0
Which would be the anode in a magnesium and zinc galvanic cell?
Wiki User
∙ 11y ago
Mg(s) Epi-Boii
Wiki User
∙ 10y ago
Wiki User
∙ 12y agoZn(s)
Anonymous
Anonymous
Jesus H
Wiki User
∙ 11y agoZn(s)
Arush Jain
Wiki User
∙ 10y agoit is definitely Mg(s)
Anonymous
Mg(s)
Leith Davidson
Add your answer:
Earn +20 pts
What is oxidized in a galvanic cell?
The anode
What is the standard cell notation of a galvanic cell made with magnesium and gold?
Zn(s)/Zn2+(aq)//Au+(aq)/Au(s)
What is another name for galvanic cell?
The voltaic cell
What is the negative electrode of a voltaic cell called?
This is the anode.
What is galvanic cell made of?
Two electrodes in electrolyte solutions
Which electrode in the anode is galvanic cell?
Zinc is the anode.
What is a Anode?
The electrode that is oxidized in a galvanic cell ~
Why is use of a sacrificial anode considered to be a way to prevent corrosion?
The anode creates a galvanic cell in which magnesium or zinc will be corroded more quickly than the metal of, let's sa a tank.
Which is the electrode is the anode in a galvanic cell?
The electrode with the highest oxidation potential
What would be the cathode in a magnesium and zinc galvanic cell?
In a galvanic cell, the less reactive metal is the cathode, where oxidation takes place. In this case the cathode is zinc.
What happens to the mass of the metal anode as the cell continues to operate?
It depends on the specifics of the cell, but in most simple galvanic cells, the anode slowly dissolves into solution.
Electrons in a galvanic cell normally flow?
A galvanic cell is a spontaneous reaction so electron flow will occur as long as a salt bridge is present.
What is the voltage of galvanic cell made with magnesium and gold?
4.2 V
What is the cathode of a galvanic cell made with magnesium and gold?
the gold electrode
What is the voltage of a galvanic cell made with magnesium and gold?
4.2 V
What is the voltage of galvanic cell made with magnesium (Mg) and gold (Au)?
4.2V
Would a galvanic cell work without a salt bridge?
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.
