Is the Rate correct? The reaction of nitrogen dioxide with fluorine 2 NO_2 + F_2

Question

Is the Rate correct?

The reaction of nitrogen dioxide with fluorine 2 NO_2 + F_2 rightarrow 2 NO_2 F is first order in NO_2 and first order in F_2. 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. Rate = k[NO^- _2][F^- _2] in an experiment to determine the rate law, the rate constant was determined to be 1.35 times 10^-4 M^-1 s^-1. Using this value for the rate constant, the rate of the reaction when [NO_2] = 3.32 M and [F_2] = 1.18 M would be Ms^-1.

Explanation / Answer

Rate = k [NO2] [F2]    is correct representation

given k = 1.35 x 10^-4 M-1s-1 , [NO2] = 3.32 M , [F2] = 1.18 M

we find rate by formula

Rate = 1.35 x 10^- 4 M-1s-1 ( 3.32M) x ( 1.18M)

   = 5.29 x 10^ - 4 Ms-1

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