MCQ Detailed View

The decomposition of nitroglycerine (C₃H₅N₃O₉) is a classic example of an autocatalytic reaction. In an autocatalytic process, one of the products formed during the reaction acts as a catalyst, thereby accelerating the reaction further. This leads to a self-accelerating cycle: as more products are formed, the reaction rate increases, sometimes leading to explosive behavior.

In the case of nitroglycerine, its decomposition produces gases such as nitrogen (N₂), oxygen (O₂), water vapor (H₂O), and carbon dioxide (CO₂), along with heat. The high temperature and reactive intermediates generated during the early stages of decomposition act as catalysts for further breakdown of remaining nitroglycerine molecules. This chain effect is why nitroglycerine is highly unstable and extremely explosive under shock, heat, or friction.

It is important to note the difference between other catalytic processes:

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  Self-catalysis or autocatalysis are sometimes used interchangeably, but in chemistry, autocatalysis specifically refers to reactions where a product accelerates the reaction.

  
  


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  Enzyme-catalysis occurs in biological systems and is unrelated to nitroglycerine.

  
  


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  Induced catalysis refers to situations where one reaction induces another reaction but does not describe nitroglycerine decomposition.

  
  

The decomposition of nitroglycerine is dangerous because of this autocatalytic nature. Once decomposition begins, it accelerates rapidly, producing large volumes of hot gases almost instantaneously. This property is utilized in explosives, where controlled detonation is required.

Thus, the phenomenon of nitroglycerine decomposition is best described as an autocatalytic reaction, where the reaction products themselves enhance the rate of further decomposition.