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Chemical Kinetics

Question

Express the rate of the following reaction in terms of disappearance of the reactants and appearance of products:
2NO(g) + O₂(g) → 2NO₂(g)

Solution

Rate of reaction in terms of disappearance of the reactants and appearance of product.

2NO(g) + O₂(g) → 2NO₂(g)

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

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Chemical Kinetics

Express the rate of the following reaction in terms of disappearance of the reactants and appearance of products:
2NO(g) + O₂(g) → 2NO₂(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?

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Chemical Kinetics

Express the rate of the following reaction in terms of disappearance of the reactants and appearance of products:2NO(g) + O2(g) → 2NO2(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?

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:
2NO(g) + O₂(g) → 2NO₂(g)

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