A →B + C at t = 0 s ?
A reaction rate can be reported quite differently depending on which product or reagent selected to be monitored.
Given a reaction:
rate of reaction = −1/a Δ[A]/Δt=−1/b Δ[B]/Δt = 1/ cΔ[C]/Δt = 1/d Δ[D]/Δt
This formula can also be written as:
rate of reaction = −1/a (rate of disappearance of A)
= −1/b (rate of disappearance of B)
= 1/c (rate of formation of C)
= 1/d (rate of formation of D)
So for A →B + C at t=0
the rate of reaction will be = - Δ[A]/Δt = Δ[B]/Δt = Δ[C]/Δt
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