Thermodynamic systems and energy accounts
| English | 中文 | Pinyin |
|---|---|---|
| internal energy/ɪnˈtɜːnl ˈenədʒi/ | 内能 | nèi néng |
| adiabatic/ˌædiəˈbætɪk/ | 绝热的 | jué rè de |
What would explain this observation?
- Compressing a gas can warm it even without a heater. Work is another path for energy transfer into the system.
- Start with a prediction. State the quantities or features you would compare, then decide what evidence could distinguish two explanations.
Build the model
- Internal energy 内能 is a property of the chosen system. Heat and work describe energy transfer across its boundary. For an ideal monatomic gas, internal energy depends on temperature and amount.
- adiabatic 绝热的: A process with no heat transfer; internal energy: Total microscopic kinetic and potential energy of a system.
In this convention, what happens during adiabatic compression?
State a sign convention before using the first law. Here change in internal energy equals heat into the system minus work done by the system. Expansion work can reduce internal energy when no heat enters.
Match each technical term to its precise meaning.
Use the definitions to distinguish related quantities and processes.
Choose evidence that can test it
- State a sign convention before using the first law. Here change in internal energy equals heat into the system minus work done by the system. Expansion work can reduce internal energy when no heat enters.
- Identify whether a process is isothermal, adiabatic or at constant volume. On a pressure-volume graph, area under the process curve gives work done by the gas. The path matters for work even when endpoints match.
Which two habits make the investigation or model in this case more defensible?
Identify whether a process is isothermal, adiabatic or at constant volume. On a pressure-volume graph, area under the process curve gives work done by the gas. The path matters for work even when endpoints match.
Work from known quantities
- State the known values and their units. Choose the relation because its assumptions fit this case, then rearrange before substitution.
- Known: gas gains 300 J by heating and does 120 J of work. With ΔU = Q-W, ΔU = 300-120 = 180 J. For adiabatic compression, Q=0 and work done by the gas is negative, so ΔU is positive.
A gas gains 500 J of heat and does 200 J work. Find internal-energy change. Use the same sequence: known quantities → model → relation → substitution → unit and interpretation.
A gas gains 500 J of heat and does 200 J work. Find internal-energy change.
The result is 300 J. Known: gas gains 300 J by heating and does 120 J of work. With ΔU = Q-W, ΔU = 300-120 = 180 J. For adiabatic compression, Q=0 and work done by the gas is negative, so ΔU is positive.
Check the conclusion and its limits
- Adiabatic does not mean constant temperature. Use the stated sign convention; some courses write work done on the gas with the opposite sign.
- Return to the original observation. Explain what the result supports, which conditions it assumes, and one way to test a competing explanation.
Every adiabatic process has constant temperature. This claim is false: Adiabatic does not mean constant temperature. Use the stated sign convention; some courses write work done on the gas with the opposite sign.
Thermodynamic systems and energy accounts: State a sign convention before using the first law. Here change in internal energy equals heat into the system minus work done by the system. Expansion work can reduce internal energy when no heat enters.
Every adiabatic process has constant temperature.
Adiabatic does not mean constant temperature. Use the stated sign convention; some courses write work done on the gas with the opposite sign.
A process with no heat transfer: write the technical term.
adiabatic means A process with no heat transfer.