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This lab was performed in the 4th of december 2017,in International English Gymnasium, and commenced at 11.05 GMT and ceased at 12:20 GMT.  In Proust’s law , also called ”the law of definite composition” expressess that a chemical compound will always contain its components elements at an established proportion of elements by mass. This states that the result of a given compound will always have the identical combination of atoms that contains an established ratio of mass. Mass is the core element in the composition of a substance, using mass we are able to quickly calculate the percentage composition which describes the composition of the given element. As we know the composition of a substance can also be represented by the combination of atoms which can direct to a certain percentage of the compound which is called a chemical formula. There are different types of formulae but the one that we utilized was the Empirical Formula. The empirical formula is the calculation of the lowest ratio of atoms that combine to create a compound. The problem is that molecular formulas are not always empirical formulas. A common example that shows this dilemma is the following,the molecular formula hydrogen peroxide (H2O2) has the empirical formula “HO” but its molecular formula is H202 , this shows that even though sometimes molecular formulas are identical to the empirical formula, eg. H2O(Molecular Formula) ? H2O(Empirical Formula) and in this case it is identical, it does not always exist (Helmenstine, Ph.D. Anne Marie, 2017) . As we know we can calculate the percent composition by using the mass information given to them, that mass information is then calculated to moles in order to use it in formulas because of the fact that we require mass to know the amount of atoms an element containsThe definition of percent compositions is that it is the percent of mass contained in each element compound, a very common example is H2O. We know that one mole of water is 18.0152 but in the compound there is two moles of Hydrogen thus resulting in 2 x 1.008(Mole of Hydrogen) = 2.016 grams

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