We can simply do a rate-to-rate comparison based on the stoichiometric coefficients.
Reaction: Cl2(g) + 3F2(g) → 2ClF3(g)
Since ClF3 is a product, the rate should be positive since products are formed/increased. Based on the balanced equation, we can see that 1 mole of Cl2 forms 2 moles of ClF3.
Consider the reaction: Cl2(g) + 3F2(g) → 2ClF3(g).
Given that Δ[Cl2]/t = -0.054 M/s. Find Δ[ClF3]/Δt
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Based on our data, we think this problem is relevant for Professor De Silva's class at Montclair State University.