# of AtomsAt Wt.Total Wt.Nitrogen214.006728.0134Hydrogen41.007944.03176Oxygen315.999447.9982Total Molecular weight80.04% of Nitrogen=28.01/80.04
=
35%
Mass of Nitrogen: 14g/mol Mass of Ammonium Nitrate (NH4NO3): 14 + 1x4 + 14 + 16x3 = 80g/mol ∴ % of Nitrogen in Ammonium Nitrate = 14/80 * 100 = 17.5%
Ammonium Nitrate = NH4NO3 or N2H4O3 the total mass of a ammonium nitrate molecule is as follows: 2*14u + 4*1u + 3*16u = 28u + 4u + 48u = 80u now, the total mass of Nitrogen in one ammonium nitrate is 2*14u = 28u. Then, we divide 28 (the mass of Nitrogen) by 80 (total mass)= 28/80 = 0.35, which is the ratio for Nitrogen mass divided by total mass. then, we get the 48.5 grams (total mass) and multiply it by this ratio (0.35): 48.5 * 0.35 = 16.975 grams of Nitrogen in 48.5 grams of Ammonium Nitrate.
1 mole of Ammonium Nitrate= 80g (R.A.M of compound) Therefore 8g of Ammonium nitrate= 8g/80g= 0.1 mole (moles = mass given over molar mass)
80.043 g/mol
The chemical formula of Ammonium sulfate is (NH4)2SO4. The first step to these problems is finding all the atomic weights of the elements involved (including how many atoms of each element there is) and then adding them all up to get the total molecular mass of ammonium sulfate.Nitrogen = 14.0 × 2 = 28.0 gramsHydrogen = 1.00 × 8 = 8.00 gramsSulfur = 32.1 gramsOxygen = 16.0 × 4 = 64.0 grams-------------------------------------------Ammonium sulfate = 132.1 gramsThen to figure out the percentage of nitrogen in the compound, take the total mass of nitrogen and divide it by the total mass.Mass of nitrogen ÷ mass of ammonium sulfate = % nitrogen28.0 ÷ 132.1 = .212 = 21.2% nitrogen in ammonium sulfate(NH4)2SO4Percentage nitrogen by mass=(Molar mass of nitrogen)/(Molar mass of ammonium sulfate)*100In ammonium sulfate there are 2 Nitrogens, 8 Hydrogens, 4 Oxygens and 1 Sulfur, and their molar masses are 14, 1, 16 and 32 respectively. So, by dividing the molar mass of nitrogen in the compound by the total molar mass of the compound and multiplying it by one hundred we get the percentage of nitrogen.(14*2)/(14*2+1*8+16*4+32)*100= 21.2121...=21%
The percentage of nitrogen in aluminium nitrate is 19,72 %.
Mass of Nitrogen: 14g/mol Mass of Ammonium Nitrate (NH4NO3): 14 + 1x4 + 14 + 16x3 = 80g/mol ∴ % of Nitrogen in Ammonium Nitrate = 14/80 * 100 = 17.5%
Ammonium Nitrate = NH4NO3 or N2H4O3 the total mass of a ammonium nitrate molecule is as follows: 2*14u + 4*1u + 3*16u = 28u + 4u + 48u = 80u now, the total mass of Nitrogen in one ammonium nitrate is 2*14u = 28u. Then, we divide 28 (the mass of Nitrogen) by 80 (total mass)= 28/80 = 0.35, which is the ratio for Nitrogen mass divided by total mass. then, we get the 48.5 grams (total mass) and multiply it by this ratio (0.35): 48.5 * 0.35 = 16.975 grams of Nitrogen in 48.5 grams of Ammonium Nitrate.
The percentage of nitrogen is 29,16 %.
4
The chemical formula of ammonium nitrate is NH4NO3.The molecular mass is 80,052 g.
1 mole of Ammonium Nitrate= 80g (R.A.M of compound) Therefore 8g of Ammonium nitrate= 8g/80g= 0.1 mole (moles = mass given over molar mass)
80.043 g/mol
The chemical formula of Ammonium sulfate is (NH4)2SO4. The first step to these problems is finding all the atomic weights of the elements involved (including how many atoms of each element there is) and then adding them all up to get the total molecular mass of ammonium sulfate.Nitrogen = 14.0 × 2 = 28.0 gramsHydrogen = 1.00 × 8 = 8.00 gramsSulfur = 32.1 gramsOxygen = 16.0 × 4 = 64.0 grams-------------------------------------------Ammonium sulfate = 132.1 gramsThen to figure out the percentage of nitrogen in the compound, take the total mass of nitrogen and divide it by the total mass.Mass of nitrogen ÷ mass of ammonium sulfate = % nitrogen28.0 ÷ 132.1 = .212 = 21.2% nitrogen in ammonium sulfate(NH4)2SO4Percentage nitrogen by mass=(Molar mass of nitrogen)/(Molar mass of ammonium sulfate)*100In ammonium sulfate there are 2 Nitrogens, 8 Hydrogens, 4 Oxygens and 1 Sulfur, and their molar masses are 14, 1, 16 and 32 respectively. So, by dividing the molar mass of nitrogen in the compound by the total molar mass of the compound and multiplying it by one hundred we get the percentage of nitrogen.(14*2)/(14*2+1*8+16*4+32)*100= 21.2121...=21%
14.58%
28.2%
The formula for sodium nitrate is NaNO3, showing that each formula unit contains one sodium atom, one nitrogen atom, and three oxygen atoms. The gram atomic masses of sodium, nitrogen, and oxygen are 22.9898, 14.0067, and 15.9994 respectively. Therefore, the percentage by mass of nitrogen in the compound is: 100{14.0067/[14.0067 + 22.9898 + 3(15.9994)]} or about 16.4795, to the justified number of significant digits.