What happens when methane undergoes combustion in systems A and B respectively?
System A: Temperature remains same \quad System B: Temperature rises
System A: Temperature falls \quad System B: Temperature rises
System A: Temperature falls \quad System B: Temperature remains same
System A: Temperature rises \quad System B: Temperature remains same
Correct answer:A
Standard Method
Given: Methane undergoes combustion in System A and System B.
Find: What happens to the temperature in the two systems.
From the solution text:
System A (Adiabatic System): In an adiabatic system, there is no heat exchange with the surroundings. During the combustion of methane, the heat generated cannot escape. This results in an increase in temperature within the system.
System B (Diathermic Container): In a diathermic container, heat can flow in and out of the system. During the combustion of methane, the heat generated escapes to maintain constant temperature.
Therefore, in System A, the temperature rises, while in System B, the temperature remains the same.
The solution concludes that the correct option is A, but this corresponds to the statement written as option D in the provided options. Based on the working, the defensible answer is D.
Confusing adiabatic with constant temperature. Adiabatic means no heat exchange with surroundings, not fixed temperature. Here combustion releases heat inside the system, so temperature rises.
Assuming a diathermic container prevents heat transfer. This is incorrect because a diathermic boundary allows heat to pass, helping the system maintain constant temperature.
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