Abstract: A differential rate equation for silica-water reactions from 0–300°C has been derived based on stoichiometry and activities of the reactants in the reaction SiO2(s) + 2H2O(l) = H4SiO4(aq) (∂aH4SiO4∂t)P.T.M. = (AM)(γH4SiO4)(k+aSiO2a2H2O − k_aH4SiO4) where (AM) = (the relative interfacial area between the solid and aqueous phases/the relative mass of water in the system), and k+ and k− are the rate constants for, respectively, dissolution and precipitation. The rate constant for precipitation of all silica phases is log k− = − 0.707 − 2598T(T, K) and Eact for this reaction is 49.8 kJ mol−1. Corresponding equilibrium constants for this reaction with quartz, cristobalite, or amorphous silica were expressed as log K = a + bT + cT. Using K =k+k−, k was expressed as log k + = a + bT + cT and a corresponding activation energy calculated: abcEact(kJ mol -1)Quarts1.174-2.028 x 103-415867.4–76.6α-Cristobalite-0.7390-358668.7β-Cristobalite-0.9360-339265.0Amorphous silica-0.369-7.890 x 10-4343860.9–64.9 Upon cooling a silica-saturated solution below the equilibrium temperature, the decreasing solubility of silica causes increasing super saturation, which tends to raise the precipitation rate, but the rate constants rapidly decrease, which tends to lower the precipitation rate. These competing effects cause a maximum rate of precipitation 25–50°C below the saturation temperature. At temperatures below that of the maximum rate, silica is often quenched into solution by very slow reaction rates. Consequently, the quartz geothermometer will give the most accurate results if samples are taken from the hottest, highest flow rate, thermal springs which occur above highly fractured areas.
Publication Year: 1980
Publication Date: 1980-11-01
Language: en
Type: article
Indexed In: ['crossref']
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Cited By Count: 1187
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