1 mole occupies 22.4 liters. 0.5 moles occupies 11.2 liters at STP.
4NH3 + 5O2 -> 4NO + 6H2O I suspect NH3 limits. Let's see. 5.15 O2 ( 4 mole NH3/5 mole O2) = 4.12 mole NH3 you do not have that much ammonia, so it limits and drives the reaction. 3.80 mole NH3 (4 mole NO/4 mole NH3) = 3.80 moles of NO made
nitrogen weighs 14, hydrogen weighs 1, so NH3 weighs 14+(3x1)=17grams
The molecular mass of ammonia (NH3) is 18.03 grams/mole
The molecular weight of NH3 is 17.03-grams per mole and 14.01 for N2. The reaction is N2 + 3H2 = NH3. Therefore for every 1-mole of N2 as a reactant 1-mole of NH3 is produced. .2941-moles of NH3 is produced with a mass of 5.01-grams.
2 x 0.60 = 1.2 the reaction is N2 + 3H2 -> 2NH3 (1 mole of nitrogen N2 give 2 moles of NH3)
The volume of ammonia is 19,5 L.
4NH3 + 5O2 -> 4NO + 6H2O I suspect NH3 limits. Let's see. 5.15 O2 ( 4 mole NH3/5 mole O2) = 4.12 mole NH3 you do not have that much ammonia, so it limits and drives the reaction. 3.80 mole NH3 (4 mole NO/4 mole NH3) = 3.80 moles of NO made
nitrogen weighs 14, hydrogen weighs 1, so NH3 weighs 14+(3x1)=17grams
The mass of NH3 mole = its molecular weight = 14 + 3 x 1 = 17 The mass of H2O mole = its molecular weight = 2 x 1 + 16 = 18 This means that one mole of NH3 weigh less than one mole of H2O
The molecular mass of ammonia (NH3) is 18.03 grams/mole
The molecular weight of NH3 is 17.03-grams per mole and 14.01 for N2. The reaction is N2 + 3H2 = NH3. Therefore for every 1-mole of N2 as a reactant 1-mole of NH3 is produced. .2941-moles of NH3 is produced with a mass of 5.01-grams.
Calculation in two steps:mass (g) / molar mass (g/mol) = moles NH4NO3 6.84 / (1*14.01 + 4*1.008 + 1*14.01 + 3*16.00) =6.84 / (80.052) = 0.0854 mole NH4NO3NH4NO3 moles * 2 moles N/mole NH4NO3 = moles N atoms 0.00854*2 = 0.171 moles N atoms
Molecules of ammonia? Will assume so. 4.2 X 1025 molecules NH3 (1 mole NH3/6.022 X 1023)(17.034 grams/1 mole NH3) = 1188 grams of ammonia ===================( could call it 1200 grams NH3 for significant figure correctness )
2 x 0.60 = 1.2 the reaction is N2 + 3H2 -> 2NH3 (1 mole of nitrogen N2 give 2 moles of NH3)
At standard temperature and pressure (STP), one mole of any ideal gas occupies 22.4 liters. To find the number of moles of ammonia gas (NH₃) required to fill a volume of 50 liters, you can use the formula: moles = volume (liters) / volume per mole (liters/mole). Therefore, the calculation is 50 liters / 22.4 liters/mole = approximately 2.24 moles of NH₃ are needed.
The reaction would be H2 + 3N2 ==>2NH3moles H2 used = 5.69104 g x 1 mole/2.00 = 2.84552 moles H2moles NH3 produced (assuming N2 is NOT limiting) = 2 moles NH3/mole H2 x 2.84552 moles H2 = 5.69104 moles NH3 producedMolecules of NH3 produced = 5.69104 moles x 6.02x10^23 molecules/mole = 3.4x10^24 molecules
The bond energy of NH3, which is the energy required to break one mole of NH3 molecules into its individual atoms, is approximately 391 kJ/mol.