What is the percent composition of O in Aluminum Sulfate?

Answer 1

There is 9.2758% Al3+ in a formula unit of aluminum oxide.

AnswerThe formula for aluminum oxide is Al2O3: Molar mass =581.77g/mol Al2O3.

In one mole Al2O3, there are two moles of Al3+ ions, therefore 2 moles Al3+ x 26.982g/mol Al3+ = 53.964g Al3+ in one mole of Al2O3.

GIVEN: mass of Al3+ = 53.964 gAl3+;Molar mass of Al2O3 = 581.77 gAl2O3

WANTED: % Al3+

EQUATION:

% Al3+...=...g Al3+x 100...g Al2O3

% Al3+...=...53.964gAl3+x100......=...9.2758%Al3+581.77g Al2O3

Answer 2

Aluminum Phosphate- AlPO4

Find the atomic masses for each element and multiply it by the number of atoms in the compound, then add.

Al- 27.0

P- 31.0

O- 16.0 * 4= 64.0

------------------------

122.0

Take the masses for each element and divide them by the total mass. Then change the answer to a percent.

Al 27.0 / 122.0= .221 = 22.1%

P- 31.0 / 122.0= .254= 25.4%

O- 64.0 / 122.0= .525= 52.5%

There is 22.1% of Aluminum, 25.4% of Phosphate, and 52.5% of Oxygen in Aluminum Phosphate.

Answer 3

Al is a metal, and thus wants to lose electrons to become like a noble gas, so it loses 3 electrons to have a [Ne] configuration, which we write as Al3+. Sulfate (SO4) has a 2- charge. Thus in order to get a neutral charge, the chemical formula for Aluminum sulfate must be Al2(SO4)3. Atomic Mass of each atom is added to get the formula mass. (Al = 27.0 g/mol * 2 atoms) + (3 * [S = 32.1 g/mol + O = 16.0 * 4 atoms]) = 342.3 g/mol

% mass of Al = (2 atoms * 27.0 g/mol) / (342.3 g/mol) = 15.77%

Answer 4

The molecular formula of aluminum sulfate is Al2(SO4)3. To calculate the percent composition of oxygen (O) in aluminum sulfate, we need to consider the number of oxygen atoms in the formula. There are 12 oxygen atoms in one molecule of Al2(SO4)3. To find the percent composition, we divide the total mass of the oxygen atoms by the molar mass of aluminum sulfate and multiply by 100. Therefore, the percent composition of oxygen in aluminum sulfate is (12 x 16 g/mol) / (342 g/mol) x 100 = 56.1%.

Answer 5

the percentage composition of aluminum sulfate is 342

Answer 6

Mr (Al2(SO4)3 ) = (2 x 27) + (3 x (32 + (4 x 16) ) ) = 342

Mr (Al) = 27

% by mass of Aluminum = (27/342) x 100 = 7.89%

Answer 7

Aluminium sulfate is Al2(SO4)3 and its molecular weight is 342.15 g/mol. There are 12 oxygens present.

So the percentage of oxygen = (12 x 16) / 342.15 = 0.561 or 56.1%

Answer 8

15.77%