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(C) When a gas cylinder explodes suddenly,the process is extremely rapid,meaning there is no time for heat exchange with the surroundings,which charac

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Irreversible adiabatic change and fall of temperature

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(C) When a gas cylinder explodes suddenly,the process is extremely rapid,meaning there is no time for heat exchange with the surroundings,which characterizes an adiabatic process. Since the process occurs spontaneously and rapidly against external atmospheric pressure,it is irreversible. According to the first law of thermodynamics,$dQ = dU + dW$. For an adiabatic process,$dQ = 0$,so $dU = -dW$. As the gas expands rapidly,it performs work on the surroundings $(dW > 0)$,which leads to a decrease in internal energy $(dU Since the internal energy of an ideal gas is directly proportional to its temperature,a decrease in internal energy results in a fall in temperature.

If a cylinder containing a gas at high pressure explodes,the gas undergoes

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