BasicThermodynamics 1.3

# BasicThermodynamics 1.3 - MSE 3050 Thermodynamics and...

This preview shows pages 1–3. Sign up to view the full content.

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: MSE 3050, Thermodynamics and Kinetics of Materials, Leonid Zhigilei Heat Capacity The heat capacity, C, of a system is the ratio of the heat added to the system, or withdrawn from the system, to the resultant change in the temperature: C = q/ Δ T = δ q/dT [J/deg] ¾ This definition is only valid in the absence of phase transitions ¾ Usually C is given as specific heat capacity , c, per gram or per mol ¾ New state of the system is not defined by T only, need to specify or constrain second variable: V V dT q C ⎟ ⎠ ⎞ ⎜ ⎝ ⎛ δ = P P dT q C ⎟ ⎠ ⎞ ⎜ ⎝ ⎛ δ =- heat capacity at constant volume- heat capacity at constant pressure The fact that δ q is not a state function and depends on the path is reflected in the dependence of the heat capacity on the path, c p ≠ c v (note that small c is used for the derived intensive quantity, per mass, per volume, or per mole, versus capital C for the extensive quantity. For a system containing n moles C p = nc p and C v = nc v where c p and c v are molar values). c V and c P can be measured experimentally isobaric process: dH = δ q = c P dT isochoric process: dU = δ q = c V dT H and U can be calculated from c P and c V MSE 3050, Thermodynamics and Kinetics of Materials, Leonid Zhigilei c v vs. c p If material is allowed to expand during heating, how this affects its heat capacity?...
View Full Document

{[ snackBarMessage ]}

### Page1 / 5

BasicThermodynamics 1.3 - MSE 3050 Thermodynamics and...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online