Wayne
Nov24-04, 09:26 AM
<jabberwocky><div class="vbmenu_control"><a href="jabberwocky:;" onClick="newWindow=window.open('','usenetCode','toolbar=no, location=no,scrollbars=yes,resizable=yes,status=no ,width=650,height=400'); newWindow.document.write('<HTML><HEAD><TITLE>Usenet ASCII</TITLE></HEAD><BODY topmargin=0 leftmargin=0 BGCOLOR=#F1F1F1><table border=0 width=625><td bgcolor=midnightblue><font color=#F1F1F1>This Usenet message\'s original ASCII form: </font></td></tr><tr><td width=449><br><br><font face=courier><UL><PRE>\n\nHi\n\nI am working on explaining the net effect of an AC bias on two copper\nelectrode (low freq.)\n\nUnder an AC voltage, the mobile ions merely oscillate back and forth\nresulting in no net flow. However, the process may produce a REDOX reaction\nthat may not be reversible. The result is that the reverse action can not\ntake place. Although each half cycle that is favourable for the reaction\nwill still accelerate the reaction.\n\nFor example one of the electrodes will start to reduce producing a gas and\nthe other will oxidise, forming say oxides that in most cases have a high\nSIR value. When the bias reverses the OX electrode will now try and reduce\nand the previous RED electrode will try and oxides. This will eventually\nincrease the SIR and reduce the flow of ions.\n\nI have seemingly contradicted myself and can not find my way out. Whilst I\nagree with my first paragraph I have evidence of the second, can anyone\nshine any light onto this?\n\n\n\nCheers\n\n\n\nWayne\n\n\n\n</UL></PRE></font></td></tr></table></BODY><HTML>');"> <IMG SRC=/images/buttons/ip.gif BORDER=0 ALIGN=CENTER ALT="View this Usenet post in original ASCII form"> View this Usenet post in original ASCII form </a></div><P></jabberwocky>Hi
I am working on explaining the net effect of an AC bias on two copper
electrode (low freq.)
Under an AC voltage, the mobile ions merely oscillate back and forth
resulting in no net flow. However, the process may produce a REDOX reaction
that may not be reversible. The result is that the reverse action can not
take place. Although each half cycle that is favourable for the reaction
will still accelerate the reaction.
For example one of the electrodes will start to reduce producing a gas and
the other will oxidise, forming say oxides that in most cases have a high
SIR value. When the bias reverses the OX electrode will now try and reduce
and the previous RED electrode will try and oxides. This will eventually
increase the SIR and reduce the flow of ions.
I have seemingly contradicted myself and can not find my way out. Whilst I
agree with my first paragraph I have evidence of the second, can anyone
shine any light onto this?
Cheers
Wayne
I am working on explaining the net effect of an AC bias on two copper
electrode (low freq.)
Under an AC voltage, the mobile ions merely oscillate back and forth
resulting in no net flow. However, the process may produce a REDOX reaction
that may not be reversible. The result is that the reverse action can not
take place. Although each half cycle that is favourable for the reaction
will still accelerate the reaction.
For example one of the electrodes will start to reduce producing a gas and
the other will oxidise, forming say oxides that in most cases have a high
SIR value. When the bias reverses the OX electrode will now try and reduce
and the previous RED electrode will try and oxides. This will eventually
increase the SIR and reduce the flow of ions.
I have seemingly contradicted myself and can not find my way out. Whilst I
agree with my first paragraph I have evidence of the second, can anyone
shine any light onto this?
Cheers
Wayne