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
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.
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%
the percentage composition of aluminum sulfate is 342
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%
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%
15.77%
The percent composition of ethanol is: - C: 52,13 % - O: 34,74 % - H: 13,13 %
21.5% oxygen30.9% sodium47.6% chlorineSee the related question below for the process in determining percent composition.
The formula of water is H2O. The gram atomic mass of hydrogen is 1.008 and the gram atomic mass of oxygen is 15.999. Therefore, the mass percent composition of hydrogen in water is 100{(2)(1.008)/[(2)(1.008) + 15.999] or 11.19 %.The percent composition of hydrogen in water is: 11,19 %.
The total mass is 222.6 + 77.4 = 300.0 g. The percent of nitrogen is therefore: 100(222.6/300.00) = 74.2 %. By difference, the percent of oxygen is 25.8 %.
R-O-SO3-
The percent composition of ethanol is: - C: 52,13 % - O: 34,74 % - H: 13,13 %
The percent composition of nitrous oxide is: - N: 63,649 % - O: 36,351 %
Aluminum sulfate has the chemical formula Al2(SO4)3, so the elements present would be aluminum (Al), sulfur (S) and oxygen (O).
BeO has 64 % oxygen.
s 50% o 50%
The percent composition of cysteine (C3H7NO2S) is: - C: 29,75 % - O: 26,43 % - H: 5,83 % - N: 11,57 % - S: 26,42 %
The percent composition of the neutral aluminium acetate - Al(C2H3O2)3 - is: - C: 35,29 % - O: 47,04 % - H: 4,45 % - Al: 13,23 %
Add up the compound's molar mass: Na=2(23), S=1(32), O=4(16). Sum is 142. Oxygen's part of that total is 64 (16x4). Percent is part/total, so 64/142 = 0.4507 = 45.1%.
373.01% c, 2.22% h, 18.50% n, 42.26% o
Na2SO4 = 46+32+64 = 142 Na = 46/142 * 100 = 32.39 % S = 32/142 * 100 = 22.54 % O = 64/142 * 100 = 45.08 %
88.5%
Percent composition means finding the total mass of each element in a molecule and then dividing it by the molecular mass. Use the molecular formula to help you find out how many atoms of each element you'll need. For carbon: 6 C x 12 g = 72 g For hydrogen: 10 H x 1 g = 10 g For oxygen: 5 O x 16 g = 80 g Molecular mass = C + H + O = 72 + 10 + 80 = 162 g Percent composition of C = 72/162 = 0.4444 = about 44.45% Percent composition of H = 10/162 = 0.061728395 = about 6.17% Percent composition of O = 80/162 = 0.49382716 = about 49.38%