Conversely, if the energy in the system is reduced then system temperature decreases.Ĭhange in system pressure and volume in the adiabatic process is illustrated by the graph below: The energy in the system (ideal gas) is proportional to the temperature (U = 3/2 n R T), therefore if the energy in the system increases then system temperature also increases. Since W is positive, U is negative (energy in the system is reduced). Conversely, if the system expands quickly (system does work), then W is positive. Because W is negative, then U is positive (energy in the system increases). If the system is pressed quickly (work is done on the system), then work is negative. No heat is in or out of the system, so Q = 0. If applied to an adiabatic process, first law Thermodynamic equation will change: In this case, the process must be done very quickly so that heat does not flow to the system or leave the system. Adiabatic processes can also occur in closed systems that are not isolated. For a well-insulated closed system, there is usually no heat that flows into the system or leaves the system. Adiabatic processes can occur in well-isolated closed systems. In the adiabatic process, no heat is added to the system or leaves the system (Q = 0).
Amount of work done system = shaded area. The shape of the graph is curved because system pressure does not change regularly during the process. After system does work on the environment, system volume changes to V 2 (system volume increases) and system pressure changes to P 2 (system pressure decrease). For the system temperature to be constant then after heat is added to the system, the system expands and does work on the environment. Internal energy does not change, so Δ U = 0.īased on this equation, in the isothermal process (constant temperature), heat (Q) added to the system is used by the system to perform work (W).Ĭhange in pressure and volume of the system in the isothermal process is illustrated by the graph below:įirst system volume = V 1 (small volume) and system pressure = P 1 (big pressure). Thus, if applied to the isothermal process, the first law of thermodynamic equation becomes: T does not change, so U also does not change. Ideal gas temperature is directly proportional to ideal internal gas energy (U = 3/2 n R T). Theoretically, the analyzed system is an ideal gas. In an isothermal process, system temperature is kept constant. Isothermal Process (constant temperature) There are four thermodynamic processes, namely Isothermal, isochoric, isobaric and adiabatic processes. Article Thermodynamic processes : Isothermal Adiabatic Isochoric Isobaric
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