Question

What is the change of energy on the surrounding when a system does 15jul of work on the surrounding and 13jul  of work are added to the system?
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Answer 1

The first law, which deals with changes in the internal energy, thus becomes 0 = Q - W, so Q = W. If the system does work, the energy comes from heat flowing into the system from the reservoir; if work is done on the system, heat flows out of the system to the reservoir.

Any other means for changing the energy of a system is called work. ... Thus we define work as being positive when the system does work on the surroundings (energy leaves the system). If work is done on the system (energy added to the system), the work is negative.

In equation form, the first law of thermodynamics is ΔU = Q − W. Here ΔU is the change in internal energy U of the system. Q is the net heat transferred into the system—that is, Q is the sum of all heat transfer into and out of the system.

When matter transfer is prevented by impermeable containing walls, the system is said to be closed and the first law of thermodynamics defines the change in internal energy as the difference between the energy added to the system as heat and the thermodynamic work done by the system on its surroundings.

Any other means for changing the energy of a system is called work. ... Thus we define work as being positive when the system does work on the surroundings (energy leaves the system). If work is done on the system (energy added to the system), the work is negative.

The change in the internal energy of a system is equal to the difference between the final and initial energies of the system: The equation for the first law of thermodynamics can be rearranged to show the energy of a system in terms of the energy of its surroundings.

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