Question

Heat and Thermodynamics: Question 1 A system loses 250 J of heat to the environment while the environment does 250 J of work on the system. What is the change in internal energy of the system?

Answer 1

0 J

Step-by-step explanation:

The change in internal energy of the system can be determined using the first law of thermodynamics, which is expressed as:

`\Delta E_{\text{int.}}=Q+W_{\text{on}}`

Where:

• 'ΔE_int.' is the change in internal energy.

• 'Q' is the heat added to the system (if the system loses heat, this value is negative).

• 'W_on' is the work done on the system (if the system does work, this value is negative).

In our case:

• The system loses 250 J of heat to the environment, so Q = −250 J.
• The environment does 250 J of work on the system, so W_on = +250J.

Plug in our values:

`\Longrightarrow \Delta E_{\text{int.}}=-250 \text{ J}+250 \text{ J}\\\\\\\\\therefore \Delta E_{\text{int.}}= \boxed{0 \text{ J}}`

The change in internal energy of the system is 0 J. This means that the internal energy of the system remains unchanged.