What volume of hydrogen is necessary to react with six liters of nitrogen to produce ammonia at STP?
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…
The balanced equation is- N(2) + 3H(2) ---> 2NH(3). There fore the ratio says that for one molecule of nitrogen, 2 molecules of ammonia is produced. Also Avogadros Law states that number of molecules of gas is directly proportional to volume occupied. Hence 260 mL of nitrogen is required. However you have not told what are other physical conditions like pressure and temperature. So we cannot find the number of moles.
No, but the bacteria and fungi doing the decomposition produce many gases including ammonia, carbon dioxide, hydrogen sulfide, and many worse smelling ones. A small portion ammonia, but most does not. Ammonia is a compound composed of nitrogen and hydrogen. When your body decomposes, much of the mass becomes carbon dioxide and water. Some if it goes into more complex compounds found in the organisms doing the decomposing.
How many liters of n2 gas at stp will be used to produce 8.16 liters of nh3 gas at stp are consumed?
How do you find liters of hydrogen and nitrogen gas required to produce 532 liters of ammonia using 3H2 g plus N2 g--- 2NH3 g?
Many processes in the body produce nitrogen-containing wasted-products. This nitrogen will sometimes form ammonia, which is poisonous to the body. In order to remove this poisonous ammonia from the body, ammonia is converted to urea which is non-toxic for the body, and more easily removed. This happens in the urea cycle. Thus urea is a way of disposing leftover waste-nitrogen from our nitrogen metabolism.
These bacteria, through the plant, receive elemental nitrogen from the air, and use it to produce ammonia (NH3). This process is called nitrogen fixation. The ammonia can then be converted in to oxides of nitrogen and nitrogen salts, such as nitrites and nitrates, which are used by the host plant and others as nutrients.
The plant source of Nitrogen is Nitrate. Plants acquire nitrate through the Nitrogen Cycle. Atmospheric Nitrogen is absorbed by Nitrogen-fixing bacteria. The bacteria produce Ammonia which becomes Nitrite. Nitrite becomes Nitrate, the usable form of Nitrogen for plants. Nitrate is assimilated and absorbed by plants. Plants produce amino acids and proteins that are consumed in the food chain. Whatever consumes the proteins and amino acids will eventually die and the decomposition produces ammonia which turns…
N2 + 3H2 -> 2NH3 The stoichiometric equation (or balanced equation) for the formation of ammonia from this we can read off the mole ratio between hydrogen and ammonia; 3M H2 needed to produce 2M NH3 times each by 9 (so the ratio remains the same and 18M NH3 is formed) 27M H2 needed to produce 18M NH3
One use is to form ammonia by catalytic reaction under heat and pressure with hydrogen. This is further used to form urea and other fertilizers. Ammonia is also used to produce nitric acid and nitrates which have many commercial uses such as explosives, fetilisers, and the production of compounds not even containing the original nitrogen such as Na2CO3 using the Ammonia Soda process. In the natural world, most nitrogen is fixed (converted from gas in…
The atomic mass of hydrogen is 1.008 and that of nitrogen is 14.007. Therefore, the ratio of the mass of hydrogen to the total mass of NH3 must be 3(1.008)/[14.007 + 3(1.008)] = 0.17756. The mass of hydrogen in the stated amount of ammonia must therefore be 14.59(0.17756) = 2.591 g, to the justified number of significant digits.
No. Ammonia is a naturally occuring chemical. It is just Hydrogen and Nitrogen combined together. It is essential to many organic reactions. A phobia is, by its very definition...an IRRATIONAL fear. Chemical plants, regardless of what they produce, can be dangerous places, but nobody will force you to go stand in the middle of one, nor will they force you to work there.
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 =…
It increases the yield. 3 moles of hydrogen react with one mole of nitrogen to produce two moles of ammonia. As there is a REDUCTION in molecules, there will be a reduction in pressure. This is alsos an equilibrium reaction. So by Le Chetalier's principle, if we increase pressure, the system will react to reduce the pressure again. This can be done by producing more ammonia - in other words, an increase in product yield.
The Haber process (also called the Haber-Bosch process) is the nitrogen fixation reaction of nitrogen gas and hydrogen gas over an enriched iron or ruthenium catalyst, which is used to produce ammonia. It's main use is in fertilizers, color compounds and N-polymers like nylon. N2 + 3H2 --> 2NH3 (exothermic)