Answer:
The system loses 90 kJ of heat
Explanation:
We can answer the question by using the 1st law of thermodynamics, which states that:
[tex]\Delta U=Q-W[/tex]
where
[tex]\Delta U[/tex] is the change in internal energy of the system
[tex]Q[/tex] is the heat absorbed by the system (positive if absorbed, negative if released by the system)
[tex]W[/tex] is the work done by the system (positive if done by the system, negative if done by the surrounding on the system)
In this problem, we have:
[tex]W=-150 kJ[/tex] is the work done (negative, because it is done by the surrounding on the system)
[tex]\Delta U=+60 kJ[/tex] is the increase in internal energy
Using the equation above, we can find Q, the heat absorbed/released by the system:
[tex]Q=\Delta U+W=+60 kJ+(-150 kJ)=-90 kJ[/tex]
And the negative sign means that the system has lost this heat.
The heat lost by the system from the given data is -110 kJ.
The given parameters;
The energy gained or lost by the system is calculated by applying the first law of thermodynamics as shown below;
ΔU = Q + W
where;
Q = ΔU - W
Q = 60 kJ - 150 kJ
Q = - 110 kJ
Thus, the heat lost by the system is -110 kJ.
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