In writing and balancing equations using sulfur chemists usually use the empirical formula, S, rather than the molecular formula. Why?
I'm not sure how to answer this question.
It makes no difference on the proudcts, nor reactants. There is no difference in mass comparing 8S to S8 or any other forms of naturally occuring sulfur.
S is easier to work with than S8
If you really want to know how many mols of S8 you used, multiply S and the rest of the balanced equation by 8 by 8
Here is the long answer:-)
http://www.ibchem.com/faq/2008/09/18/what-is-the-molecular-formula-of-sulphur/
To answer this question, we need to understand the difference between empirical formula and molecular formula.
The empirical formula represents the simplest whole number ratio of atoms in a compound. On the other hand, the molecular formula shows the actual number of atoms of each element in a molecule.
In the case of sulfur, the empirical formula is S, which means that compounds commonly contain only one sulfur atom. Using the empirical formula is more convenient in writing and balancing equations because it simplifies the notation and makes the equations easier to understand. It also allows chemists to focus on the overall chemical reaction rather than the specific molecular details.
However, it is important to note that sometimes chemists may use the molecular formula for certain sulfur compounds, especially when the compound is well-known and its structure is crucial to the reaction being studied. But in most cases, using the empirical formula S is sufficient for general purposes.