first we work out the Mr.
Mr= 80g
Then we find out the Mr of Oxygen in NH4NO3.
Mr of oxygen=48g
Then we do 40/80 which equals 0.5 then we multiply it by 100 and we get 50%
This is our Percentage by mass.
The formula given shows that each formula unit contain two nitrogen atoms (one in the ammonium ion and one in the nitrate ion). The gram formula mass of ammonium nitrate is 80.04 and the gram Atomic Mass of nitrogen is 14.0067. Therefore, the percent by mass of nitrogen in ammonium nitrate is:
100[(2)(14.0067)/80.04] or 35.00 %, to the justified number of significant digits. (A more precise gram formula mass of ammonium nitrate would justify more significant digits.)
1. Determine the molar mass of NH4NO3 by determining the molar mass of each element in the formula and then adding them together.
N: 2 x 14.534g/mol = 29.068g/mol
H: 4 x 1.008g/mol = 4.032g/mol
O: 3 x 15.999g/mol = 47.997g/mol
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Molar mass of NH4NO3 = 81.097g/mol
2. Divide the molar mass of each element by the molar mass of NH4NO3 and multiply the result times 100. This gives you the percent composition of each element in the compound.
N: (29.068g/mol)/(81.097g/mol) x 100 = 35.843%
H: (4.032g/mol)/(81.097) x 100 = 4.971%
O: (47.997g/mol)/(81.097g/mol) x 100 = 59.188%
N: 1(14)= 14
O: 2(16)= 32
14+32= 46
32/24x100= 70%
NH4NO3
N - 14.0 X 2 = 28
H4 - 1.0 X 4 = 4
O3 - 16.0 X 3 = 48
Total molecular mass = 80
48/80 = 60%
Sodium bicarbonate contain 57,137 % oxygen.
The percentage by mass of sodium (Na) in a formula unit of sodium hydrogen carbonate (NaHCO3) is 27,38 %.
The percent by mass of oxygen in N2O4 is 69,56 %.
28 g N/80 g NH4NO3 *100
ammonium nitrate contains 35% nitrogen.
The percent by mass of oxygen in N2O4 is 69,56 %.
The mass percent of oxygen in SO2 is 50 %.
Determine the molar mass of NO2 using the subscripts in the formula and the atomic weights in grams from the periodic table. 1 mole NO2 = (1 x 14.0067g N) + (2 x 15.9994g O) = 46.0055g NO2 Calculate the moles NO2 by dividing the given mass by the molar mass. 25.5g NO2 x (1mol NO2/46.0055g NO2) = 0.554mol NO2
The answer is "one mole of NO2." Good Luck! Have a great day!
60%
The percent by mass of oxygen in N2O4 is 69,56 %.
To find the percent composition of oxygen in Na2O, find the total molar mass of the compound. Then, divide the molar mass of oxygen by the molar mass of the compound, and multiply by 100% to get the percent oxygen.
The mass percent of oxygen in SO2 is 50 %.
Determine the molar mass of NO2 using the subscripts in the formula and the atomic weights in grams from the periodic table. 1 mole NO2 = (1 x 14.0067g N) + (2 x 15.9994g O) = 46.0055g NO2 Calculate the moles NO2 by dividing the given mass by the molar mass. 25.5g NO2 x (1mol NO2/46.0055g NO2) = 0.554mol NO2
To determine the percentage of oxygen in FeCr2O4, you would first calculate the molar mass of the compound (iron(II) chromite) using the atomic masses of each element (Fe = 55.85 g/mol, Cr = 51.996 g/mol, O = 16 g/mol). Then, calculate the molar mass percentages of each element within the compound, and finally, determine the percentage of oxygen by mass in the compound.
4.17 g O3
The answer is "one mole of NO2." Good Luck! Have a great day!
NO2, or nitrogen dioxide.
Estriol (C18H24O3) contain 16,644 % oxygen.
60%
The mass of the elements that are not oxygen equals 194.8g. The mass of oxygen is 230g - 194.8g = 35.2g of oxygen. Mass percent of oxygen = 35.2g O/230g x 100 = 15% O
Oxygen atoms weigh more than Hydrogen atoms.