, hence this is the rate determining slep. & rate will always depends on the conc. of reactents consumed,

Hence the rate in this eq. Rate = K[ 2]. option A is the right answe