Question

A system releases 100 kJ of heat while 80 kJ of work is done on the system. Calculate the change in internal energy.
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Answer 1

Answer:

∆u= -20kj

Explanation:

∆Q=∆u+∆w

heat is extracted is taken to be negative.

work on the system is taken to benegative.

Answer 2

The change in internal energy of the system is -180 kJ. This indicates that the system has lost energy.

   

Calculating Internal Energy:

The change in internal energy of a system can be calculated using the first law of thermodynamics: ΔU = Q - W

Where ΔU is the change in internal energy, Q is the heat added to the system, and W is the work done on the system.

From the question,  

Q = -100 kJ

As the energy is released from the system use a negative sign

W = 80 kJ

As the work is being done on the system use a positive sign]

Substituting these values into the equation:

ΔU = -100 kJ - 80 kJ

ΔU = -180 kJ

Therefore,

The change in internal energy of the system is -180 kJ. This indicates that the system has lost energy.

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