A gas expands against a non-zero external pressure while in...

A gas expands against a non-zero external pressure while in thermal isolation from the surroundings. For this expansion
a. $\Delta \mathrm{E}=\mathrm{q}$
b. $\Delta \mathrm{E}$ increases
c. $\Delta \mathrm{E}$ does not change
d. $\Delta \mathrm{E}$ decreases

Key Concepts

Internal Energy

Internal energy is the total energy contained within a system, encompassing kinetic and potential energies of molecules. It is a state function that changes in response to heat exchange and work done. In an adiabatic expansion, since there is no heat input, the internal energy change is entirely due to the work done by the gas, often resulting in a decrease in energy.

Work in Thermodynamics

Work in thermodynamics refers to the energy transferred when an external force acts upon a system, such as during expansion or compression. When a gas expands against a non-zero external pressure, it performs work on the surroundings. This work is taken from the internal energy of the gas, leading to a decrease in its internal energy in an adiabatic process.

Adiabatic Process

An adiabatic process is one in which no heat is exchanged with the surroundings. As a result, any energy change in the system is solely due to the work done by or on the system. In the context of a gas expanding in thermal isolation, the absence of heat exchange means that the internal energy change is directly related to the work performed.

First Law of Thermodynamics

The First Law of Thermodynamics states that energy can neither be created nor destroyed, only transferred or transformed. In thermodynamic processes, the change in internal energy of a system is equal to the heat added to the system plus the work done on it. This principle provides the foundation for analyzing energy changes during processes such as expansion or compression of gases.

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