In Haber’s process, the equivalent weight of ammonia (NH3) is calculated based on its molar mass and the number of moles of hydrogen ions (H⁺) it can donate or accept. The molar mass of NH3 is approximately 17 g/mol. Since one mole of NH3 can donate one mole of H⁺, its equivalent weight is also 17 g. Thus, the equivalent weight of NH3 in the context of Haber’s process is 17 g/equiv.
The molarity of a 5% solution of NH3 in water depends on the density and molecular weight of NH3. Without this information, it is not possible to calculate the molarity.
The product in the Haber process is ammonia (NH3).
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
Relation of mols : N2 + 4H2 → 2NH4This means : 1 mol of molecular nitrogen will give you 2 mols of ammonia.Atomic weight : N; 14.0067, H; 1.00797Molecular weight : N2 ; 28.0134 g/mol, NH4; 18.03858 g/molFrom mol relation, the weight relation is: 28.0134 g of N2 give 36.00772 g of NH4So 35.0 g of N2 will give you: 36.00772 g x 35.0 g / 28.0134 g ~ 45.0 g of NH4
NH3 is Ammonia, which is not an acid.
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The densities of NH3 at variable temperatures are - At boiling point - 0.86 kg/m3 At 15 oC - 0.73 kg/m3 At -33 oC - 681.9 kg/m3 (liquid) At -80 oC - 817 kg/m3 (transparent solid)
2.49x10-1mol NH3Source: e2020
chloramine NH3 + HCl --> NH4Cl (ammonium chloride, son!)
The molarity of a 5% solution of NH3 in water depends on the density and molecular weight of NH3. Without this information, it is not possible to calculate the molarity.
The product in the Haber process is ammonia (NH3).
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
Yes, NH3 diffuses faster than HCl because NH3 has a lower molecular weight and faster average speed due to fewer collisions with surrounding molecules. Additionally, NH3's smaller size allows it to move through openings and travel longer distances more quickly than HCl.
Ammonia (NH3) is typically formed by the reaction of nitrogen gas (N2) and hydrogen gas (H2) in the presence of a catalyst under high pressure and temperature. This process, known as the Haber process, is the main industrial method for producing ammonia on a large scale.
The boiling point of a compound is influenced by its molecular weight and intermolecular forces. AsH3 has a lower boiling point than NH3 because it is a lighter molecule (lower molecular weight) and has weaker hydrogen bonding interactions between its molecules compared to NH3, which has stronger hydrogen bonding.
By balancing the chemical equation for the reaction N2 + 3H2 -> 2NH3, we can see that 1 mol of N2 produces 2 mol of NH3. Therefore, 2.23 mol of N2 will produce 2.23 x 2 = 4.46 mol of NH3. Since the molar mass of NH3 is approximately 17 g/mol, 4.46 mol of NH3 is equivalent to 4.46 x 17 = 75.82 grams of NH3.
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.