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Rate of Reaction: N2 + 3H2 -> 2NH3
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[QUOTE="mjc123, post: 6029578, member: 610180"] You cannot write "rate of disappearance of H[SUB]2[/SUB] = -1/3 Δ[H[SUB]2[/SUB]]/Δt" because that simply isn't true. By definition, the rate of disappearance of H[SUB]2[/SUB] is -Δ[H[SUB]2[/SUB]]/Δt. (Strictly, that should be the rate of [I]change[/I] of [H[SUB]2[/SUB]]. The rate of disappearance would be positive, and equal to minus the rate of change.) It is the "rate of reaction" that is subject to ambiguous definition. You could define the "reaction" as: N[SUB]2[/SUB] + 3H[SUB]2[/SUB] → 2NH[SUB]3[/SUB] in which case rate of reaction = rate of consumption of N[SUB]2[/SUB] = 1/3 rate of consumption of H[SUB]2[/SUB] 1/2N[SUB]2[/SUB] + 3/2H[SUB]2[/SUB] → NH[SUB]3[/SUB] in which case rate of reaction = rate of production of NH[SUB]3[/SUB] = 2/3 rate of consumption of H[SUB]2[/SUB] 1/3N[SUB]2[/SUB] + H[SUB]2[/SUB] → 2/3NH[SUB]3[/SUB] in which case rate of reaction = rate of consumption of H[SUB]2[/SUB] = 3* rate of consumption of N[SUB]2[/SUB] That is why I don't like "rate of reaction", and always like to do kinetics in terms of the rate of change of a specified reagent. But you need to know this stuff to do exams these days. [/QUOTE]
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Rate of Reaction: N2 + 3H2 -> 2NH3
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