Given the following skeleton equation, what are the coefficients for the chemicals in the reaction? __ FeSO4 + __ Al(OH)3 → __ A
2 answers:
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Answer:
There are 0.0186 moles of formula units in 6.35 grams of aluminum sulfate .
Explanation:
What's the empirical formula of aluminum sulfate?
Sulfate is an anion with a charge of -2 per ion. When sulfate ions are bonded to metals, the compound is likely ionic.
Aluminum is a group III metal. Its ions tend to carry a charge of +3 per ion.
The empirical formula of an ionic compound shall balance the charge on ions with as few ions as possible.
The least common multiple of 2 and 3 is 6. That is:
- Three sulfate ions
will give a charge of -6.
- Two aluminum ions
will give a charge of +6.
Pairing three ions with two
will balance the charge. Hence the empirical formula:
.
What's the mass of one mole of aluminum sulfate? In other words, what's the formula mass of ?
Refer to a modern periodic table for relative atomic mass data:
- Al: 26.982;
- S: 32.06;
- O: 15.999.
There are
- two Al,
- three S, and
- twelve O
in one formula unit of .
Hence the formula mass of :
.
How many moles of formula units in 6.35 grams of ?
.