Question 1

How are open, closed and isolated systems different?

Accepted Answer

An open system can exchange both matter and energy with its surroundings. A closed system can exchange energy but not matter. An isolated system exchanges neither matter nor energy.

Question 2

What is the difference between extensive and intensive properties?

Accepted Answer

Extensive properties depend on the amount of matter and include mass, volume, amount, internal energy, enthalpy and entropy. Intensive properties do not depend on amount and include pressure, temperature, density and specific heat capacity.

Question 3

What happens when an identical thermodynamic system is split in half?

Accepted Answer

Each half has half the amount, volume, internal energy and entropy when the intensive properties remain unchanged. The two halves together still have the same totals as the original system, while temperature, pressure, density and specific heat capacity remain unchanged.

Question 4

Why are heat and work called path functions?

Accepted Answer

Heat and work describe energy transfer across a system boundary; they are not stored properties of a state. Their values depend on how the system moves between its initial and final states, unlike the change in internal energy or entropy.

Question 5

What does the equation ΔU = q + w mean?

Accepted Answer

It is the thermodynamic sign convention used in this lab. The symbol q is heat absorbed by the system, while w is work done on the system. Under this convention, a positive heat-transfer arrow points toward the system.

Thermodynamics System & Boundary Properties 3D Lab

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