Corrosion is the returning of metals back into their natural constituents when exposed to an atmosphere with which it can react. Both metals and non-metals are able to undergo redox reactions as well as other ceramics and polymers which are known to undergo a similar process which is referred to as degradation. This investigation aims to outline and assess the factors affecting corrosion and explore in depth how redox reactions work. Reduction and oxidization reactions (redox reactions) are responsible for corrosion. Half reaction equations will be playing a major role in this investigation. (Corrosion technology Australia. 2009) Redox reactions are an exchange of electrons between materials. In a redox reaction there is always an anode (electron donor) and a cathode (electron recipient). The exchange of the electrons can be either in a direct process or can be an indirect transfer of electrons along a conductor from the anode to the cathode. Either direct or indirect, the corrosion will always occur at the anode. My experiment is aimed at testing the corrosion of 2 different types of nails in a certain molar solution of salt water in anticipation of determining which of the two would be more suitable for beachside residencies. I hypothesized that the iron nails would almost double in content of rust as the molarity of the solution they’re soaked in increases. The galvanized nails hopefully will end up with limited amounts of rust in all solutions. The activity series plays a major role in corrosion itself. The activity series is basically an empirical series of metals; in order of reactivity from highest to lowest. Gold being the least reactive at the bottom of the list and lithium being the most reactive at the top of the list. Starting at gold and working up to lithium at the top of the list; the metals increase in reactivity, lose electrons more readily to form positive ions, corrode more readily, require more energy to be...
Please join StudyMode to read the full document