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Chemical Kinetics

Question

Nitrogen dioxide (NO₂) reacts with fluorine (F₂) to form nitryl fluoride (NO_zF) according to the reaction

$2 {NO}_{2} (g) + F_{2} (g) \to 2 {NO}_{2} F (g)$

Write the instantaneous rate of reaction in terms of
(i) rate of formation of NO₂ ,F
(ii) rate of disappearance of NO₂(iii) rate of disappearance of F₂.

Solution

Nitrogen dioxide (NO₂) reacts with fluorine (F₂) to form nitryl fluoride (NO_zF) according to the reaction

$2 {NO}_{2} (g) + F_{2} (g) \to 2 {NO}_{2} F (g)$

(i) Rate of formation of ${NO}_{2} F (r) = \frac{d ({NO}_{2} F)}{dt} .$
(ii) Rate of disappearance of ${NO}_{2} (r) = - \frac{d ({NO}_{2})}{dt} .$
(iii) Rate of disappearance of $F_{2} (r) = - \frac{d (F_{2})}{dt} .$

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Chemical Kinetics

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Chemical Kinetics

Nitrogen dioxide (NO2) reacts with fluorine (F2) to form nitryl fluoride (NOzF) according to the reaction2NO2(g)+F2(g)→2NO2F(g)Write the instantaneous rate of reaction in terms of(i) rate of formation of NO2 ,F(ii) rate of disappearance of NO2(iii) rate of disappearance of F2.

Some More Questions From Chemical Kinetics Chapter

A reaction is 50% complete in 2 hours and 75% complete in 4 hours. What is the order of the reaction.

The rate law for the decomposition of N2O5 is rate = k[N2O5]. What is the significance of k in this equation?

Define activation energy of a reaction.

Mock Test Series

NCERT Sample Papers

Entrance Exams Preparation

The rate law for the decomposition of N₂O₅ is rate = k[N₂O₅]. What is the significance of k in this equation?