Understanding Open Systems in Thermodynamics
An open system in thermodynamics is defined by its interaction with the surroundings. It allows for the transfer of both energy and matter across its boundaries.
Defining System Boundaries
- Open System: Characterized by the exchange of both energy (like heat or work) and matter with its surroundings.
- Closed System: Allows exchange of energy but prevents the transfer of matter.
- Isolated System: Permits neither energy nor matter transfer.
Based on these definitions, the correct statement describing an open system is that it involves the exchange of both energy and matter.
Analyzing the Options
- Option 1: States that energy and matter are exchanged. This matches the definition of an open system.
- Option 2: Incorrectly states no energy exchange is possible.
- Option 3: Describes an isolated system, not an open one.
- Option 4: Incorrectly states no matter exchange is possible.
Therefore, the statement accurately describing an open system is the one allowing both energy and matter exchange.
Important Questions from First Law of Thermodynamics
A system is said to be in thermodynamic equilibrium if the system is in:
Isothermal expansivity of an ideal gas is
The first law of thermodynamics is equivalent to the principle of conservation of
For an adiabatic process the first law of thermodynamics becomes
Heat transfer in a cyclic process are +20 kJ, -5 kJ, -10 kJ and +15kJ. Net work done for this cycle will be given by:
