The harder the water the more difficult it is to rust a hot-dip galvanised nail as it affects the pH and the action of sodium and chlorine ions that come from the dissolved salt in the water see this link. As you can see without water rusting doesnt take place in any cases. Experiment involves the corrosion of nails in Coke lemon juice oil and water. In conclusion the hypothesis was confirmed in that the nails that were covered in oil or grease were better protected against rusting by water as they rusted less than the nails that were not protected. There is no rustlittle rust on the iron nail in test tube D. My conclusion is that my hypothesis partially correct. The thick layer of Chromium and Zinc on the galvanised steel slows the rusting as it prevents oxygen reaching the metal at least for a while. The clorox had less oxygen than the vinegar or the water resulting in why the clorox showed less rust on the nail. Iron is susceptible to rusting. This experiment is a component of the Year 11 Chemistry course and was assigned as a Practical Assessment Task.

Controlling humidity test tube C prevents rusting. As you can see without water rusting doesnt take place in any cases. The hypothesis was proved partially correct as the most corrosion was recorded with aluminium foil in vinegar though it did not apply to the other metals in vinegar. If the results of the experiment were taken after just a few days the iron nail in the salty solution would have rusted more than the nail in the plain solution because NaCl speeds up the rusting process. Conclusion By using observing the electrochemical cell produced between an iron nail and another metal it was found that metals that are more reactive will protect the iron nail from corrosion in keeping with the hypothesis. There is no rusting on the iron nail in test tube E. The hematite is visible and covers the nail that was in the vinegar. If you are in high school you should probably weigh the nail with an analytical balance before the experiment and rub all the rust off after the experiment and express the rusting in terms of weight loss. Significant results were found in some metals placed in salt and tap water although not mentioned in the hypothesis. Since magnesium lost electrons to iron iron was prevented from losing electrons and could not form Fe2aq ions.

There is no rust observed on the iron nail in test tube C. The finishes prevent iron nails from rusting. The vinegar initially dissolved any small amount of rust that was on the nail then it began to slowly dissolve the iron itself as proven by your weight loss measurement. Galvanising using a more reactive metal such as zinc prevents the rusting of iron. The thick layer of Chromium and Zinc on the galvanised steel slows the rusting as it prevents oxygen reaching the metal at least for a while. The independent variable of this experiment. Conclusion By using observing the electrochemical cell produced between an iron nail and another metal it was found that metals that are more reactive will protect the iron nail from corrosion in keeping with the hypothesis. There is no rustlittle rust on the iron nail in test tube D. Conclusion In this project I can conclude that the vinegar made the nail rust faster. My conclusion is that my hypothesis partially correct.

Conclusion In this project I can conclude that the vinegar made the nail rust faster. The thick layer of Chromium and Zinc on the galvanised steel slows the rusting as it prevents oxygen reaching the metal at least for a while. Controlling humidity test tube C prevents rusting. The clorox had less oxygen than the vinegar or the water resulting in why the clorox showed less rust on the nail. A difficulty experienced during the experiment was that the liquids used reduced significantly in quantity by the end of the second week due to evaporation and had to be topped up. This experiment received a the following result. A Year 11 chemistry experiment which involves the reaction of nails in different types of liquid. The vinegar initially dissolved any small amount of rust that was on the nail then it began to slowly dissolve the iron itself as proven by your weight loss measurement. This video is a science experiment in which we want to know in which condition does the nail rust the fastestthis video is made by Kay Vanessa Raymond Nael. Conclusion By using observing the electrochemical cell produced between an iron nail and another metal it was found that metals that are more reactive will protect the iron nail from corrosion in keeping with the hypothesis.

Espeically galvanized nail lasts longer than coated mails. I think the iron will rust faster in the salt water than the fresh water and vinegar. This was because magnesium being more reactive lost electrons more easily than iron. The vinegar initially dissolved any small amount of rust that was on the nail then it began to slowly dissolve the iron itself as proven by your weight loss measurement. My conclusion is that my hypothesis partially correct. This experiment received a the following result. Only some of the substances used in the experiment were succesful. The harder the water the more difficult it is to rust a hot-dip galvanised nail as it affects the pH and the action of sodium and chlorine ions that come from the dissolved salt in the water see this link. The hematite is visible and covers the nail that was in the vinegar. Since magnesium lost electrons to iron iron was prevented from losing electrons and could not form Fe2aq ions.