| Analysis of the search query | which electrode does oxidation take place in electrolysis |
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Top competitors on query "which electrode does oxidation take place in electrolysis"
Batteries: The Absolute Definitive Guide
http://gizmodo.com/5952938/everything-you-need-to-know-about-batteries Competition: low
Essentially, the anode of a rechargeable Li-ion are made from many millions of microscopically thin sheets of carbon graphite, stacked atop one another. LCO's lose just 5-10 percent of their charge per month, compared to more than 30 percent a month for NiMH cells and 10 percent a month for NiCd batteries
http://www.docbrown.info/page07/redox3.htm Competition: low
A mixture of the amine and water 'steam distils' into the condenser and separates into two layers in the collection flask which can then be further processed using a separating funnel. The diagram shows a bunsen burner being used to supply the heat ('my days'), these days its more likely, and safer, to use an electrical heater that the round bottomed flask fits in snugly
No-Rosion Products Technical Questions and Answers
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Our Coolant Test Packet is a quick, easy, cost-effective way of determining whether the product has been dosed properly, or whether the inhibitors have been depleted from coolant. And importantly, it enhances the overall performance of No-Rosion, allowing it to more effectively function and provide the full range of benefits that it has been engineered to provide
Separate Hydrogen and Oxygen from Water Through Electrolysis : Electrolysis of Water - An Explanation
http://www.instructables.com/id/Separate-Hydrogen-and-Oxygen-from-Water-Through-El/step1/Electrolysis-of-Water-An-Explanation/ Competition: low
(In this case the hydrogen gains electrons and the oxygen loses them) In doing so these ions balance their charges, and become real, electrically balanced, bona fide atoms (or in the case of the hydrogen, a molecule).The reason this system isn't very efficient is because some of the electrical energy is converted into heat during the process. It is used in various industrial applications such as...1Step 1: Electrolysis of Water - An Explanation This section is an explanation of the electrolysis of water, feel free to skip it if you don't find it interesting
http://metaldetectingworld.com/cleaning_coin_p15_electrolysis.shtml Competition: low
If this reaction does not take place, it is probably because you were unsure of the output wire polarity, there is no contact between the coin and cathode - the electric circuit is not complete, or your converter is simply not functioning. Electrochemical Reduction - GALVANIC CLEANING Reduction is the decomposition of oxidation on the coin surfaces by separation of the oxygen, chlorine, sulfur, etc., from the compounds of oxygen, chlorine, sulfur, etc
oxidation-reduction reaction (chemical reaction) -- Encyclopedia Britannica
http://www.britannica.com/EBchecked/topic/436636/oxidation-reduction-reaction Competition: low
By the end of the century, his ideas were widely accepted and had been successfully applied to the more complex processes of respiration and photosynthesis. You can make it easier for us to review and, hopefully, publish your contribution by keeping a few points in mind: Encyclopaedia Britannica articles are written in a neutral, objective tone for a general audience
Electrolysis Cleaning Method
http://users.eastlink.ca/~pspencer/nsaeta/electrolysis.html Competition: low
Of course my main question is why have a machine to make Sodium Hydroxide when we (at least in North America) can easily buy large bags of pure Sodium Hydroxide for not a lot of money? You could make 100's of litres of a cleaning solution with that. It is not enough to produce a Hindenburg-like explosion in your workshop, but it is flammable all the same so this should be done in a reasonably ventilated area and caution is advised
SparkNotes: SAT Chemistry: Redox and Electrochemistry
http://www.sparknotes.com/testprep/books/sat2/chemistry/chapter6section7.rhtml Competition: low
Example Which one of the following would be the best oxidizing agent: Ba, Na, Cl, F, or Br? Explanation Using the reduction potential chart and the fact that oxidizing agents are the elements that are most easily reduced, we determine fluorine is the best oxidizing agent. The equation for the reaction is Zn(s) + I2(s)ZnI2(s) + energy Identify the elements that are oxidized and reduced, and determine the oxidizing and reducing agents
http://www.amazon.com/Clean-Easy-Deluxe-Home-Electrolysis/dp/B002QXLM3I Competition: low
Read more Published 5 days ago by InkedAngel 3.0 out of 5 stars Stylet Tips Now Too Short I thought I had found the perfect solution for permanent hair removal at home. To join, select "Yes, I want FREE Two-Day Shipping with Amazon Prime" above the Add to Cart button and confirm your Amazon Prime free trial sign-up during checkout
Yahoo! Answers - Electrolytic cell and voltaic cell question? 10 points?
http://malaysia.answers.yahoo.com/question/index?qid=20110501112326AAIHOgS Competition: low
OILRIG In a voltaic cells, electrons are produced as an element is oxidized (oxidation is loss), and move to where they are used in the reduction of an other element (reduction is gain). In an electrolytic cell, a potential difference (voltage) is applied from an outside source and electrons move toward where they are used in the reduction of an element (reduction is gain)
http://www.shodor.org/UNChem/advanced/redox/ Competition: low
We again change the sign since we're actually reversing the Fe reaction Using the calculator again, we calculate the nonstandard potential of the Cd reaction. The oxidation number of a compound has some analogy to the pH and pK measurements found in acids and bases -- the oxidation number suggests the strength or tendency of the compound to be oxidized or reduced, to serve as an oxidizing agent or reducing agent
http://www.science.uwaterloo.ca/~cchieh/cact/c123/eltlysis.html Competition: low
How many Faradays and how many Coulombs passed through the cell? What is the current? Solution Using the same method as indicated above, you have 1 mol 2 F 3.175 g Cu ------- -------- (At.wt. The following discussion provides an introductory guide regarding electrolysis, which is also used to produce and refine metals for industries, making jewelries, protecting metal from corrosions and more
http://www.docbrown.info/page04/Mextractb.htm Competition: low
The extraction of aluminium and sodium by electrolysis How do we extract reactive metals that cannot be obtained using carbon? Why do we need to use electrolysis to obtain certain metals from their ores? e.g. What does the complete electrical circuit consist of? There are two ion currents in the electrolyte flowing in opposite directions: positive cations e.g
http://www.shodor.org/UNChem/glossary.html Competition: low
The equilibrium expression is equal to the concentration of each product raised to its coefficient in a balanced chemical equation and multiplied together, divided by the concentration of the product of reactants to the power of their coefficients. ionic bonds When two oppositely charged atoms share at least one pair of electrons but the electrons spend more time near one of the atoms than the other
http://www.ucidiver.com/electrolysis.html Competition: low
Rust has a tendency to pit and scar the surface of the metal item recovered and the longer the rust is allowed to stay on the item, the more damage it does. Safety Precautions Before we begin, you must first understand that electrolysis can be dangerous if you are not careful and take some safety precautions like: Always wear eye protection and gloves because the cleaning solution we submerged the rusted item in is alkaline and will irritate the skin and your eyes
http://dictionary.reference.com/browse/electrolysis?s=t Competition: low
the passage of an electric current through an electrolyte with subsequent migration of positively and negatively charged ions to the negative and positive electrodes
Experiments in Electrochemistry
http://www.funsci.com/fun3_en/electro/electro.htm Competition: low
You have learned to measure potentials of reduction of various materials and to predict the voltage generated by a battery when you know it's material components. Since we can build a functioning version with other types of electrolytes, in this experiment we will use a more benign substance, like those specified in the materials list - a solution of copper sulfate, for example
CR Scientific: Electrolysis Experiments - Introduction
http://www.crscientific.com/electrolysis.html Competition: low
Electrolysis of Water To accomplish this, one must make the water conductive by using an electrolyte that does not react under the conditions of the experiment. Electrolysis can force many chemical reactions to go against their "normal" (spontaneous) direction; this will occur when a certain electric potential (i.e., applied voltage) is reached
What is an Electrode? (with picture)
http://www.wisegeek.org/what-is-an-electrode.htm Competition: low
For reasons that are historical rather than scientific, electricity in a circuit is, by convention, depicted as traveling from positive to negative, so that it is seen as a flow of positive charge out from the cathode, and into the anode. An electrical current, however, consists of a flow of tiny negatively charged particles called electrons, so this flow is actually in the opposite direction
Electrolytic Cells - ChemWiki
http://chemwiki.ucdavis.edu/Analytical_Chemistry/Electrochemistry/Electrolytic_Cells Competition: low
The direction of electron flow in electrolytic cells, however, may be reversed from the direction of spontaneous electron flow in galvanic cells, but the definition of both cathode and anode remain the same, where reduction takes place at the cathode and oxidation occurs at the anode. If a solution of sodium chloride (containing water) was used in the above system, hydrogen would undergo reduction instead of sodium, because it is a stronger reducing agent that sodium
http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/electrode.html Competition: low
Note that the cell potential is equal to the standard value if the concentrations are equal even if they are not equal to the standard value of 1M, since the logarithm gives the value zero. Two main hurdles must be overcome to establish such a tabulation The electrode potential cannot be determined in isolation, but in a reaction with some other electrode
Reactions at Electrodes during Electrolysis? - Yahoo! Answers
http://answers.yahoo.com/question/index?qid=20071130221016AAcTM06 Competition: low
If anyone could provide an explanation that would be awesome! Your help is greatly appreciated!!! 6 years ago Report Abuse by Guray T Member since: October 26, 2007 Total points: 16,029 (Level 6) Add Contact Block Best Answer - Chosen by Asker First of all I must say that your questions are not easy and I will start to clarify your trouble first
Electrolysis - Wikipedia, the free encyclopedia
http://en.wikipedia.org/wiki/Electrolysis Competition: low
Reduced species (often an anion) with a more positive cell potential are more difficult to oxidize than reduced species with a more negative cell potential. These factors together mean that a higher potential is required for the reduction and oxidation of water than predicted, and these are termed overpotentials
Electrochemistry - Wikipedia, the free encyclopedia
http://en.wikipedia.org/wiki/Electrochemistry Competition: low
If a chemical reaction is driven by an externally applied voltage, as in electrolysis, or if a voltage is created by a chemical reaction as in a battery, it is an electrochemical reaction. The action potentials that travel down neurons are based on electric current generated by the movement of sodium and potassium ions into and out of cells
Electrochemistry Dictionary and Encyclopedia
http://electrochem.cwru.edu/ed/dict.htm Competition: low
diffusion control An electrode reaction is considered to be under "diffusion control" when the overall rate of the reaction is is controlled by the rate of the diffusion of the reactants to the electrode surface rather than the rate of the reaction itself or the ir drop in the solution. bus(bar) A typically not insulated (not covered with insulation) conductor used to carry a large current or to make a common connection between several circuits
Batteries: The Absolute Definitive Guide
Essentially, the anode of a rechargeable Li-ion are made from many millions of microscopically thin sheets of carbon graphite, stacked atop one another. LCO's lose just 5-10 percent of their charge per month, compared to more than 30 percent a month for NiMH cells and 10 percent a month for NiCd batteries
A mixture of the amine and water 'steam distils' into the condenser and separates into two layers in the collection flask which can then be further processed using a separating funnel. The diagram shows a bunsen burner being used to supply the heat ('my days'), these days its more likely, and safer, to use an electrical heater that the round bottomed flask fits in snugly
No-Rosion Products Technical Questions and Answers
Our Coolant Test Packet is a quick, easy, cost-effective way of determining whether the product has been dosed properly, or whether the inhibitors have been depleted from coolant. And importantly, it enhances the overall performance of No-Rosion, allowing it to more effectively function and provide the full range of benefits that it has been engineered to provide
Separate Hydrogen and Oxygen from Water Through Electrolysis : Electrolysis of Water - An Explanation
(In this case the hydrogen gains electrons and the oxygen loses them) In doing so these ions balance their charges, and become real, electrically balanced, bona fide atoms (or in the case of the hydrogen, a molecule).The reason this system isn't very efficient is because some of the electrical energy is converted into heat during the process. It is used in various industrial applications such as...1Step 1: Electrolysis of Water - An Explanation This section is an explanation of the electrolysis of water, feel free to skip it if you don't find it interesting
If this reaction does not take place, it is probably because you were unsure of the output wire polarity, there is no contact between the coin and cathode - the electric circuit is not complete, or your converter is simply not functioning. Electrochemical Reduction - GALVANIC CLEANING Reduction is the decomposition of oxidation on the coin surfaces by separation of the oxygen, chlorine, sulfur, etc., from the compounds of oxygen, chlorine, sulfur, etc
oxidation-reduction reaction (chemical reaction) -- Encyclopedia Britannica
By the end of the century, his ideas were widely accepted and had been successfully applied to the more complex processes of respiration and photosynthesis. You can make it easier for us to review and, hopefully, publish your contribution by keeping a few points in mind: Encyclopaedia Britannica articles are written in a neutral, objective tone for a general audience
Electrolysis Cleaning Method
Of course my main question is why have a machine to make Sodium Hydroxide when we (at least in North America) can easily buy large bags of pure Sodium Hydroxide for not a lot of money? You could make 100's of litres of a cleaning solution with that. It is not enough to produce a Hindenburg-like explosion in your workshop, but it is flammable all the same so this should be done in a reasonably ventilated area and caution is advised
SparkNotes: SAT Chemistry: Redox and Electrochemistry
Example Which one of the following would be the best oxidizing agent: Ba, Na, Cl, F, or Br? Explanation Using the reduction potential chart and the fact that oxidizing agents are the elements that are most easily reduced, we determine fluorine is the best oxidizing agent. The equation for the reaction is Zn(s) + I2(s)ZnI2(s) + energy Identify the elements that are oxidized and reduced, and determine the oxidizing and reducing agents
http://www.amazon.com/Clean-Easy-Deluxe-Home-Electrolysis/dp/B002QXLM3I Competition: lowRead more Published 5 days ago by InkedAngel 3.0 out of 5 stars Stylet Tips Now Too Short I thought I had found the perfect solution for permanent hair removal at home. To join, select "Yes, I want FREE Two-Day Shipping with Amazon Prime" above the Add to Cart button and confirm your Amazon Prime free trial sign-up during checkout
Yahoo! Answers - Electrolytic cell and voltaic cell question? 10 points?
OILRIG In a voltaic cells, electrons are produced as an element is oxidized (oxidation is loss), and move to where they are used in the reduction of an other element (reduction is gain). In an electrolytic cell, a potential difference (voltage) is applied from an outside source and electrons move toward where they are used in the reduction of an element (reduction is gain)
We again change the sign since we're actually reversing the Fe reaction Using the calculator again, we calculate the nonstandard potential of the Cd reaction. The oxidation number of a compound has some analogy to the pH and pK measurements found in acids and bases -- the oxidation number suggests the strength or tendency of the compound to be oxidized or reduced, to serve as an oxidizing agent or reducing agent
How many Faradays and how many Coulombs passed through the cell? What is the current? Solution Using the same method as indicated above, you have 1 mol 2 F 3.175 g Cu ------- -------- (At.wt. The following discussion provides an introductory guide regarding electrolysis, which is also used to produce and refine metals for industries, making jewelries, protecting metal from corrosions and more
The extraction of aluminium and sodium by electrolysis How do we extract reactive metals that cannot be obtained using carbon? Why do we need to use electrolysis to obtain certain metals from their ores? e.g. What does the complete electrical circuit consist of? There are two ion currents in the electrolyte flowing in opposite directions: positive cations e.g
The equilibrium expression is equal to the concentration of each product raised to its coefficient in a balanced chemical equation and multiplied together, divided by the concentration of the product of reactants to the power of their coefficients. ionic bonds When two oppositely charged atoms share at least one pair of electrons but the electrons spend more time near one of the atoms than the other
Rust has a tendency to pit and scar the surface of the metal item recovered and the longer the rust is allowed to stay on the item, the more damage it does. Safety Precautions Before we begin, you must first understand that electrolysis can be dangerous if you are not careful and take some safety precautions like: Always wear eye protection and gloves because the cleaning solution we submerged the rusted item in is alkaline and will irritate the skin and your eyes
the passage of an electric current through an electrolyte with subsequent migration of positively and negatively charged ions to the negative and positive electrodes
Experiments in Electrochemistry
You have learned to measure potentials of reduction of various materials and to predict the voltage generated by a battery when you know it's material components. Since we can build a functioning version with other types of electrolytes, in this experiment we will use a more benign substance, like those specified in the materials list - a solution of copper sulfate, for example
CR Scientific: Electrolysis Experiments - Introduction
Electrolysis of Water To accomplish this, one must make the water conductive by using an electrolyte that does not react under the conditions of the experiment. Electrolysis can force many chemical reactions to go against their "normal" (spontaneous) direction; this will occur when a certain electric potential (i.e., applied voltage) is reached
What is an Electrode? (with picture)
For reasons that are historical rather than scientific, electricity in a circuit is, by convention, depicted as traveling from positive to negative, so that it is seen as a flow of positive charge out from the cathode, and into the anode. An electrical current, however, consists of a flow of tiny negatively charged particles called electrons, so this flow is actually in the opposite direction
Electrolytic Cells - ChemWiki
The direction of electron flow in electrolytic cells, however, may be reversed from the direction of spontaneous electron flow in galvanic cells, but the definition of both cathode and anode remain the same, where reduction takes place at the cathode and oxidation occurs at the anode. If a solution of sodium chloride (containing water) was used in the above system, hydrogen would undergo reduction instead of sodium, because it is a stronger reducing agent that sodium
Note that the cell potential is equal to the standard value if the concentrations are equal even if they are not equal to the standard value of 1M, since the logarithm gives the value zero. Two main hurdles must be overcome to establish such a tabulation The electrode potential cannot be determined in isolation, but in a reaction with some other electrode
Reactions at Electrodes during Electrolysis? - Yahoo! Answers
If anyone could provide an explanation that would be awesome! Your help is greatly appreciated!!! 6 years ago Report Abuse by Guray T Member since: October 26, 2007 Total points: 16,029 (Level 6) Add Contact Block Best Answer - Chosen by Asker First of all I must say that your questions are not easy and I will start to clarify your trouble first
Electrolysis - Wikipedia, the free encyclopedia
Reduced species (often an anion) with a more positive cell potential are more difficult to oxidize than reduced species with a more negative cell potential. These factors together mean that a higher potential is required for the reduction and oxidation of water than predicted, and these are termed overpotentials
Electrochemistry - Wikipedia, the free encyclopedia
If a chemical reaction is driven by an externally applied voltage, as in electrolysis, or if a voltage is created by a chemical reaction as in a battery, it is an electrochemical reaction. The action potentials that travel down neurons are based on electric current generated by the movement of sodium and potassium ions into and out of cells
Electrochemistry Dictionary and Encyclopedia
diffusion control An electrode reaction is considered to be under "diffusion control" when the overall rate of the reaction is is controlled by the rate of the diffusion of the reactants to the electrode surface rather than the rate of the reaction itself or the ir drop in the solution. bus(bar) A typically not insulated (not covered with insulation) conductor used to carry a large current or to make a common connection between several circuits
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