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How to calculate the number of moles in an experiment?

An experiment is conducted where 54g of aluminium is reacted with chlorine to produce aluminium chloride.2Al + 3Cl Al(2)Cl(6)Determine the number of moles of aluminium used in this experiment.Determine the number of moles of chlorine gas required to react completely with 54.0g of aluminium.P/S the answer in my book indicates that the number of moles for aluminium is 2.I don't get it why must you ignore the 2 in 2Al?


Get a square of an iron on denim patch twice the size of the area where the glue is locatedPut your iron on medium heat and place the patch over where there is gluePress the iron onto the patch for about 10 seconds or until it feels like it's beginning to stick to the clothPeel the patch away and the glue should come right along with it.
you could stitch a cloth applique oniron on may scorch yarn and not be visiblewhy not make cloth quilt blocks with appliques?
As noted, your book has given you the answer to the first question One way to think about why you ignore the 2 in 2Al is thisIf I ask you, without showing you the chemical reaction, to calculate the number of moles of aluminum in 54 grams, could you do it? Would you need to know the rate at which my chemical reaction was going to consume the aluminum? The reason that you ignore it is that you are not dealing with a compound or isotope known as 2AlYou are dealing with the element aluminumYour reaction just happens to use 2 parts aluminum to 3 parts chlorine(Or at least, that's what the left side of your equation says)If I were to take those same 54 grams of aluminum and use them in a different reaction that used them at the rate of 3 parts aluminum to 1 part unobtainium, I would still have the same 54 grams ( 2 moles) of aluminumIn order to convert grams to moles for any substance, all you need to know is its atomic massFor Al, that is 27amu (rounded)The amu is also the number of grams-per-moleSo, 54 grams of Al is 2 molesNotice you do not need to see a chemical reaction involving the substance in order to make this calculation The 2 in 2Al simply tells you the rate (compared to other substances) at which Al is consumed by the reaction Your second question cannot be answered until you balance the equationI suspect that you have entered it incorrectlyPerhaps you had 3 Cl(2) on the left side? You would, in that case, need 3 moles of Cl(2)[edited] the problem with the proposed balanced equation 4Al + 3Cl2 2 Al2C3 is that it replaces 3CL with 3Cl(2), doubles the reaction rate of the aluminum, and produces a different compound Only the first step is neededBy simply replacing 3Cl with 3Cl(2), the equation is already balanced 2Al + 3Cl(2) Al(2)Cl(6).

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