Q.One mole of a monatomic ideal gas ($\gamma = 5/3$) expands adiabatically and reversibly, its temperature falling from $500\ \text{K}$ to $350\ \text{K}$. Calculate the work done by the gas during this expansion. (Take $R = 8.314\ \text{J mol}^{-1}\text{K}^{-1}$.)

A process with $Q = 0$ throughout — no heat enters or leaves the system — is called adiabatic.

By definition, an adiabatic process is one that occurs without any exchange of heat between the system and its surroundings, i.e. $dQ = 0$ at every stage. This is achieved either by thermally insulating the system (perfectly non-conducting walls) or by carrying out the process so quickly that there is no time for heat to flow.

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A sudden tyre burst happens so fast that there is no time for heat to be exchanged with the surroundings, which is the defining condition of an adiabatic process.

An adiabatic process is one in which no heat enters or leaves the system (Q = 0); any change in internal energy occurs purely due to work done by or on the gas.

When a cycle tyre bursts, the compressed air inside expands almost instantaneously. This expansion happens on a timescale far too short for heat to flow between the escaping air and its surroundings.

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