State true or false.Decomposition of nitrogen pentoxide follows second order mechanism, assuming that the kinetics is controlled by a single step mechanism.a)Trueb)FalseCorrect answer is option 'B'. Can you explain this answer?

Question

Answer

False

Nitrogen pentoxide decomposes via a first-order mechanism, not a second-order mechanism. Let's break down the reasons why the statement is false:

- Understanding the mechanism:
- The decomposition of nitrogen pentoxide (N2O5) is known to follow a first-order mechanism. This means that the rate of reaction is directly proportional to the concentration of only one reactant, in this case, N2O5.

- Single-step mechanism:
- The decomposition of N2O5 occurs in a single step, where one molecule of N2O5 breaks down into two molecules of nitrogen dioxide (NO2) and one molecule of oxygen (O2). This single-step mechanism contributes to the first-order kinetics of the reaction.

- Rate expression:
- The rate expression for the decomposition of N2O5 is typically expressed as rate = k[N2O5], where k is the rate constant and [N2O5] represents the concentration of N2O5.

- Experimental evidence:
- Experimental data and studies have confirmed the first-order kinetics of the decomposition of nitrogen pentoxide. The reaction rate is found to be directly proportional to the concentration of N2O5, supporting the first-order mechanism.

In conclusion, the statement that the decomposition of nitrogen pentoxide follows a second-order mechanism assuming the kinetics is controlled by a single step mechanism is false. The correct mechanism for the decomposition of N2O5 is a first-order process.

Answer

The rate of N₂O₅ decomposition is given by, r = k[N₂O₅].
Hence, the reaction follows first order.

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