If at a certain instant during the course of the reaction,

2NO2(g) + F2(g) → 2NO2F(g)

the rate of the formation of the product were 0.16 mol·L–1·s–1, how fast would the F2(g) be disappearing (also in mol·L–1·s–1) at that same instant in time?

Question

If at a certain instant during the course of the reaction,

2NO2(g) + F2(g) → 2NO2F(g)

the rate of the formation of the product were 0.16 mol·L–1·s–1, how fast would the F2(g) be disappearing (also in mol·L–1·s–1) at that same instant in time?

BlackTom AI · Accepted Answer

Let's restate the scenario clearly and lay out the data and relationships involved.
- Reaction: 2 NO2 + F2 → 2 NO2F
- Given: rate of formation of the product NO2F is 0.16 mol L–1 s–1 at a certain instant.
- We are asked for the rate at which F2 is disappearing (i.e., the rate of consumption of F2) at that same instant.

To relate rates to stoichiometry, recall that the rate of reaction (often denoted r) links the rates of change of all species via their stoichiometric coefficients:
- d[NO2F]/dt = +2 r (since 2 moles of NO2F are formed per reaction event)
- d[NO2]/dt = −2 r (2 moles of NO2 consumed per event)
- d[F2]/dt = −1 r (1 mole of F2 consumed per event)

Given d[NO2F]/dt = 0.16 M s–1, we can solve for r:
- 0.16 = 2 r  ⇒  r = 0.08 M s–1

Now use the stoichiometry for F2:
- d[F2]/dt = −1 × r = −0.08 M s–1

Hence, the disappearance rate of F2 is 0.08 mol L–1 s–1 (the negative sign indicating consumption).

Now evaluate the answer choices:
- Option 0.080 mol·L–1·s–1: This matches the calculated rate of disappearance (magnitude) and corresponds to the stoichiometric factor of 1 for F2 in the balanced equation, so it is correct.
- Option 0.16 mol·L–1·s–1: This would be the rate of formation of NO2F if the stoichiometry were 1:1 with the product, which it is not; the product rate is twice the reaction rate, so this value is not appropriate for F2 disappearance.
- Option 0.32 mol·L–1·s–1: This is twice the rate we calculated and would imply a different linkage between product formation and reactant consumption; it does not align with the 2:1 stoichiometry for NO2F formation versus F2 consumption.
- Option 0.48 mol·L–1·s–1: This is three times larger than the correct magnitude and likewise inconsistent with the stoichiometric ratios and the given product formation rate.

In summary, the correct understanding comes from linking d[NO2F]/dt to the reaction rate and then using the stoichiometry to find d[F2]/dt. The only option that matches 0.08 M s–1 for the F2 disappearance is the first one, 0.080 mol·L–1·s–1.

If at a certain instant during the course of the reaction, 2NO2(g) + F2(g) → 2NO2F(g) the rate of the formation of the product were 0.16 mol·L–1·s–1, how fast would the F2(g) be disappearing (also in mol·L–1·s–1) at that same instant in time?单项选择题

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