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According to the first law of thermodynamics, what happens to the internal energ

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Question: According to the first law of thermodynamics, what happens to the internal energy of a system when heat is added and work is done by the system?

Options:

  1. Increases
  2. Decreases
  3. Remains constant
  4. Cannot be determined

Correct Answer: Decreases

Solution: 

The first law states ΔU = Q - W. If heat Q is added and work W is done by the system, the internal energy decreases.

According to the first law of thermodynamics, what happens to the internal energ

Practice Questions

Q1
According to the first law of thermodynamics, what happens to the internal energy of a system when heat is added and work is done by the system?
  1. Increases
  2. Decreases
  3. Remains constant
  4. Cannot be determined

Questions & Step-by-Step Solutions

According to the first law of thermodynamics, what happens to the internal energy of a system when heat is added and work is done by the system?
  • Step 1: Understand the first law of thermodynamics, which is expressed as ΔU = Q - W.
  • Step 2: Identify what each symbol means: ΔU is the change in internal energy, Q is the heat added to the system, and W is the work done by the system.
  • Step 3: Recognize that when heat (Q) is added to the system, it increases the internal energy.
  • Step 4: Understand that when work (W) is done by the system, it takes energy away from the internal energy.
  • Step 5: Combine these ideas: If heat is added (positive Q) and work is done by the system (positive W), the equation becomes ΔU = positive Q - positive W.
  • Step 6: Conclude that if the amount of work done (W) is greater than the heat added (Q), the internal energy (ΔU) will decrease.
  • First Law of Thermodynamics – The first law states that the change in internal energy (ΔU) of a system is equal to the heat added to the system (Q) minus the work done by the system (W).
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