chemical physics of discharges - Argonne National Laboratory
chemical physics of discharges - Argonne National Laboratory chemical physics of discharges - Argonne National Laboratory
212 the principal axis 43 cm from the gas inlet. A 0.6-cm tube, C, passed diametrically through the cylinder and held the spechen on a central projection. Sample temperature was regulated, in part, by circulating liquids between this tube and a constant temperature bath. Radiofrequency excitation was supplied from a 250-watt, crystal controlled 13.56-MHz generator, described previously (3). Except as otherwise noted, an output of 115 watts was employed. Power was transferred to the gas by means of impedance matching network terminating in a lo-turn coil of $-inch O.D. copper tubing tapped 2 turns from ground. The coil, B, which had an inside diameter of 4.5 cm and was 12.5 cm long, was coaxial with the reaction tube and placed 10 hm from the gas inlet. After passage through a rotometer, molecular gas entered the reaction system through a capillary orifice, A. Pressure was monitored by a McCloud gauge attached to side ann E, located 50 cm beyond the gas inlet. Pressure was maintained at 1.2 torr; and flow rates at 150 cc per minute, S.T.P. U.S.P. grade oxygen and instrument grade carbon dioxide were used. The temperature of solid specimens in the plasma was determined by means of an infrared radiation thermometer (Infrascope Model 3-lC00, Huggins Laboratories Inc., Sunnyvale, Calif.) attached to a chart recorder. This device employs a lead sulfide detector and suitable filters to permit remote measurement of 1.2 to 2.5~ radiation emitted by the specimen. To compensate for variations in emissitivity and inhomogeneity in the optical field, empirical calibration curves were constructed. Themcouples were employed to determine cylinder-wall temperatures. To eliminate interaction with the radiofrequency field, the transmitter was inactivated during the latter measurements. High purity graphite rods (National Carbon Co., Grade AGKSP) were employed as standard specimens. These rods were 0.61 cm in diameter and had a cavity machined into their base to affix them to the cooling tube. Pellets of sucrose and carbon containing small quantities of cupric acetate were also epployed. The latter were produced by heating and then pressing a slurry of the salt solution and m-mesh graphite powder. Results and Discussion Sample Temerature: The temperature variation of oxidation rate of graphite exposed to the oxygen plasma is shown in figure 2. Over tpe range 120 to 300OC, the Arrhenius equation, X = Ce'Ea/RT, fits the data well and yields a value of 6.5 Kcal/mol for the apparent activation energy, Ea. Between 300 and 450°C, the highest temerature studied, oxidation rate is not dependent on temperature. The oxidation of graphite by molecular oxygen at high tempgrature is strongly dependent on the purity of the graphite. To determine if a similar effecb occurs in plasma oddation, pellets composed of pure graphite powder and inorganic salts were utilized. The results of the addition of 0.01 _M cupric acetate are shown in figure 2. At low temperature the change in oxidation rate of pure and impure graphite with temperature is similar. However, the rate of oxidation of the impure graphite becomes independent of taprature at a lower temperature. Measurements performed with specimens contabhg 1-r , concentrations of cupric acetate led to results which fell between the illustrated curves. The gas in the law pressure electrodeless discharge is chemically similar to that k in the positive column of a low pressure arc. Wlecule-molecule and ion-molecule collisions are frequent. The ions and neutral species are, therefore, nearly in ther- 1 mal quildbrium. Elastic collisions between these species and electrons are less ' frequent. At low pressure electron temperatures are quite high. In the oxygen die- Charge atodc oxygen (%) is believed to be the most abundant active species. Higher energy states of atomic oxygen, positive and negative ions, and electronically 1 ,,
2 E, W t- a Z 9 I- a 2 X 0 I50 too 50 30 20 A A A A 1 K SOURCE ~ ~~ ~ Fig. 1. Experimental apparatus : capillary inlet, A; power coil, B; specimen mounting tube, C; sidearm to manometer, D; outlet to vacuum pump, E. 1 IO 1.5 2-0 2.5 SURFACE TEMPERATURE )/r x Fig. 2. Rate of oxidation vs. surface temperature for graphite rods,@, and graphite pellets containing 0.01 ,M cupric acetate,A. I
- Page 161 and 162: I 161 THE GLOW DISCHARGE DEPOSITION
- Page 163 and 164: Fig. 1 Process Apparatus -__l.ll__
- Page 165 and 166: v) t- at- InIo Io0 t-Q) loo lcua O
- Page 167 and 168: This study is only an approximation
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- Page 171 and 172: \ i (4) Effect of System Pressure T
- Page 173 and 174: 173 Pressure. Since pressure is a c
- Page 175 and 176: 175 Table VI X-RAY DATA OF DEPOSIT
- Page 177 and 178: 177 Another source of weakness is t
- Page 179 and 180: 179 PLATING IN A CORONA DISCHARGE R
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- Page 189 and 190: I (b) Polarized Light Fig. 6 Cross
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- Page 199 and 200: 199 a red heat in this cell using d
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- Page 205 and 206: BELL JAR STANC TO VACUUM SYSTEM U T
- Page 207 and 208: 207 of the boron oxide film, the fi
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- Page 217 and 218: I- z W 0 w a a 100 80 60 40 20 215
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- Page 233 and 234: - 233 SOME PROBLEMS OF THE KINETICS
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- Page 237 and 238: 237 Table 2 Experimental Variables
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- Page 241 and 242: 241 Discussion The systematic varia
- Page 243 and 244: I \ 1 243 FORMATION OF HYDROCARBONS
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212<br />
the principal axis 43 cm from the gas inlet. A 0.6-cm tube, C, passed diametrically<br />
through the cylinder and held the spechen on a central projection. Sample temperature<br />
was regulated, in part, by circulating liquids between this tube and a constant<br />
temperature bath. Radi<strong>of</strong>requency excitation was supplied from a 250-watt, crystal<br />
controlled 13.56-MHz generator, described previously (3). Except as otherwise noted,<br />
an output <strong>of</strong> 115 watts was employed. Power was transferred to the gas by means <strong>of</strong><br />
impedance matching network terminating in a lo-turn coil <strong>of</strong> $-inch O.D. copper tubing<br />
tapped 2 turns from ground.<br />
The coil, B, which had an inside diameter <strong>of</strong> 4.5 cm and<br />
was 12.5 cm long, was coaxial with the reaction tube and placed 10 hm from the gas<br />
inlet.<br />
After passage through a rotometer, molecular gas entered the reaction system<br />
through a capillary orifice, A. Pressure was monitored by a McCloud gauge attached<br />
to side ann E, located 50 cm beyond the gas inlet. Pressure was maintained at 1.2<br />
torr; and flow rates at 150 cc per minute, S.T.P. U.S.P. grade oxygen and instrument<br />
grade carbon dioxide were used.<br />
The temperature <strong>of</strong> solid specimens in the plasma was determined by means <strong>of</strong> an<br />
infrared radiation thermometer (Infrascope Model 3-lC00, Huggins Laboratories Inc.,<br />
Sunnyvale, Calif.) attached to a chart recorder. This device employs a lead sulfide<br />
detector and suitable filters to permit remote measurement <strong>of</strong> 1.2 to 2.5~ radiation<br />
emitted by the specimen. To compensate for variations in emissitivity and inhomogeneity<br />
in the optical field, empirical calibration curves were constructed.<br />
Themcouples were employed to determine cylinder-wall temperatures. To eliminate<br />
interaction with the radi<strong>of</strong>requency field, the transmitter was inactivated during<br />
the latter measurements.<br />
High purity graphite rods (<strong>National</strong> Carbon Co., Grade AGKSP) were employed as<br />
standard specimens. These rods were 0.61 cm in diameter and had a cavity machined<br />
into their base to affix them to the cooling tube. Pellets <strong>of</strong> sucrose and carbon<br />
containing small quantities <strong>of</strong> cupric acetate were also epployed. The latter were<br />
produced by heating and then pressing a slurry <strong>of</strong> the salt solution and m-mesh<br />
graphite powder.<br />
Results and Discussion<br />
Sample Temerature: The temperature variation <strong>of</strong> oxidation rate <strong>of</strong> graphite<br />
exposed to the oxygen plasma is shown in figure 2. Over tpe range 120 to 300OC, the<br />
Arrhenius equation, X = Ce'Ea/RT, fits the data well and yields a value <strong>of</strong> 6.5<br />
Kcal/mol for the apparent activation energy, Ea. Between 300 and 450°C, the highest<br />
temerature studied, oxidation rate is not dependent on temperature. The oxidation<br />
<strong>of</strong> graphite by molecular oxygen at high tempgrature is strongly dependent on the purity<br />
<strong>of</strong> the graphite. To determine if a similar effecb occurs in plasma oddation, pellets<br />
composed <strong>of</strong> pure graphite powder and inorganic salts were utilized. The results <strong>of</strong><br />
the addition <strong>of</strong> 0.01 _M cupric acetate are shown in figure 2. At low temperature the<br />
change in oxidation rate <strong>of</strong> pure and impure graphite with temperature is similar.<br />
However, the rate <strong>of</strong> oxidation <strong>of</strong> the impure graphite becomes independent <strong>of</strong> taprature<br />
at a lower temperature. Measurements performed with specimens contabhg 1-r ,<br />
concentrations <strong>of</strong> cupric acetate led to results which fell between the illustrated<br />
curves.<br />
The gas in the law pressure electrodeless discharge is <strong>chemical</strong>ly similar to that k<br />
in the positive column <strong>of</strong> a low pressure arc. Wlecule-molecule and ion-molecule<br />
collisions are frequent. The ions and neutral species are, therefore, nearly in ther- 1<br />
mal quildbrium.<br />
Elastic collisions between these species and electrons are less<br />
' frequent. At low pressure electron temperatures are quite high. In the oxygen die-<br />
Charge atodc oxygen (%) is believed to be the most abundant active species. Higher<br />
energy states <strong>of</strong> atomic oxygen, positive and negative ions, and electronically<br />
1<br />
,,