Express the rate of the following reaction in terms of disappearance of the reactants and appearance of products:
CO(g) + NO₂(g) → CO₂(g) + NO(g)

Solution

The rate of the reaction in terms of disappearance of the reactant and appearance of product.

CO(g) + NO₂(g) → CO₂(g) + NO(g)

$rate = \frac{- d [CO]}{dt} = \frac{- d [{NO}_{2}]}{dt} = \frac{d [{CO}_{2}]}{dt} = \frac{d [NO]}{dt}$

Some More Questions From Chemical Kinetics Chapter

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Chemical Kinetics

Express the rate of the following reaction in terms of disappearance of the reactants and appearance of products:
CO(g) + NO₂(g) → CO₂(g) + NO(g)

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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?

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Chemical Kinetics

Express the rate of the following reaction in terms of disappearance of the reactants and appearance of products:CO(g) + NO2(g) → CO2(g) + NO(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

Express the rate of the following reaction in terms of disappearance of the reactants and appearance of products:
CO(g) + NO₂(g) → CO₂(g) + NO(g)

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