Kinetics of the Carbonic Acid Dehydration

Scheurer, Paul G.; Brownell, R. M.; LuValle, James E.

doi:10.1021/j150565a009

Cited by 12 publications

(5 citation statements)

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“…The determination of this quantity, which was a major goal of the early work, was later subordinated to the investigators' kinetic interests. Several authors (30,32) have recently revived Saal's zero-time pH method, for whicli the latest rapid mixing apparatus is well-adapted. The new values are significantly lower than the earlier ones (Table 3).…”

Section: Postwar Electicism and The Stopped Flow Methodsmentioning

confidence: 99%

“…When solutions of weak electrolytes are subjected to alternating fields of up to 200 kv/cm, there is superimposed on the usual Wien effect a further enhancement of the conductivity caused by the increased dissociation in 8 From Figure 2 it appears that Saal's experiments were free from this disturbing effect. Scheurer(1958) 1.9 * The early work is difficult to evaluate because of inadequate correction for ionic strength. The dissociation is almost double at = 0.1 (Harnee, H., and Bonner, F., J.…”

Section: Postwar Electicism and The Stopped Flow Methodsmentioning

confidence: 99%

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The hydration of carbon dioxide

Kern¹

1960

J. Chem. Educ.

419

200

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Section: Postwar Electicism and The Stopped Flow Methodsmentioning

confidence: 99%

Section: Postwar Electicism and The Stopped Flow Methodsmentioning

confidence: 99%

The hydration of carbon dioxide

Kern¹

1960

J. Chem. Educ.

419

200

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“…The value of yHCO-in KCI1 is taken from Walker et al (1927), whereas yH+ in K Owen (1943). We have assumed that amtcot [H2C 0 3] is a reaso Berger (1968) continuous flow, potentiom etric 26 Gibbons & Edsall (1963) stopped flow, spectrophotometric 14 Magid & Turbeck (1968) pH -stat 18 Scheuer et al (1958) stopped flow, spectrophotometric 22 Eigen et al (1961) tem perature jum p 15 Pearson et a l . (1956) continuous flow, conductometric 28 Berger & Stoddart (1965) stopped flow, spectrophotometric 24 stopped flow, thermometric 22 Sirs (1958) stopped flow, potentiom etric 24 Rough ton (1941) continuous flow, therm om etric 28 Gibson & Roughton (1955) stopped flow, spectrophotometric 22 Brinkman et al (1933) continuous flow, photoelectric 23 m anom etric C 0 2 determ ination 20…”

Section: T Heorymentioning

confidence: 99%

The dissolution of calcite in aqueous solution at pH < 4: kinetics and mechanism

Compton

Unwin

1990

Phil. Trans. R. Soc. Lond. A

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The requirements of any experimental investigation of a reaction, such as dissolution or precipitation, at the solid-liquid interface are delineated, and it is shown that no previously adopted experimental method successfully meets all of these criteria. A new strategy for studying such reactions is therefore proposed, and described specifically for the dissolution kinetics of calcium carbonate in acidic aqueous solution. This technique involves locating a calcite crystal in part of one wall of a rectangular duct, through which reactant flows under laminar conditions, and positioning either an amperometric or potentiometric detector electrode immediately adjacent to and downstream of the crystal. The rate of the reaction at the crystal surface is then followed by measuring the concentration of the reactant or products reaching the electrode as a function of solution flow rate. In this way both transport (to the crystal and detection system) and the surface topography of the crystal are defined and controllable, and, most importantly, the concentrations interrogated by the detector electrode are those pertaining at the crystal surface and not the bulk values, which are those probed with other (previous) methods. A mechanistic model for the dissolution reaction at pH < 4, H + + CaCO 3 → C a 2 + + HCO 3 − , is developed, and it is recognized that half-, first- and second-order reactions in surface H + constitute possible candidate heterogeneous processes. The model also takes the following homogeneous (solution) reactions into account: HCO 3 − + H + ⇌ H 2 C O 3 ⟶ k H 2 C O 3 C O 2 + H 2 O , K H 2 C O 3 = a H + a HCO 3 − / a H 2 C O 3 The backward implicit finite difference method is used to provide theory for the proposed flow cell experiment. Specifically this relates the rate of an n th order process at the crystal surface to the transport-limited current at an amperometric detector electrode, as a function of solution flow rate and cell-crystal-electrode geometry. The computational method selected allows both the full parabolic velocity profile and any value of n to be considered. The validity of the numerical approach is checked by invoking the Lévêque approximation (linearizing the parabolic velocity profile) and solving the problem analytically for n = 0 and 1. The numerical method is extended so that both parallel heterogeneous and homogeneous reactions are covered, specifically so that theory describing the mechanistic model can be derived as related to the flow cell experiment. The design and construction of the necessary experimental apparatus is described, along with experiments devised to prove the validity of the experimental approach. The results of flow cell dissolution experiments carried out with 0.25–1.0 mM HCl solutions are presented, and it is shown for the first time that the reaction between H + and calcite is not transport-controlled. Assuming k H 2 C O 3 = 20 s − 1 and K H 2 C O 3 = 3.06 × 1 0 − 4 M , a best fit to the data is obtained for a first-order heterogeneous process with a rate constant of (0.043 ± 0.015) cm s -1 .

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“…The rate laws are linear and no back reactions are involved. This simplicity is directly responsible for the analytical integrability of equations (13)(14)(15).…”

Section: Hydrolysis Of Tripolyphosphatementioning

confidence: 99%