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When 28 g of nitrogen and 6 g of hydrogen react 34 g of ammonia are produced. If 80 g of nitrogen react with 4 g of hydrogen how much ammonia will be produced?
Using the law of multiple proportions, we can see that the ratio of nitrogen to hydrogen in ammonia is 28:6 = 4.67:1. Therefore, for 80 g of nitrogen, 80/4.67 = 17.12 g of hydrogen would be needed to react completely. Since only 4 g of hydrogen is available, the limiting reactant is hydrogen and only 6 g of ammonia will be produced.
The reaction of hydrogen with nitrogen to produce ammonia is shown below. If there are 3 moles of nitrogen how many moles of hydrogen are needed to react completely with the nitrogen?
The balanced equation for the reaction is: 3H2 + N2 -> 2NH3 From the balanced equation, we can see that 3 moles of hydrogen are needed to react completely with 1 mole of nitrogen. So if there are 3 moles of nitrogen, you would need 9 moles of hydrogen to react completely.
What are three ways for nitrogen to be fixed?
Biological nitrogen fixation: Certain bacteria, like rhizobia, can convert inert atmospheric nitrogen into ammonium. Industrial nitrogen fixation: The Haber-Bosch process takes atmospheric nitrogen and hydrogen to produce ammonia for fertilizers. Lightning: Nitrogen fixation can also occur through lightning strikes, which provide the energy needed to convert nitrogen gas into reactive nitrogen compounds.
How many hydrogen molecules are needed to produce 525 grams of ammonia?
To produce 525 grams of ammonia (NH3), you would need 25 moles of ammonia. Since the balanced chemical equation for the reaction between hydrogen and nitrogen to form ammonia is 3H2 + N2 -> 2NH3, you would need 75 moles of hydrogen molecules (H2) to produce 525 grams of ammonia. This is equivalent to 4,500 molecules of hydrogen.
What organism is needed to turn nitrogen into a usable form?
Nitrogen-fixing bacteria, such as Rhizobium and Azotobacter, are needed to convert atmospheric nitrogen into a usable form like ammonia that plants can absorb. These bacteria form symbiotic relationships with plants or live freely in the soil.
What element is needed to create ammonia?
Nitrogen and Hydrogen.
How many moles of nitrogen and hydrogen are needed to get 10 moles of ammonia?
The reaction of nitrogen with hydrogen to form ammonia is: N2 +3H2 = 2NH3 Therefore to make 10 moles of ammonia you need 5 moles N2 and 15 moles H2
What mass of nitrogen and hydrogen needed to produce 91.3 Kg of ammonia?
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
How many hydrogen atoms would be needed to bond with one nitrogen atom to stabilize all atoms?
Three hydrogen atoms would be needed to bond with one nitrogen atom and the name of this molecule is ammonia.
Why pure nitrogen and pure hydrogen are used in haber's process?
Pure nitrogen and pure hydrogen are used in Haber's process because they are the starting materials needed to produce ammonia. Nitrogen is the main component in the atmosphere, and hydrogen is readily available through various industrial processes. By using pure nitrogen and pure hydrogen, the reaction conditions can be controlled to optimize the production of ammonia.
When 28 g of nitrogen and 6 g of hydrogen react 34 g of ammonia are produced. If 80 g of nitrogen react with 4 g of hydrogen how much ammonia will be produced?
Using the law of multiple proportions, we can see that the ratio of nitrogen to hydrogen in ammonia is 28:6 = 4.67:1. Therefore, for 80 g of nitrogen, 80/4.67 = 17.12 g of hydrogen would be needed to react completely. Since only 4 g of hydrogen is available, the limiting reactant is hydrogen and only 6 g of ammonia will be produced.
The reaction of hydrogen with nitrogen to produce ammonia is shown below. If there are 3 moles of nitrogen how many moles of hydrogen are needed to react completely with the nitrogen?
The balanced equation for the reaction is: 3H2 + N2 -> 2NH3 From the balanced equation, we can see that 3 moles of hydrogen are needed to react completely with 1 mole of nitrogen. So if there are 3 moles of nitrogen, you would need 9 moles of hydrogen to react completely.
What are three ways for nitrogen to be fixed?
Biological nitrogen fixation: Certain bacteria, like rhizobia, can convert inert atmospheric nitrogen into ammonium. Industrial nitrogen fixation: The Haber-Bosch process takes atmospheric nitrogen and hydrogen to produce ammonia for fertilizers. Lightning: Nitrogen fixation can also occur through lightning strikes, which provide the energy needed to convert nitrogen gas into reactive nitrogen compounds.
How many hydrogen molecules are needed to produce 525 grams of ammonia?
To produce 525 grams of ammonia (NH3), you would need 25 moles of ammonia. Since the balanced chemical equation for the reaction between hydrogen and nitrogen to form ammonia is 3H2 + N2 -> 2NH3, you would need 75 moles of hydrogen molecules (H2) to produce 525 grams of ammonia. This is equivalent to 4,500 molecules of hydrogen.
What mass of nitrogen is needed to make 34 grams of ammonia?
To find the mass of nitrogen needed to make ammonia, first determine the molar mass of ammonia (NH3) which is 17 g/mol. Since there is one nitrogen atom in ammonia, the nitrogen mass is 14 g/mol. To make 34 grams of ammonia, you would need 14 grams of nitrogen.
How many grams of nitrogen are needed to produce 660 grams 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.
What organism is needed to turn nitrogen into a usable form?
Nitrogen-fixing bacteria, such as Rhizobium and Azotobacter, are needed to convert atmospheric nitrogen into a usable form like ammonia that plants can absorb. These bacteria form symbiotic relationships with plants or live freely in the soil.
