5 posts • Page 1 of 1
The first law of thermodynamics states that the internal energy (delta U) of an isolated system is constant. This means that delta U = 0 in an isolated system, because no energy can be transferred to/from the system and no work can be done on or is being done by the system.
Looking at the equation Delta U = q + w, delta U is only 0 when q = -w which means heat put into the system is equal to the heat out of the system, in other words the system is isolated with no net change in internal energy.
Who is online
Users browsing this forum: No registered users and 2 guests