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 percent by mass of oxygen in N2O4 is 69,56 %.
The gram-formula mass of a compound is the sum of the atomic masses of all the atoms in a formula unit of the compound. For NO2, the gram-formula mass is calculated by adding the atomic mass of nitrogen (N) and two times the atomic mass of oxygen (O).
(16.0g + 16.0g)/(32.1g + 16.0g + 16.0g) x 100 %
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 molar mass of SO2 is 64.07 g/mol. Since oxygen has a molar mass of 16 g/mol and there are 2 oxygen atoms in SO2, the total mass of oxygen in SO2 is 32 g. Therefore, the mass percent of oxygen in SO2 is 32/64.07 * 100% = 50.05%.
The mass percent of oxygen is approximately 21% in Earth's atmosphere.
To calculate the mass of ozone produced, we need to first determine the balanced chemical equation for the reaction between NO2 and oxygen to form ozone. Then, we can calculate the molar mass of ozone and use stoichiometry to find the mass produced from 4.00 g of NO2.
The percent by mass of oxygen in N2O4 is 69,56 %.
The gram-formula mass of a compound is the sum of the atomic masses of all the atoms in a formula unit of the compound. For NO2, the gram-formula mass is calculated by adding the atomic mass of nitrogen (N) and two times the atomic mass of oxygen (O).
To find the mass percent of oxygen in the compound, first calculate the total mass of the compound by adding the masses of magnesium and oxygen: 14.5 g + 3.5 g = 18.0 g. Then, use the formula for mass percent: (mass of oxygen / total mass) × 100%. Thus, the mass percent of oxygen is (3.5 g / 18.0 g) × 100% ≈ 19.44%.
To find the percent by mass of oxygen in propanal (CH3CH2CHO), calculate the molar mass of oxygen (O) and the molar mass of the entire compound. Then divide the molar mass of oxygen by the molar mass of the entire compound and multiply by 100 to get the percentage. In this case, the percent by mass of oxygen in propanal is around 47.3%.
To find the percent of oxygen by mass in a compound, you need to know the molar mass of the compound and the molar mass of oxygen. Divide the molar mass of oxygen by the molar mass of the compound and multiply by 100 to get the percentage.
To determine the mass percent of oxygen in a compound, you would calculate the mass of oxygen in the compound and then divide it by the total mass of the compound, before multiplying by 100. The formula is: (mass of oxygen in compound / total mass of compound) x 100%.
(16.0g + 16.0g)/(32.1g + 16.0g + 16.0g) x 100 %
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 molar mass of SO2 is 64.07 g/mol. Since oxygen has a molar mass of 16 g/mol and there are 2 oxygen atoms in SO2, the total mass of oxygen in SO2 is 32 g. Therefore, the mass percent of oxygen in SO2 is 32/64.07 * 100% = 50.05%.
The molar mass of SO2 is 64.07 g/mol. Oxygen has a molar mass of 16.00 g/mol. To calculate the mass percent of oxygen in SO2, we can divide the molar mass of oxygen (32.00 g) by the molar mass of SO2 (64.07 g) and multiply by 100 to get 50.05%.