Answer:
-77870 J is the change in internal energy for the system.
Explanation:
According to the first law of thermodynamics:-
[tex]\Delta U = q + w[/tex]
Where,
U is the internal energy
q is the heat
w is the work done
From the question,
q = + 130 J (+ sign as the heat is being absorbed)
[tex]w=-78\ kJ=-78000\ J[/tex] (negative sign as work is done by the system)
So,
[tex]\Delta U = +130\ J-78000\ J = -77870\ J[/tex]
-77870 J is the change in internal energy for the system.
The internal energy change of the system is -77.87 kJ.
From the first law of thermodynamics, energy can neither be created nor destroyed but is converted from one form to another.
Given that;
ΔE = q + w
E = internal energy
q = heat gained/lost
w = work done by or on the system
Since the system was heated, it absorbed heat hence q is positive. The gas expanded so it did work and w is negative.
Hence;
ΔE = 130 J - 78 × 10^3 J
ΔE = -77.87 kJ
Learn more: https://brainly.com/question/1340582
