Which explains aluminum\'s resistance to corrosion? Any aluminum oxide that forms readily falls off the metal and exposes the corrosion-resistant metal. The aluminum oxide that forms adheres to the metal surface. The reduction half-reaction Al3+(aq) + 3e- ---gt; Al(s) occurs readily. The standard reduction potential for the Al3+/Al half-reaction is above the standard reduction potential for the O2/H2O half-reaction.The aluminum oxide that forms adheres to the metal surface explains aluminum\'s resistance to corrosion. Aluminum naturally forms a protective oxide film, which is stable in aqueous media when the pH is between about 4.0 and 8.5. The oxide film is naturally self-renewing and accidental abrasion or other mechanical damage of the surface film is rapidly repaired. The conditions that promote corrosion of aluminum and its alloys, therefore, must be those that continuously abrade the film mechanically or promote conditions that locally degrade the protective oxide film and minimize the availability of oxygen to rebuild it.i would start by plugging in some of those key terms into wikipedia. it often has shockingly good engineering physics articles. there are really only 4 variables: exhaust tube, annealing furnace, age hardened
aluminum alloy. play with those, and you might find terms that lead you to your answerThe fourth one.the fourth one is correct the fourth statement tells us that aluminium is more reactive(it has higher electrode potential) so it cannot be displaced by 02/H20 which has lower electrode potential (which means it is less reactive)so less reactive cannot displace more reactive hope so it will helpthe fourth statement.Other related question