The reaction A + B ⟶ C + D rate = k [ A ] [ B ] 2 A+B⟶C+Drate=k[A][B]2 has an initial rate of 0.0570 M / s. 0.0570 M/s. What will the initial rate be if [ A ] [A] is halved and [ B ] [B] is tripled?

0.257 M/s

Explanation:

Let's consider the following reaction.

2 A+B ⟶ C + D

The rate law is:

rate= k × [A] × [B]²

The initial rate is 0.0570 M/s.

rate₀ = 0.0570 M/s = k × [A]₀ × [B]₀²

If [A] = 1/2 [A]₀ and [B] = 3 [B]₀,

rate= k × [A] × [B]²

rate= k × 1/2 [A]₀ × (3 [B]₀)²

rate = 9/2 k × [A]₀ × [B]₀² = 9/2 rate₀ = 9/2 × 0.0570 M/s = 0.257 M/s

it is the most commonly accepted one

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