Sacrificial anode Essays

the metallic phase (the electrode) or aqueous phase (the electrolyte). (Lower 2004) These reactions involve the transfer of electric charges between the electrodes and the electrolyte. These cells have two electrodes which are named the anode and the cathode. The anode is the electrode where oxidation occurs and the cathode is the electrode where reduction occurs (Electrochemical cells 2014). Oxidation always occurs simultaneously to reduction and the process of this electron transfer is named a redox

Electrolytes are minerals found in liquids that carry either a negative or positive charge. This allows them to conduct electricity and move electrical currents throughout its mass. (Morris) “[Electrolytes allow cells to] generate energy, maintain the stability of their walls, and to function in general.” (Wedro) Heart, muscle, and nerve cells use electrolytes to maintain and carry the electrical current/impulses across their membranes. (Nordqvist) They also regulate muscles and nerves, allow fluids

In the zinc electrolytic cell it was a oxidation reaction losing electrons in the equation Zn(s)--> Zn(aq)^2+2e^- For copper in it;s cathode there is the reduction reaction Cu(aq)^2+ + 2e^--> Cu(s) The flow of electrons will move from zinc ( anode electrolytic cell) to copper (cathode electrolytic cell). The overall reaction looks like

Batteries have been around for a very long time. It is thought that the very first type of battery may have been made by the Parthians around 250 B.C. They lived in Baghdad and made a clay jar with vinegar and a copper cylinder inside with a iron rod sticking out. Batteries have definitely changed since then. In the 1800 an Italian physicist Alessandro Volta invented the voltaic pile, which was made of zinc and copper plates with vinegar with leather or pasteboard between each plate. The plates

Electricity Course: Chem 106 Date: 7/11/2015 INTRODUCTION A galvanic cell is an electrochemical cell that goes through a redox reaction and produces electrical energy . It converts chemical energy to electrical energy and the energy goes from the anode to the cathode. In this lab we had manipulate an exothermic zinc reaction to produce electricity. The same process is used in the making of commercial batteries. A more detailed information about the procedure can be found in Cornerstone chemistry

are connected in a circuit together. In the last lab, hydrochloric acid as well as copper, lead, and magnesium were used to create voltaic cells. Batteries is an example of a voltaic cell. They have three main parts, an anode, a cathode, and the electrolyte. The cathode and anode (the positive and negative sides at either end of a traditional battery) connect the battery to the circuit. The electrolyte of a battery consists of soluble salts, acids or other bases in liquid, gelled and dry forms, and

Batteries are electrolysis going backwards, they convert chemicals to electricity-making cathode become positive, and anode negative. (“How does a battery work?” 2012) Cathode and anode electrodes are separated by the electrolyte. When the battery is connected to an object, chemical reactions take place. One of the reactions produces positive electrons, and electrons in the negative electrode. Positive

which to be treated, by electrodissolution of anodes. Compared with flocculation process and chemical coagulation, electrocoagulation (EC) has no of advantages, such as removal of the smallest colloidal particles. Compare to conventional coagulation process, Less amount of sludge is generated during EC process. Excessively addition of coagulants can be avoided by using EC, due to the generation of the coagulants by electro oxidation of a sacrificial anode. EC has easy operation and simple equipment