Following reaction takes place in one step:

$2 NO (g) + O_{2} (g) ⇋ 2 {NO}_{2} (g)$

How will the rate of the above reaction change if the volume of the reaction vessel is diminished to one third of its original volume? Will there be any change in the order of the reaction with the reduced volume ?

Solution

The below reaction take place in one step, thus rate of reaction is

2 NO (g) + O_{2} (g) ⇌ 2 {NO}_{2} (g)

Rate = k {[NO]}^{2} [O_{2}]

Suppose x moles of NO and Y moles of O₂ are taken in the vessle of volume V litre, then

r_{1} = k {[\frac{x}{V}]}^{2} [\frac{y}{V}]

If the volume of vessel is reduced to V/3, then for the same moles of NO₂ and O₂

_{$r_{2} = k {[\frac{x}{V / 3}]}^{2} {[\frac{y}{V / 3}]}^{2} = 27 k {[\frac{y}{V}]}^{2} [\frac{y}{V}]$

$∴$ $\frac{r_{2}}{r_{1}} = 27 or r_{2} = 27 r_{1}$}The rate of the reaction becomes 27 times the initial rate. Order of reaction remains unaffected.

Some More Questions From Chemical Kinetics Chapter

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Chemical Kinetics

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.

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Chemical Kinetics

Following reaction takes place in one step:2NO(g) + O2(g) ⇋2NO2(g)How will the rate of the above reaction change if the volume of the reaction vessel is diminished to one third of its original volume? Will there be any change in the order of the reaction with the reduced volume ?

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?