Heat And Work Flashcards
Describe an isolated system
- no exchange of matter
- no exchange of energy (heat)
Describe closed system
- no matter exchange
- it can exchange energy (heat)
Describe open system
- it can exchange energy (heat)
- it can exchange matter
how do we differentiate between absolute and specific quantities?
Uppercase – absolute quantities
Lower case – specific quantities
define absolute and specific quantities
absolute quantities = normal
specific (relative) quantities = absolute quantity divided by some other quantity
define steady and unsteady flow
steady = constant flow rate
unsteady = variable flow rate
what are processes on a fluid in a closed and open system called?
Non-Flow Processes and Flow Processes respectively
When work (W) is said to be done by a thermodynamic system, is that work +W or –W ?
+W
When work (W) is said to be done on a thermodynamic system, is that work +W or –W ?
–W
When heat is added to a thermodynamic system, is the heat flow (Q) said to be +Q or –Q ?
+Q
The state of a thermodynamic system can be defined by the change in its properties. Do the changes in these properties depend on the intermediate states or are they irrespective of the intermediate values?
The change in thermodynamic properties during a process is independent of the intermediate states of the system. Depends only on the initial and final states of the system.
When work is done in a thermodynamic system, does it depend on the intermediate states?
the work done in a thermodynamic process is determined by the initial and final states and is not affected by the intermediate states through which the system passes.
When the fluid in a thermodynamic system is in thermal equilibrium, is this described as a reversible or irreversible system?
whether the system is described as reversible or irreversible depends on the nature of the process leading to thermal equilibrium. If the process leading to thermal equilibrium is reversible, the system can be described as reversible. If not, it’s considered irreversible.
