For the reaction, $2 N_{2} O_{5} (g) \overset{}{\to} 4 N O_{2} (g) + O_{2} (g)$ the rate of formation of NO₂ (g) is 2.8 x 10^-3 Ms^-1. Calculate the rate of disappearance of N₂O₅ (g).

Solution

$2 N_{2} O_{5} (g) \overset{}{\to} 4 N O_{2} (g) + O_{2} (g) R a t e o f r e a c t i o n - \frac{1}{2} \frac{d [N_{2} O_{5}]}{d t} = \frac{1}{4} \frac{d [N O_{2}]}{d t} = \frac{d [O_{2}]}{d t} A c c o r d i n g t o q u e s t i o n \frac{d [N O_{2}]}{d t} = 2.8 x 10^{- 3} M s^{- 1} - \frac{d [N_{2} O_{5}]}{d t} = \frac{2}{4} \frac{d [N O_{2}]}{d t} = \frac{1}{2} x 2.8 x 10^{- 3} M s^{- 1} = 1.4 x 10^{- 3} M s^{- 1}$

Some More Questions From Chemical Kinetics Chapter

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Chemical Kinetics

For the reaction, $2 N_{2} O_{5} (g) \overset{}{\to} 4 N O_{2} (g) + O_{2} (g)$ the rate of formation of NO₂ (g) is 2.8 x 10^-3 Ms^-1. Calculate the rate of disappearance of N₂O₅ (g).

Some More Questions From Chemical Kinetics Chapter

What will be the effect of temperature on rate constant?

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.

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Chemical Kinetics

For the reaction,2N2O5 (g) → 4 NO2 (g) + O2 (g) the rate of formation of NO2 (g) is 2.8 x 10-3 Ms-1. Calculate the rate of disappearance of N2O5 (g).

Some More Questions From Chemical Kinetics Chapter

What will be the effect of temperature on rate constant?

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

For the reaction, $2 N_{2} O_{5} (g) \overset{}{\to} 4 N O_{2} (g) + O_{2} (g)$ the rate of formation of NO₂ (g) is 2.8 x 10^-3 Ms^-1. Calculate the rate of disappearance of N₂O₅ (g).

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