A compound X contains 50% sulpher and 50% oxygen by mass. what is the empirical ( simplest) formula of the compound X? Options a) SO b) SO2 c)SO3 d) SO4 please please Explain. :(

Question

20931 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2018-02-03T01:45:45

$=SO_2$

Assuming that the mass of the compound is 100g; therefore, mass of its constituent elements are:
$S=100gxx50%=50g$
$O=100gxx50%=50g$
Find the relative atomic masses of these elements which are obtainable from the periodic table; i.e.,
$S=32.07" g/mol"$
$O=16.00" g/mol"$
Now, find the mole value of each element.
$etaS=(50cancel(g))/((32.07cancel(g))/(mol))=1.5591mol$
$etaO=(50cancel(g))/((16.00cancel(g))/(mol))=3.1250mol$
Then, determine the ratio of moles using the smallest mole value as the denominator.
$S=1.5591/1.5591=1$
$O=3.1250/1.5591=2$
Therefore, the empirical formula of the compound is $S_1O_2$ or simply written as $SO_2$