We’re being asked to **calculate the rate of the reaction**** **for the following reaction:

Cl_{2}(g) + 3 F_{2}(g) → 2 ClF_{3}(g)

Recall that for a reaction **aA → bB**, the ** rate of a reaction** is given by:

$\overline{){\mathbf{Rate}}{\mathbf{=}}{\mathbf{-}}\frac{\mathbf{1}}{\mathbf{a}}\frac{\mathbf{\Delta}\mathbf{\left[}\mathbf{A}\mathbf{\right]}}{\mathbf{\Delta t}}{\mathbf{=}}\frac{\mathbf{1}}{\mathbf{b}}\frac{\mathbf{\Delta}\mathbf{\left[}\mathbf{B}\mathbf{\right]}}{\mathbf{\Delta t}}}$

where:

**Δ[A]** = change in concentration of reactants or products (in mol/L or M)

**Δt** = change in time

Consider the reaction: Cl_{2}(g) + 3F_{2}(g) → 2ClF_{3}(g).

Given that Δ[Cl_{2}]/Δt = -0.054 M/s. Find the rate of the reaction.

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