chemical physics of discharges - Argonne National Laboratory
chemical physics of discharges - Argonne National Laboratory chemical physics of discharges - Argonne National Laboratory
214 states of molecular oqgen are also present. It is instructive to compare these results with measurements of the activation energy of graphite with atomic oxygen removed from the luminous discharge. In severearly studies a vdue of zero was reported (2) (16). Hennig (8) observed no dependence on temperature at a pressure of 1.0 torr and a value of 7 Kcal/mol at 10 torr. This difference was attributed to ozone formation. In a recent detailed study of the atomic oxygen-graphite reaction, Marsh et al. (U) reported an activation energy of 10 Kcal/mol between U and 2OO0C, which approached zero at 350°C. 'Although the rate of oxidation in these studies was considerably lower than that obtained in the plasm, their values are consistent with the belief that atomic oqygen is a major reactant within the discharge. Of a variety of specimens, only graphite exhibited an abrupt change in activation energy near 3Oo0C. For example, the apparent activation energy in the decomposition of sucrose is approximately 4 Xcal/mol over the entire measurement range. The independence of oxidation rate for graphite at high temperatures is ascribed to the formation of surface oxides. Numerous studies of graphite combustion have shown that such surface compounds control rate at elevated temperatures in excess oxygen. As anticipated, increasing radiofreqiiency power to the discharge does not measurablv increase the rate of graphite oxidation at high sample temperature. The exhaust gas of the ovgen-graphite reaction contains both carbon monoxide a d carbon dioxide, with the latter predominating. Tn the lumi~ous discharge region these gases react with graphite. The results of measuremepts in which carbon dioxide was passed through the radiofrequency field and then exposed to graphite rods activated are shown in figure 3. Between 150 and 4OOOC the Arhennius equation fits well, yielding an apparent activation energy of 3.2 Kcal,/mol. Below 120°C less than one mg per hour of carbon was removed. This small weight loss is attributed to ion and electron bombardment. W& Conditions: In a number of experiments, increasing power beyond an optimum value led to the anomolous result of reducing ashing rate. Earlier it was noted that placing a dry ice-acetone trap in the exhaust stream extended the length of the luminous discharge (5). To study this effect, wall temperatures were varied while the carbon rod was maintained at 200°C. The results of a series of measurements are shown in figure 4. Assuming that the decrease in oxidation rate at increased wall tempera- ture ip due to recombination of active species at the wall, the overall activation energy at low temperatures for this process is approximately 2 Kcal/ml. The major sources leading to loss of active oxygen species are recombination of atomic oxygen and ions at the'walls of the vessel. The recombination of discharged oxygen on glass surfaces has been investigated. Linnett and Marsden (10) reported that the recombination coefficient of atomic oxygen on clean borosilicate glass (Pyrex) was independent of temperature. However, positive values were observed on contaminated surfaces. In a later series of papers Greaves and Linnett (7) studied a number of oxide surfaces, in all cases the recombination coefficient was temperature ' dependent. For silica apparent activation energies were 1 to 13 Kcal/mol over the temperature range 15 to 3OOOC. The exceptional nature of Pyrex was noted. ' The second major source of loss of active species results from electron-ion recombination at the chamber walls. The electric field restricts the drift of ions to the chamber walls. Rate of-recombination is controlled by ambipolar diffusion, but is limited by the presence of negatively charged oqgen ions in the discharge (15). Although diffusion is not dependent on wall temperature, a distortion of the symmetric electrical field will enhance wall recombination, producing an inarease in This effect is noted in t&le 1. The presence of a 6-cm long metallic ring on the exterior wall of the reduced oddation rate by more than ten per cent. Grounding the ring in comn with . wall temperature and a reduction of oxidation rate. < / I 1 I
'i' 100 50 IC 21 5 2.0 2.5 SURFACE TEMPERATURE, I/T i103 Fig. 3. Rate of gassification vs. temperature for graphite rods exposed to carbon dioxide discharge. 5c 4c 3c 20 IC 1.5 2 .o 2.5 3.0 3.5 WALL TEMPERATURE, x lo3 Fig. 4. Effect of wall temperature on the oxidation rate of graphite.
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214<br />
states <strong>of</strong> molecular oqgen are also present.<br />
It is instructive to compare these results with measurements <strong>of</strong> the activation<br />
energy <strong>of</strong> graphite with atomic oxygen removed from the luminous discharge. In severearly<br />
studies a vdue <strong>of</strong> zero was reported (2) (16). Hennig (8) observed no dependence<br />
on temperature at a pressure <strong>of</strong> 1.0 torr and a value <strong>of</strong> 7 Kcal/mol at 10 torr. This<br />
difference was attributed to ozone formation. In a recent detailed study <strong>of</strong> the<br />
atomic oxygen-graphite reaction, Marsh et al. (U) reported an activation energy <strong>of</strong><br />
10 Kcal/mol between U and 2OO0C, which approached zero at 350°C. 'Although the rate<br />
<strong>of</strong> oxidation in these studies was considerably lower than that obtained in the plasm,<br />
their values are consistent with the belief that atomic oqygen is a major reactant<br />
within the discharge.<br />
Of a variety <strong>of</strong> specimens, only graphite exhibited an abrupt change in activation<br />
energy near 3Oo0C. For example, the apparent activation energy in the decomposition<br />
<strong>of</strong> sucrose is approximately 4 Xcal/mol over the entire measurement range. The independence<br />
<strong>of</strong> oxidation rate for graphite at high temperatures is ascribed to the formation<br />
<strong>of</strong> surface oxides. Numerous studies <strong>of</strong> graphite combustion have shown that such surface<br />
compounds control rate at elevated temperatures in excess oxygen. As anticipated,<br />
increasing radi<strong>of</strong>reqiiency power to the discharge does not measurablv increase the rate<br />
<strong>of</strong> graphite oxidation at high sample temperature.<br />
The exhaust gas <strong>of</strong> the ovgen-graphite reaction contains both carbon monoxide a d<br />
carbon dioxide, with the latter predominating. Tn the lumi~ous discharge region these<br />
gases react with graphite. The results <strong>of</strong> measuremepts in which carbon dioxide was<br />
passed through the radi<strong>of</strong>requency field and then exposed to graphite rods activated<br />
are shown in figure 3. Between 150 and 4OOOC the Arhennius equation fits well, yielding<br />
an apparent activation energy <strong>of</strong> 3.2 Kcal,/mol. Below 120°C less than one mg per<br />
hour <strong>of</strong> carbon was removed. This small weight loss is attributed to ion and electron<br />
bombardment.<br />
W& Conditions: In a number <strong>of</strong> experiments, increasing power beyond an optimum<br />
value led to the anomolous result <strong>of</strong> reducing ashing rate. Earlier it was noted that<br />
placing a dry ice-acetone trap in the exhaust stream extended the length <strong>of</strong> the luminous<br />
discharge (5). To study this effect, wall temperatures were varied while the<br />
carbon rod was maintained at 200°C. The results <strong>of</strong> a series <strong>of</strong> measurements are shown<br />
in figure 4.<br />
Assuming that the decrease in oxidation rate at increased wall tempera-<br />
ture ip due to recombination <strong>of</strong> active species at the wall, the overall activation<br />
energy at low temperatures for this process is approximately 2 Kcal/ml.<br />
The major sources leading to loss <strong>of</strong> active oxygen species are recombination <strong>of</strong><br />
atomic oxygen and ions at the'walls <strong>of</strong> the vessel. The recombination <strong>of</strong> discharged<br />
oxygen on glass surfaces has been investigated. Linnett and Marsden (10) reported<br />
that the recombination coefficient <strong>of</strong> atomic oxygen on clean borosilicate glass<br />
(Pyrex) was independent <strong>of</strong> temperature. However, positive values were observed on<br />
contaminated surfaces. In a later series <strong>of</strong> papers Greaves and Linnett (7) studied<br />
a number <strong>of</strong> oxide surfaces, in all cases the recombination coefficient was temperature<br />
'<br />
dependent. For silica apparent activation energies were 1 to 13 Kcal/mol over the<br />
temperature range 15 to 3OOOC. The exceptional nature <strong>of</strong> Pyrex was noted.<br />
' The second major source <strong>of</strong> loss <strong>of</strong> active species results from electron-ion<br />
recombination at the chamber walls. The electric field restricts the drift <strong>of</strong> ions<br />
to the chamber walls. Rate <strong>of</strong>-recombination is controlled by ambipolar diffusion,<br />
but is limited by the presence <strong>of</strong> negatively charged oqgen ions in the discharge (15).<br />
Although diffusion is not dependent on wall temperature, a distortion <strong>of</strong> the<br />
symmetric electrical field will enhance wall recombination, producing an inarease in<br />
This effect is noted in t&le 1.<br />
The presence <strong>of</strong> a 6-cm long metallic ring on the exterior wall <strong>of</strong> the<br />
reduced oddation rate by more than ten per cent. Grounding the ring in comn with<br />
. wall temperature and a reduction <strong>of</strong> oxidation rate.<br />
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