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What is the limiting reactant when 3.14g of nitrogen react with 2.79g of hydrogen to produce ammonia and how many grams of ammonia are produce?
To determine the limiting reactant, we need to find the moles of each reactant. Then, we calculate the amount of ammonia that can be produced from each reactant. Whichever reactant produces the least amount of ammonia is the limiting reactant. Finally, we calculate the grams of ammonia produced based on the limiting reactant.
Calculate the amount of ammonia produced from 50g of N in the equation N2+3H2=2NH3?
In the equation N2+3H2=2NH3, the amount of ammonia produced from 50g of N would be 16.667g.
If an excess of nitrogen is reacted with 3.41 grams of hydrogen how many grams of ammonia can be produced?
Balanced equation first. N2 + 3H2 >> 2NH3 (hydrogen is limiting and drives the reaction ) 3.41 grams H2 (1mol/2.016g )(2mol NH3/3mol H2 )(17.034g NH3/1mol NH3 ) = 19.2 grams of ammonia produced ( this is called the Born-Haber process )
Do nitrogen fixing Bactria reduce the amount of nitrogen in the atmosphere?
Nitrogen-fixing bacteria do reduce the amount of nitrogen in the atmosphere by converting N2 into ammonia.
If you reacted 88.9 grams of ammonia with excess oxygen?
The reaction between ammonia and oxygen will form nitrogen dioxide and water as products. Balancing the equation reveals that 4 moles of NH3 react with 7 moles of O2. To determine the amount of N2O4 produced, you will need to calculate the limiting reactant first.
If you start with twenty eight grams of nitrogen and six grams of hydrogen what is the mass of ammonia formed?
The formula for ammonia is NH3. To find the mass of ammonia formed, you would need to calculate the molar mass of NH3 (14.01 g/mol for nitrogen and 1.01 g/mol for hydrogen) and then use the molar ratio to determine the amount of ammonia produced from the given amounts of nitrogen and hydrogen.
What mass of ammonia NH3 could be produced from the reaction of 44.5 g of nitrogen N2 and 2.58 g of hydrogen H2?
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.
What is the limiting reactant when 3.41 g of nitrogen react with 2.79g of hydrogen to produce ammonia and how many grams of ammonia are produced?
The reaction for the Haber process isN2 + 3 H2 ⇌ 2 NH3Amount of N2 = 3.41/28.0 = 0.122molAmount of H2 = 2.79/2.0 = 1.40molAccording to the stoichiometry of the reaction, 1 mol of N2 reacts with 3 mol of H2. 0.122mol of N2 will therefore react with only 0.366mol of H2, but there is 1.40mol of H2 available. Thus H2 is in excess and N2 is the limiting reactant.1mol of N2 reacts to form 2 mol of NH3.Under the maximum possible yield, 0.122mol of N2 reacts to form 0.244mol of NH3.Mass of NH3 = 0.244 x 17.0 = 4.15g
Kjeldahl method for estimation of nitrogen in inorganic organic compound?
This is a very convenient method but its use is restricted.This method is suitable for estimating nitrogen in those organic compounds in which nitrogen is linked to carbon and hydrogen. The method is not used in the case of nitro, azo and azoxy compounds. The method is extensively used for estimated nitrogen in food, fertilizers and agricultural products.Principle:- the method is based on the fact that when the nitrogenous compound is heated with concentrated sulphuric acid in presence of copper sulphate, the nitrogen present in the compound is quantitatively converted to ammonium sulphate. The ammonium sulphate so formed is decomposed with excess of alkali and the ammonia evolved is estimated volumetrically. The percentage of nitrogen is then calculated from the amount of ammonia.
The decomposition of 10 g ammonia produces hydrogen and nitrogen gases and releases 6300 cal of energy.How much energy is required to form 10g of ammonia from a mixture of hydrogen and nitrogen gases?
The decomposition of 10g of ammonia releases 6300 cal of energy. To form 10g of ammonia from hydrogen and nitrogen gases would require the same amount of energy, 6300 cal, but in the reverse process.
A sentence with the word ammonia in it?
It seemed also particularly desirable to ascertain whether ammonia was absorbed, as a small amount is contained in rain-water.
What maximum amount of ammonia in kilograms can be synthesized from 5.22 kg of H2 and 31.5 kg of N2?
Based on the balanced chemical equation for the synthesis of ammonia (NH3) from hydrogen (H2) and nitrogen (N2), the molar ratio between H2 and NH3 is 3:2. Knowing that 1 mole of NH3 is approximately 17 grams, you can calculate the maximum amount of NH3 that can be synthesized from the given amounts of H2 and N2. The answer turns out to be approximately 35.25 kg of ammonia that can be synthesized.
