 ###### Main Sections

1. Microprobe analyses

2. Mineral groups

3. Solid solutions

4. Thermobarometers 5. Uncertainties

6. P-T calculations

7. Phase diagrams

8. THERMOCALC tips

###### THERMOCALC Stuff

Activity coding

Applications

Bibliography

Bugs and quirks

Bulk compositions

Modal proportions

# Practical Aspects of Mineral Thermobarometry

## Thermobarometer Calibration

The aim of this section will be to cover briefly such topics such as

• Conditions of heterogeneous equilibrium
• The equilibrium constant and its P-T dependence.
• A simple geothermometer: garnet-biotite Fe-Mg exchange
• A geobarometer based on a net-transfer reaction with large volume change
• How thermometers and barometers are calibrated
• Self-consistent thermodynamic data sets and their application to thermobarometry

You can read about these subjects in Spear 1993, chapter 8, pp. 241-244, and chapter 15, pp. 511-537.

Here's some provisional content, from lecture course handouts:

#### Condition for heterogeneous equilibrium

[Spear, p. 511]. A balanced chemical reaction such as Grs + 2 Ky + Qtz = 3 An could also be written in the form 3 An - Grs - 2 Ky - Qtz = 0, reminding us that the mass of each system component is conserved, and that reaction coefficients can be positive ("products") or negative ("reactants"). At equilibrium, a similar relationship holds among the chemical potentials of phase components (n are the reaction coefficients and there are m phase components): i.e. there is no free energy difference between "reactants" and "products".

#### Expand the expression for heterogeneous equilibrium

[Spear, p. 512]. Adding up, for all the phase components, the expressions µi = µ°i + RTln(ai), gives us GR = 0 = G0 + RTlnK

where K is the equilibrium constant or activity product, which depends on measured phase compositions. G0 is the standard state free energy change - something we can calculate if we have thermochemical data. Expanding G0 to see what thermochemical data are needed, we get: The subscripts and limits reflect the fact that thermochemical data are generally tabulated at 298K and 1 bar.

#### Linear approximation for solid-solid reactions

[Spear, p. 523]. CP  = 0. The CP terms adjust H and S for different P and T. The heat capacities of solid phases vary sympathetically, so CP is small, and can often be ignored, particularly over small ranges of temperature. V constant. The volume integral brings the enthalpies from their reference pressure P0 (1 bar) up to the pressure of interest (usually several thousand bars). V is not a function of P or T if all solids are roughly equally compressible, so the volume integral becomes V(P - P0). Also, P0 is negligible compared to P.

This gives us the greatly simplified expression which, for a given value of lnK, is the equation of a straight line on a P-T diagram. The curve for lnK = 0 (i.e. K = 1) is the curve for pure phases, such as might be determined in the experimental laboratory. Other values of lnK displace the curve across the P-T diagram.

#### Dependence of lnK on T and P

[Spear, pp. 515-6]  where S and V are calculated at the P and T of interest. Also remember the Clausius-Clapeyron equation: ; or, more strictly, Therefore, a good geobarometer needs a large V, in order to have a large sensitivity to P and for curves of constant K to have a low slope on the P-T diagram.

### Geothermometry and geobarometry using multivariant equilibria

At equilibrium

DGP,T = DH1,T - T.DST + (P-1).DV + RT.lnK = 0

K is the equilibrium constant, the product of the activities of end members in the phases of variable composition.

#### The Grt-Pl-Ky-Qtz geobarometer

Ca3Al2Si3O12 + 2Al2SiO5 + SiO2 = 3CaAl2Si2O8

grossular(Grt) + kyanite + quartz = anorthite(Pl)

Substituting thermochemical data, dividing through by the gas constant R, and expanding K gives the calibration:

7635 - 19.66T + 0.7963(P-1) + 3Tln(XCa,Pl /XCa,Grt) = 0

DV is large, because of the density difference between open feldspar and close-packed garnet and kyanite structures. The P-T slope is relatively low, making this equilibrium useful as a barometer. Uncertainty on calculated P is about ± 1.3 kbar.

#### The Grt-Bt Fe-Mg exchange thermometer

Fe3Al2Si3O12 + KMg3AlSi3O10(OH)2 = Mg3Al2Si3O12 + KFe3AlSi3O10(OH)2

Almandine (Grt) + Phlogopite (Bt) = Pyrope(Grt) + Annite (Bt)

DG for cation exchange is small, and the calibration here is fitted to exchange equilibrium experiments

6266 - 2.35T + 0.029(P-1) + 3TlnKD = 0

KD is most simply expressed as (Mg/Fe)Grt /(Mg/Fe)Bt

DV is very small, and cation exchange equilibria are generally insensitive to pressure. The usually-quoted uncertainty on calculated T is ± 50°.

#### Application

An amphibolite-facies metapelitic schist from the Eastern Alps contains garnet of composition (% end members) Alm80Sps3Prp13.5Grs3.5 , biotite with Mg/Fe = 0.91, and plagioclase An15 , together in apparent equilibrium with kyanite and quartz. From these data we calculate the two P-T curves. Their intersection (with a surrounding box of uncertainty) gives us an estimate of the conditions of equilibration. ## Self-consistent data-sets

[ Material to incorporate from Petrology course lecture slides ]

^ Top