Respuesta :
The change in the internal energy of the system after absorbing the energy is [tex]\boxed{40\,{\text{J}}}[/tex] .
Further Explanation:
Given:
The energy absorbed by the system from the surroundings is [tex]12\,{\text{J}}[/tex] .
The work done by the surroundings on the system is [tex]28\,{\text{J}}[/tex] .
Concept:
Since there is some amount of the work done on the system and the system also absorbs some amount of energy from the surroundings, the change in internal energy of the system is given by the First Law of Thermodynamics.
The First Law of Thermodynamics state that the total energy of an isolated system is always conserved. It means that the change in the internal energy of the system is equal to the sum of the amount of energy absorbed by the system and the amount of work done by the surroundings on the system.
[tex]\Delta U=Q+W[/tex]
Here, [tex]\Delta U[/tex] is the change in internal energy of the system, [tex]Q[/tex] is the energy absorbed by the system and [tex]W[/tex] is the work done on the system.
Substitute the value of the energy absorbed and the work done in above expression.
[tex]\begin{aligned}\Delta U&=12\,{\text{J}}+28\,{\text{J}}\\&={\text{40}}\,{\text{J}}\\\end{aligned}[/tex]
Thus, the change in the internal energy of the system is [tex]\boxed{40\,{\text{J}}}[/tex] .
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Answer Details:
Grade: College
Subject: Physics
Chapter: Heat and Thermodynamics
Keywords:
System absorbs, heat from surroundings, work done, energy absorbed, change in internal energy, first law of thermodynamics,
