Calculate the change in internal energy of the following system: a balloon is cooled by removing 0.659 kJ of heat. It shrinks on cooling, and the atmosphere does 384J of work on the balloon.
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To calculate the change in internal energy (ΔU) of the system, we use the first law of thermodynamics:
ΔU = Q - W
where ΔU is the change in internal energy of the system, Q is the heat added or removed from the system, and W is the work done on or by the system.
Given:
Q = -0.659 kJ (heat removed from the system, negative indicates heat removed)
W = 384 J (work done by the system, positive indicates work done)
Converting the heat and work values to the SI unit (Joules):
Q = -0.659 kJ × 1000 J/kJ = -659 J
W = 384 J
Now, plug these values into the equation to calculate the change in internal energy:
ΔU = Q - W
ΔU = -659 J - 384 J
ΔU = -1043 J
Therefore, the change in internal energy of the system is -1043 Joules.
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