I need this answer right now please and thank you. A compound is found to contain 50.05% sulfur (S) and 49.95% oxygen (O) by weight. What is the empirical formula for this compound?
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1
Answer:
SO2
Explanation:
Assuming that the mass of the compound is 100g; therefore, mass of its constituent elements are:
S
=
100
g
×
50
%
=
50
g
O
=
100
g
×
50
%
=
50
g
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.
η
S
=
50
g
32.07
g
m
o
l
=
1.5591
m
o
l
η
O
=
50
g
16.00
g
m
o
l
=
3.1250
m
o
l
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
1
O
2
or simply written as
S
O
2
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