0
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%
Wiki User
∙ 14y ago
Add your answer:
Earn +20 pts
How many g of nitrogen are in 35.8kg of ammonium nitrate?
Mass(g)of N = 35.8 g NH4NO3 X 28 g of N / 80 g NH4NO3 = 12.53 g N
What is the mass percent of nitrogen in ammonium carbonate?
14.58%
What is the percent by mass of oxygen in NO2?
The molar mass of NO2 is 46.01 g/mol. The molar mass of oxygen in NO2 is 32.00 g/mol. To find the percent by mass of oxygen in NO2, divide the molar mass of oxygen by the molar mass of NO2 and multiply by 100%. Therefore, the percent by mass of oxygen in NO2 is (32.00 g/mol / 46.01 g/mol) x 100% ≈ 69.6%.
How many grams of nitrogen are in 48.5g ammonium nitrate?
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.
Calculate the percent nitrogen by mass in chlorophyll C55H72MgN4O5?
To calculate the percent nitrogen by mass in chlorophyll, first find the molar mass of nitrogen: 14.01 g/mol. Then calculate the molar mass of the entire molecule using the atomic masses of C, H, Mg, N, and O. Finally, divide the mass of nitrogen by the total molar mass of the compound and multiply by 100 to get the percentage. In this case, the percent nitrogen by mass in chlorophyll is approximately 1.53%.
What compound has a lower percent of mass by nitrogen- NO or N2O3?
The oxide N2O3 has a lower percent of mass nitrogen.
What is the percent of nitrogen in CN2H4O?
The molar mass of CN2H4O is 42 g/mol. The molar mass of nitrogen is 14 g/mol. To find the percent of nitrogen in CN2H4O, divide the molar mass of nitrogen by the molar mass of CN2H4O and multiply by 100. The percent of nitrogen in CN2H4O is approximately 33.3%.
How many g of nitrogen are in 35.8kg of ammonium nitrate?
Mass(g)of N = 35.8 g NH4NO3 X 28 g of N / 80 g NH4NO3 = 12.53 g N
What is the mass percent of nitrogen in ammonium carbonate (NH4)2CO3?
To calculate the mass percent of nitrogen in ammonium carbonate (NH4)2CO3, first find the molar mass of the compound: 2(N) + 8(H) + 1(C) + 3(O) = 96 g/mol. The molar mass of nitrogen in the compound is 2(N) = 28 g/mol. To find the mass percent of nitrogen, divide the molar mass of nitrogen by the molar mass of the compound and multiply by 100: (28 g/mol / 96 g/mol) x 100 = 29.2%.
What is the mass percent of nitrogen in ammonium carbonate?
14.58%
How do you find the molar mass of HNO3?
To find the molar mass of HNO3, you would add up the atomic masses of hydrogen (H), nitrogen (N), and three oxygen atoms (O) in one molecule of HNO3. The molar mass of HNO3 is approximately 63.01 grams per mole.
What is the percent by mass of oxygen in NO2?
The molar mass of NO2 is 46.01 g/mol. The molar mass of oxygen in NO2 is 32.00 g/mol. To find the percent by mass of oxygen in NO2, divide the molar mass of oxygen by the molar mass of NO2 and multiply by 100%. Therefore, the percent by mass of oxygen in NO2 is (32.00 g/mol / 46.01 g/mol) x 100% ≈ 69.6%.
What is the percent composition of nitrogen in NH42HPO4?
To calculate the percent composition of nitrogen in NH4 2HPO4, first calculate the molar mass of NH4 2HPO4 ( nitrogen: 14.01 g/mol, hydrogen: 1.01 g/mol, phosphorus: 30.97 g/mol, oxygen: 16.00 g/mol). Then, find the molar mass of nitrogen in NH4 2HPO4 ( nitrogen: 14.01 g/mol x 2). Finally, divide the molar mass of nitrogen by the molar mass of NH4 2HPO4 and multiply by 100 to get the percent composition of nitrogen.
How many grams of nitrogen are there in NH4NO3?
Firstly, find the percent composition of hydrogen in the compound (ammonium nitrate). So we have: 2 x Nitrogen atom = 28.02 amu 4 x Hydrogen atoms = 4.04 amu 3 x Oxygen atoms = 48.00 amu Total of: 80.06 amu or g/mol % H = 4.04 g/mol ÷ 80.06 g/mol = 0.050462153385 = 5.05 % (sig. figs.) Then, we take the percentage of hydrogen and multiply it by the mass of the substance. 50.00 g NH4NO3 x 0.050462153385 = 2.52310766925 = 2.52 g H So, there is 2.52 g of hydrogen in 50.00 g of NH4NO3
What is the mass percent of nitrogen in the dyeing agent picric acid (C6H3N3O7)?
The percentage of nitrogen in the picric acid is 18,34 %.
How many grams of nitrogen are in 48.5g ammonium nitrate?
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.
Which has a higher percentage of nitrogen ammonia NH3 or ammonium nitrate NH4NO3?
Ammonium nitrate (NH4NO3) has a higher percentage of nitrogen compared to ammonia (NH3). In ammonium nitrate, nitrogen accounts for about 35% of the compound's molecular weight, whereas in ammonia, nitrogen accounts for about 82% of the molecular weight.
