A gas phase reaction between nitrogen dioxide and fluorine is proposed to occur

Question

A gas phase reaction between nitrogen dioxide and fluorine is proposed to occur by the following mechanism: step1 slow: No2+FNO,F F step 2 fast. F+NO.NO.F (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank (4) Complete the rate laiw for the overall reaction that is consistent with this mechanism. (Use the form k[A] [B]"..., where 1' is understood (so don't write it) for m, n etc.)

Explanation / Answer

Q1

overall reaction --> addition of both steps

NO2 + F2 + F + NO2 = NO2F + F + NO2F

cancel common terms

2NO2 + F2=2NO2F

Q2

catalyst will be consumed then formed, there is none present

Q3

intermediates will be formed then consumed

from the reaction, only F is formed, then consumed

Q4

Rate = k*[reactants]^r

from the list, only slow step must be considered

Rate = k*[NO2][F2]

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