The reaction of nitrogen dioxide with fluorine 2 NO2 F22 NO2F is first order in NO2 and first order in F2. Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear.
In an experiment to determine the rate law, the rate constant was determined to be 1.58E-4 M-1s-1. Using this value for the rate constant, the rate of the reaction when [NO2] = 2.84 M and [F2] = 3.60 M would be Ms-1.

1.62 × 10⁻³ M s⁻¹

Explanation:

Let's consider the following reaction.

2 NO₂ +  F₂ = 2 NO₂F

The generic rate law is:

rate = k × [NO₂]ᵃ × [F₂]ᵇ

where,

The reaction is first order in NO₂ and first order in F₂ and the rate constant is k = 1.58 × 10⁻⁴ M⁻¹ s⁻¹.

The rate law is:

rate = 1.58 × 10⁻⁴ M⁻¹ s⁻¹ × [NO₂] × [F₂]

When [NO₂] = 2.84 M and [F₂] = 3.60 M, the reaction rate is:

rate = 1.58 × 10⁻⁴ M⁻¹ s⁻¹ × 2.84 M × 3.60 M

rate = 1.62 × 10⁻³ M s⁻¹

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