Anode(:
Anode
The correct answer is Electrons flow away from the anode and also Oxidation occurs at the anode.
In a galvanic cell, the less reactive metal is the cathode, where oxidation takes place. In this case the cathode is zinc.
A: at the anode in both an electrolytic cell and a voltaic cell
Anode - the electrode at which oxidation occurs. Cathode - the electrode at which reduction occurs. Electrolytes - containing the ions involved in the redox reaction.
The electrolyte of a commercial galvanic cell normally extends from anode to cathode without interruption by a salt bridge. A salt bridge is normally a teaching tool to help show that: 1. Galvanic half-cells do not produce voltage 2. Conductors and insulators are not necessarily salt bridges. An electrolyte must extend from anode to cathode before the galvanic cell can produce voltage. 3. The chemical composition of the salt bridge can differ from the electrolytes in the half cells. 4. Ions travel through the salt bridge between the cell's anode and cathode. Salt bridges raise more questions than answers. For example: 1. Can the difference between an electrolyte and a conductor be defined? 2. How do ions quickly move through a solid or a long electrolyte? 3. When salt bridge composition differs from the galvanic cell electrolyte(s), must the salt bridge chemically react with the galvanic cell electrolyte(s)? 4. Why does galvanic cell voltage remain nearly constant while anode to cathode distance doubles.
This is the anode.
The Cathode is the negative electrode; the anode is the positive electrode
Electron flow is from anode (+) to cathode (-)
Cathode
Oxidation occurs at the anode ("an ox") and reduction occurs at the cathode ("red cat").See the Web Link to the left for the specific reaction in a dry cell.
An anolyte is the portion of an electrolyte near an anode, especially in a cell in which the cathode and anode are in separate compartments.
The correct answer is Electrons flow away from the anode and also Oxidation occurs at the anode.
Anode ,cathode ,pef
It can be complicated depending on the type of cell one is looking at. However, here is my simple explanation.The anode is the electrode where the oxidation reaction takes place, and oxidation is the loss of electrons, so in a galvanic cell the anode is a source of free electrons and so it is negatively charged.The cathode is the electrode where reduction takes place, and reduction is the gain of electrons, so in a galvanic cell the cathode is positively charge and ready to accept negatively charged electrons.Now, the anode isn't always negative and the cathode isn't always positive. It has to do with the direction of current flow (anode = current in, cathode = current out). In an electrolytic cell, the charges on the anode and the cathode are reversed from that seen in a galvanic cell.
Anode is positive and cathode is negative. Cathode is the longest led frame. Anode is where the oxidation reaction takes place while cathode is where the reduction reaction takes place or in a galvanic corrosion the anode is the metal that corrodes while the cathode is protected.
Anode is positive electrode which attracts the negative anions while cathode is the negative electrode which attracts the positive cations during electrolysis.
Anode is the positive electrode while cathode is the negative electrode. Negative ions(anions) travel towards the anode(hence the name) Positive ions(cations) travel towards the cathode(hence the name) Example for anode:Copper Example for cathode:Zinc