25 grams / (17 grams/mole) x 6.022x1023 molecules/mole = 8.9x1023 molecules
There are no molecules.There are four atoms.
Answer: 4.3 gram
Each mole of NH3 is 14 g + 3 times 1 g = 17 g in total,
so:
0.25 mole = 0.25 x 17 = 4.3 gram
1g of NH3 is 0.5871645822324moles (divide by 17.031). Now multiply this by avagadros number of 6.022x10^23, and you get 3.536x10^23 molecules.
NH3 = 17g/mol, and 25/17 = about 1.5mol. 1.5 x (6x10^23) = 9x10^23, which represents the number of NH3 molecules. NH3 = 4 atoms per molecule, so (9x10^23) x 4 = 3.6x10^24 atoms total.
25 grams of nitrogen trihydride (NH3) is equivalent to 1,468 moles.
813.28
1 mole N2O3 = 76.0116g N2O3 (atomic weights x subscripts) 1 mole N2O3 = 6.022 x 1023 molecules N2O3 75g N2O3 x (1mol N2O3/76.0116g N2O3) = 0.99mol N2O3 0.99mol N2O3 x (6.022 x 1023 molecules N2O3/1mol N2O3) = 6.0 x 1023 molecules N2O3
The number of ammonia molecules is 59 720.10e23.
NH3 Molecules = ( 8.1 x 10^20 H atoms ) ( 1 NH3 molecule / 3 H atoms ) NH3 Molecules = 2.7 x 10^20 NH3 molecules NH3 moles = ( NH3 molecules ) / ( N Avogadro ) NH3 moles = ( 2.7 x 10^20 NH3 molecules ) / ( 6.022 x 10^23 molecules / mole ) NH3 moles = 4.48 x 10^-4 NH3 moles <--------------
Balanced equation is N2 + 3H2 ==> 2NH33.07104 g H2 x 1 mol/1.0079 g = 1.7679 moles H2 presentmoles NH3 produced = 2/3 x 1.7679 moles = 1.1786 moles NH3 formedmolecules NH3 = 1.1786 moles x 6.022x10^23 molecules/mole = 7.098x10^23 molecules (4 sig figs based on sig figs used in 6.022x10^23)
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 answer is 1,57.10e27 molecules.
1 mole N2O3 = 76.0116g N2O3 (atomic weights x subscripts) 1 mole N2O3 = 6.022 x 1023 molecules N2O3 75g N2O3 x (1mol N2O3/76.0116g N2O3) = 0.99mol N2O3 0.99mol N2O3 x (6.022 x 1023 molecules N2O3/1mol N2O3) = 6.0 x 1023 molecules N2O3
The number of ammonia molecules is 59 720.10e23.
NH3 Molecules = ( 8.1 x 10^20 H atoms ) ( 1 NH3 molecule / 3 H atoms ) NH3 Molecules = 2.7 x 10^20 NH3 molecules NH3 moles = ( NH3 molecules ) / ( N Avogadro ) NH3 moles = ( 2.7 x 10^20 NH3 molecules ) / ( 6.022 x 10^23 molecules / mole ) NH3 moles = 4.48 x 10^-4 NH3 moles <--------------
The mass is 9,6.10e-22 g for 34 molecules.
Balanced equation is N2 + 3H2 ==> 2NH33.07104 g H2 x 1 mol/1.0079 g = 1.7679 moles H2 presentmoles NH3 produced = 2/3 x 1.7679 moles = 1.1786 moles NH3 formedmolecules NH3 = 1.1786 moles x 6.022x10^23 molecules/mole = 7.098x10^23 molecules (4 sig figs based on sig figs used in 6.022x10^23)
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
74.168 u NH3Determine relative mass of NH3 molecule: (1 x 14.007 u N) + (3 x 1.008 u H) = 42.357 uMultiply the number of molecules of NH3 by its relative molecular mass.1.751024 molecules NH3 x (42.357 u NH3)/(1 molecule NH3) = 74.168 u NH3
This value is 21,85 g.
Ammonia = NH3 and has a molar mass of 17.031 g/molmoles NH3 = 63.9 g x 1 mol/17.031 g = 3.752 molesmolecules NH3 = 3.752 moles x 6.02x10^23 molecules/mole = 2.259x10^24 moleculesEach molecule of NH3 has 4 atoms (1 N + 3 H), thus....number of atoms = 4 atoms/molecule x 2.259x10^24 molecules = 9.04x10^24 atoms (to 3 sig figs)
Ok, so I'm assuming that the chemical formula is written as - 3H2 + N2 ----> 2NH3 2.80 = moles of N2 17.03052 g/mol = Molar mass of NH3 (2.80 mol N2) x (2 NH3) / (1 N2) = 5.6 mol NH3 x (17.03052 g) / (1 mol NH3) = 95.4 g NH3
The molar mass of ammonia is 17,031 g.17,031 g NH3-------------------1 mol500 g NH3-------------------------xx= 500/17,031 = 29,36 moles