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First Law Fundamentals

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First Law Fundamentals

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Fundamental energy conservation

Created by

Saipreeti Gouripeddi
Saipreeti Gouripeddi
India

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First Law Fundamentals
 

First Law FundamentalsOnline version

Fundamental energy conservation

by Saipreeti Gouripeddi
1

If an isolated system undergoes a process, what is ΔU (change in internal energy)?

2

Zeroth law implies what about thermal equilibrium and temperature?

3

Which quantity is a state function: internal energy, heat, or work?

4

Numerical: A system receives q = 500 J and does w = -200 J of work on the surroundings. Find ΔU.

5

Which best describes a system versus its surroundings?

6

In the first law, which convention is commonly used: q in = heat added to system; w by system = work done by system?

7

Which statement best defines equilibrium in thermodynamics?

8

For an ideal gas in an isothermal process, what is ΔU?

9

Which is a true statement about state functions?

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In an isolated system, q=0 and w=0, so ΔU = q + w = 0.

Thermal equilibrium is transitive; equal temperatures imply mutual equilibrium.

State functions depend only on the state, not on the path; internal energy is a state function.

ΔU = q + w; 500 + (-200) = 300 J.

The system is what you analyze; surroundings are everything else beyond its boundary.

Common convention: q in (positive for heat added), w by system (positive for work done by system).

Equilibrium means no net macroscopic change without external influence.

For an ideal gas, internal energy depends only on temperature; isothermal means T constant, so ΔU = 0.

State functions like U, H, S depend only on state, not the path.

 
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