The order of the reaction $N_2O_5 \, \rightarrow \, N_2O_4(g) + \frac{1}{2}O_2(g)$ is
- 3
- 2
- 1
- 0
The Correct Option is C
Solution and Explanation
A reaction is said to be first order when its rate depends on the concentration of only one reactant raised to the power one.
For the given case, the rate of reaction is directly proportional to the concentration of N2O5.
\(\text{Rate} \propto [N_2O_5]\)
This means that if the concentration of N2O5 is doubled, the rate of reaction also doubles, and if it is halved, the rate becomes half.
This direct proportionality confirms that the reaction follows first-order kinetics.
Hence, the reaction is first order because its rate is proportional to [N2O5].
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Concepts Used:
Order of Reaction
The Order of reaction refers to the relationship between the rate of a chemical reaction and the concentration of the species taking part in it. In order to obtain the reaction order, the rate equation of the reaction will given in the question.
Characteristics of the reaction order
- Reaction order represents the number of species whose concentration directly affects the rate of reaction.
- It can be obtained by adding all the exponents of the concentration terms in the rate expression.
- The order of reaction does not depend on the stoichiometric coefficients corresponding to each species in the balanced reaction.
- The reaction order of a chemical reaction is always defined with the help of reactant concentrations and not with product concentrations.
- Integer or a fraction form the value of the order of reaction will be there and it can be zero.