PChem312 f20 w3

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Monday, Aug 31, 2020

Continue reading chapter 2

Sec 2.1: Internal Energy and !st Law of Thermodynamics

U <-- internal energy (1st thermodynamic state function)

U_f - U_i = ΔU, the change in the internal energy

• we cannot measure U_f or U_i, only ΔU.

First Law of Thermodynamics: the change in the system's internal energy is equal to, but opposite in sign, to the change in the surround's internal energy.

ΔU_sys = - ΔU_surr

How does one measure ΔU?

- changes in the system variables (ΔP, ΔV, ΔT, Δn) are an indication of ΔU; changes in system variables result in either heat (q) transfer or work (w) being done on or by the system; calculation of q or w leads directly to ΔU.

ΔP, ΔV, ΔT, Δn --> q (heat), w (work) --> ΔU

Heat and work are both defined as a transfer of energy between the system and surroundings.

The first Law of thermodynamics can also be stated as:

ΔU = q + w

Sec 2.2: Heat (q)

Heat is transitory; heat is not a thing. We DO NOT use the term Δq (for change in heat), we instead say that heat flows from one place to another.

Heat naturally flows from hotter/higher temperature to cooler/lower temperature objects (Zeroth Law of Thermodynamics).

Heat sign convention

- we speak of heat from the perspective of the system (unless otherwise stated).

- when the system loses heat, we identify this quantity of heat as negative, -q; loss of heat is generally associated with a decrease in temperature, ↓T.

- when the system gains heat, we identify this quantity of heat as positive, +q or q; ; gain of heat is generally associated with a increase in temperature, ↑T.

Sec 2.2: Work (w)

work is transitory, only energy, not work is associated with the initial or final states. We DO NOT use the term Δw (for change in work), we instead say that work was done on or by the system.

Work occurs when a force is applied by the system or on the surroundings.

Thursday, Sept 3, 2020

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