To determine the mass of NO2 formed when NO reacts with O2, we need to write and balance the chemical equation for the reaction. The balanced equation is 2NO + O2 -> 2NO2. From the equation, we see that 2 moles of NO will react with 1 mole of O2 to produce 2 moles of NO2. Next, we need to calculate the number of moles of O2 present in 384g using its molar mass. Finally, we can use the mole ratio from the balanced equation to find the mass of NO2 formed.
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 NO2 is 46.01 g/mol. Therefore, 3.00 moles of NO2 have a mass of 138.03 grams (3.00 moles x 46.01 g/mol).
To calculate the number of moles in 25.6 g of NO2, you need to divide the given mass by the molar mass of NO2, which is 46.01 g/mol. Moles = 25.6 g / 46.01 g/mol = 0.556 moles. Therefore, there are 0.556 moles of NO2 in 25.6 g.
The molar mass of NO2 (nitrogen dioxide) is approximately 46 grams per mole.
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).
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 find the number of moles in 1.18 g of NO2, you need to divide the given mass by the molar mass of NO2. The molar mass of NO2 is approximately 46 g/mol. So, 1.18 g / 46 g/mol = roughly 0.026 moles of NO2.
The molar mass of NO2 is 46.01 g/mol. Therefore, 3.00 moles of NO2 have a mass of 138.03 grams (3.00 moles x 46.01 g/mol).
To calculate the number of moles in 25.6 g of NO2, you need to divide the given mass by the molar mass of NO2, which is 46.01 g/mol. Moles = 25.6 g / 46.01 g/mol = 0.556 moles. Therefore, there are 0.556 moles of NO2 in 25.6 g.
To find the number of moles in 19 g of NO2, we first need to determine the molar mass of NO2, which is 46.01 g/mol. Next, we divide the given mass by the molar mass: 19 g / 46.01 g/mol ≈ 0.413 moles of NO2.
The molar mass of nitrogen dioxide (NO2) is approximately 46 grams per mole.
The molar mass of NO2 (nitrogen dioxide) is approximately 46 grams per mole.
In this reaction, Ca2+ reacts with NO2^1- to form Ca(NO2)2. The balanced chemical equation for this reaction is: Ca2+ + 2NO2^- → Ca(NO2)2.
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).
Magnesium will react with nitric acid and most other acids to produce hydrogen gas.
If the reaction is not specified, we can't determine the exact moles of NO formed from NO2 based on this information alone. The reaction and stoichiometry are needed to calculate the moles of NO produced from 8.44 moles of NO2.
Potassium nitrite, not Potassium nitrate which is KNO3