1 mole of nitrogen makes 3 of ammania so..
moles of ammonia=34/17=2 moles
as 1 mole of nitrogen makes 3 of ammania so..
2/3 x 2 x14 = 18.67 g
28 grams of Nitrogen is necessary to produce 34 grams of ammonia.
Ammonia contains about 82.35 % nitrogen by mass.
Ammonia-NH3 2N+3H2=2NH3 2moles of Nitrogen produced 2moles of Ammonia (2*14)g of Nitrogen produced (2*17)g of Ammonia 28g of Nitrogen produced 34g of Ammonia 34g of Ammonia is produced by 28g of Nitrogen 0.034kg of Ammonia is produced by 0.028kg of Nitrogen 91.3kg of Ammonia will be produced by 0.028*91.3/0.034 91.3kg of Ammonia will be produced by 75.19kg of Nitrogen FOR HYDROGEN: 3moles of H2 produces 2moles of NH3 (2*3)g H2 produces 2*17g NH3 6g hydrogen produces 34g ammonia 0.006kg hydrogen produces o.o34kg ammonia 91.3kg ammonia will be produced by 91.3*0.006/.034=16.11kg of Hydogen Therefore, 75.19kg of Nitrogen and 16.11kg of Hydrogen will produce 91.3kg of Ammonia
The equation for the formation of ammonia from nitrogen and hydrogen gases at standard temperature and pressure is N2 + 3 H2 -> 2 NH3. The gram molecular mass of ammonia is 17.03 and the gram molecular mass of divalent nitrogen is 28.0134. Therefore, designating the unknown mass of nitrogen needed as p, the proportion 660/p equals (2 X 17.03)/28.0134 is valid. This expression is algebraically equivalent to 660 = (34.06)p/28.0134, for which p = 543 grams, rounded to the justified number of significant digits, limited by the three significant digits specified by the given number 600.
yes
28 grams of Nitrogen is necessary to produce 34 grams of ammonia.
Ammonia contains about 82.35 % nitrogen by mass.
NH3 which is ammonia has the highest percentage by mass of nitrogen.
Ammonia-NH3 2N+3H2=2NH3 2moles of Nitrogen produced 2moles of Ammonia (2*14)g of Nitrogen produced (2*17)g of Ammonia 28g of Nitrogen produced 34g of Ammonia 34g of Ammonia is produced by 28g of Nitrogen 0.034kg of Ammonia is produced by 0.028kg of Nitrogen 91.3kg of Ammonia will be produced by 0.028*91.3/0.034 91.3kg of Ammonia will be produced by 75.19kg of Nitrogen FOR HYDROGEN: 3moles of H2 produces 2moles of NH3 (2*3)g H2 produces 2*17g NH3 6g hydrogen produces 34g ammonia 0.006kg hydrogen produces o.o34kg ammonia 91.3kg ammonia will be produced by 91.3*0.006/.034=16.11kg of Hydogen Therefore, 75.19kg of Nitrogen and 16.11kg of Hydrogen will produce 91.3kg of Ammonia
Molar mass of ammonia = (14.01 + 3.03) (Molar mass of nitrogen + 3 times molar mass of hydrogen, as chemical formula of ammonia is NH3). Molar mass= 17.04 Molar mass x moles = mass 17.04 x 3 = 51.12 Mass of 3 moles of ammonia is 51.12g.
The equation for the formation of ammonia from nitrogen and hydrogen gases at standard temperature and pressure is N2 + 3 H2 -> 2 NH3. The gram molecular mass of ammonia is 17.03 and the gram molecular mass of divalent nitrogen is 28.0134. Therefore, designating the unknown mass of nitrogen needed as p, the proportion 660/p equals (2 X 17.03)/28.0134 is valid. This expression is algebraically equivalent to 660 = (34.06)p/28.0134, for which p = 543 grams, rounded to the justified number of significant digits, limited by the three significant digits specified by the given number 600.
The gram molecular mass of ammonia is 17.03. The formula shows that only one atom of nitrogen is required for each mole of ammonia; 4.12 mol of diatomic nitrogen contains 8.24 mol of nitrogen atoms, and with excess H, all of this nitrogen can be converted to ammonia. Therefore, 8.24 mol of ammonia can be produced, and multiplying this number by17.03 yields a total mass of 140.3 grams of ammonia, to the justified number of significant digits.
Ammonia is a chemical compound. It does not "make" any mass.
it can be calculated using the formula percentage composition of N =Gram molecular mass of nitrogen in the compound/ Gram molecular mass of compound *100
The equation for the reaction is N2 + 3 H2 -> 2 NH3. The gram atomic mass of nitrogen is 14.0067, and the gram atomic mass of hydrogen is 1.00794. Therefore, the mass fraction of nitrogen in ammonia is 14.0067/[14.0067 + (3*)(1.00794)] or about 0.8225, and, since nitrogen and hydrogen are the only two elements present, the mass fraction of hydrogen is 1*- 0.8225 or about 0.1775. The mass fraction of nitrogen in the amounts of nitrogen and hydrogen specified is 44.5/(44.5 + 2.58) or about 0.945. Therefore, hydrogen is the limiting reactant in this mixture, and the mass of ammonia produced is 2.58/0.1775 or 14.5 grams, to the justified number of significant digits. ________________ *An exact integer.
First you need to find the atomic masses of each element involved in the compound NH3, and add them up to find the total molecular mass of ammonia.Nitrogen = 14.0 gramsHydrogen = 1.01 × 3 atoms = 3.03 grams----------------------------------------------------Ammonia = 17.03 gramsThen you take the mass of nitrogen in one molecule and divide it by the total mass to find the percent composition.14.0 grams Nitrogen ÷ 17.03 grams Ammonia = .822 = 82.2% nitrogen in ammoniaThen you simply need to take 82.2% of 7.5 grams to find how much nitrogen is in that particular amount.82.2% × 7.50 = 6.17 grams of nitrogen in 7.50 grams of ammonia
yes