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Chemical Kinetics

Question

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How is the rate of formation of NO₂ related to the rate of disappearance of NO and O₂ in the reaction given below:
$2 NO (g) + O_{2} (g) \to 2 {NO}_{2} (g)$

Solution

Formation of NO₂ rate of disappearnace of NO and O₂ is given by rate equation:

Rate = \frac{1}{2} \frac{d [{NO}_{2}]}{dt} = \frac{- 1}{2} \frac{d [NO]}{dt} = \frac{- d [O_{2}]}{dt}

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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