Question

Consider the reaction

A+2B⇌C

whose rate at 25 ∘C was measured using three different sets of initial concentrations as listed in the following table:

Trial	[A] (M)	[B] (M)	Rate (M/s)
1	0.50	0.050	1.5×10−2
2	0.50	0.100	3.0×10−2
3	1.00	0.050	6.0×10−2

What is the rate law for this reaction?

Express the rate law symbolically in terms of k, [A], and [B].

Answer 1

A+2B--->C

considering initial con. of reactant in 1&2 [B] when doubled rate is also doubled con. of [A] is constant so [B]is first oder for the reaction.

considering initial con. of reactant in 3&1 when con. of [A] doubled rate is increased by four times so keeping concentration of [B]constant. [A] is second oder for this reaction

so ,

rate= K[A]^2[B]