
Interpretation:
A balanced equation for the given hypothetical reaction is to be written, and the oxidation and hybridization state of sulfur in
required and the mass of
produced is to be calculated.
Concept introduction:
The oxidation state of an element is zero. The sum of the oxidation states of all the elements is equal to zero in a molecule of a compound, and in case of an ion, it is equal to the charge on the ion. Oxygen has a fixed oxidation state of
in its compounds.
To find hybridisation of an atom in a molecule, at first draw the Lewis structure of the molecule. Find the number of electrons domains around the atom. This gives the number of hybrid orbitals required for bonding. The number of hybrid orbitals is equal to the number of atomic orbitals that hybridise. Thus, one
and one
orbital hybridize to form two
and two
orbitals hybridize to form three
hybrid orbitals, and one
and three
orbitals hybridize to form four
hybrid orbitals.
The conversion factor is a fraction that is used to convert one unit to another. Use of more than one factor to find a solution is called dimensional analysis.

Answer to Problem 115AP
Solution: The balanced equation for the reaction is as follows:
The oxidation state of sulfur in elemental sulfur
is
is
is
is
is
and mass of
produced is
Explanation of Solution
The hypothetical reaction between elemental sulfur and sulfur trioxide is as follows:
The balanced equation for this reaction is as follows:
In
The oxidation state of oxygen is
Let
is the oxidation state of sulfur.
Then
is calculated as follows:
The oxidation state of sulfur in
is
In
Let
is the oxidation state of sulfur and the oxidation state of oxygen is
is calculated as follows:
The oxidation state of sulfur in
is
The Lewis structure of
In
hybrid orbitals.
In
hybrid orbitals.
In
hybrid orbitals.
Consider the balanced equation:
One mole of
combines with
moles of
moles of
is
is given as
Convert the mass of
to moles as follows:
One mole of
combines with
moles of
Thus, for
needed is calculated as follows:
Molar mass of
is
Thus, the amount of
One mole of
produces
moles of
Thus, for
produced is calculated as follows:
Molar mass of
is
Thus, the amount of
Hence, mass of
required is
produced is
The balanced equation for the reaction between elemental sulfur and sulfur trioxide to produce sulfur dioxide is written; the oxidation and hybridization state of sulfur in
required and the mass of
produced by
of elemental sulfur are calculated.
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Chapter 9 Solutions
Chemistry
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