By continuing, I agree that I am at least 13 years old and have read and About 60% of total U.S. ammonia production The proportions of … Can you explain this answer? NITROGEN (FIXED)—AMMONIA (Data in thousand metric tons of contained nitrogen unless otherwise noted) Domestic Production and Use: Ammonia was produced by 16 companies at 35 plants in 16 States in the United States during 2019; 2 additional plants were idle for the entire year. Nitrogen reacts with hydrogen to produce ammonia: N 2 (g) + 3H 2 (g) → 2NH 3 (g) Calculate the volume of ammonia that can be produced from 150 cm 3 of hydrogen and an excess of nitrogen. Calculate the percentage of nitrogen and oxygen in ammonium nitrate. You can study other questions, MCQs, videos and tests for Class 9 on EduRev and even discuss your questions like Atoms And Molecules - Olympiad Level MCQ, Class 9 Science, RD Sharma Solutions for Class 9 Mathematics, English Grammar (Communicative) Interact In English- Class 9, Class 9 Physics, Chemistry & Biology Tips & Tricks. The commercial grade contains about 33.5 percent nitrogen, all of which is in forms utilizable by plants; it is the most common nitrogenous component of artificial fertilizers. The Kjeldahl method is used to determine the amount of nitrogen present in an unknown sample. The molar mass of ammonia is #"17.031 g/mol"#. (This figure also varies from plant to plant.) At each pass of the gases through the reactor, only about 15% of the nitrogen and hydrogen converts to ammonia. if 100N are 100 units of nitrogen (as an element), the content of N in NH4NO3 is 34% so if you divide 100 by 0.34 you obtain 294 which is the amount of fertilizer that will provide 100 units of N Cite Example Problem: 0.1688 g when analyzed by the Dumas method yield 31.7 mL of moist nitrogen measured at 14º C and 758 mm mercury pressure. The percentage of nitrogen in the food is: The percentage of nitrogen in the food is: A Molar mass (NH4)2SO4 = 132.14 g/mol 1mol (NH4)2SO4 contains 2 mol N Molar mass N = 14g/mol , Mass of 2 mol N = 28g %N in (NH4)2SO4 = 28g/ 132g * 100 = 21.2% In the Kjeldahl's method for estimation of nitrogen present in a soil sample, ammonia evolved from 0.75 g of sample neutralized 10 mL of 1 M H 2 SO 4. The percentage of nitrogen in the soil is (a) 37.33 (b) 45.33 (c) 35.33 (d) 43.33 It is highly unreactive in the atmosphere. Ammonia contains about 82.35 % nitrogen by mass. Ammonia nitrogen exists mainly as ammonium in the pH range of most natural waters, but the fraction of un-ionized ammonia increases at higher pH levels and temperatures. Nitrogen is necessary for all living things and must be converted into other compounds by micro-organisms in soil. Therefore, the fraction of un-ionized ammonia is … This discussion on The percentage of nitrogen in ammonia is given by the expression :-a)14 x 100/17b)(3/17 x 100)c)4x 100/34d)3/34 x 100Correct answer is option 'A'. What is the mass percentage of nitrogen in ammonia? Calculate the percentage by mass of nitrogen in the bag of fertilizer. Apart from being the largest Class 9 community, EduRev has the largest solved During estimation of nitrogen present in an organic compound by Kjeldahl's method, the ammonia evolved from 0. Question bank for Class 9. It can also be used as a measure of the health of water in natural bodies such as rivers or lakes, or in man made water reservoirs. However, mineral nitrogen in soil accounts for only 2 % of the nitrogen in soil. how much of that is nitrogen? Explain the effect of raising the temperature of exothermic equilibrium reaction. The ammonia, which is a weak base, can be neutralized with hydrochloric acid, as described by the equation. Percentage by mass of nitrogen = ( Mass of nitrogen atom / Mass of ammonia molecule ) x 100 = ( 14 / 17 ) x 100 = 82%. 5 g of the compound in Kjeldahl's estimation of nitrogen neutralized 1 0 mL of 1 M H 2 S O 4. . At higher pressures ammonia becomes a liquid, making it easier to transport and store. By continual recycling of the unreacted nitrogen and hydrogen, the overall conversion is about 98%. agree to the. The chemical formula for ammonia is #"NH"_3#. soon. At high temperatures nitrogen can form compounds with oxygen that are harmful to the environment. Show the covalent bonding in terms of electrons in their outer shell for a molecule of Carbon Dioxide. Draw the chemical structures of butane, butene and butyne. 82.24% percent composition of N and 17.76% percent composition of H. [Relative molecular mass of ammonium nitrate is 80, H = 1, N= 14, 0= 16], Can you explain this answer? Explaining the conditions. NH3(aq)+HCl(aq)----->NH4Cl(aq) If 46.0 mL of 0.150 M HCl(aq) is needed to neutralize all the NH3(g) from a 2.25-g sample of organic material, calculate the mass percentage of nitrogen in … community of Class 9. The percentage of nitrogen in the compound is : Excessive nitrogen deposition can lead to significant biodiversity loss through loss of plant species and changes in … Nitrogen in manure can be converted to ammonia through bacterial degradation, primarily the conversion of urinary urea to ammonia. Can you explain this answer? The percentage of nitrogen in ammonia is given by the expression :-a)14 x 100/17b)(3/17 x 100)c)4x 100/34d)3/34 x 100Correct answer is option 'A'. Approximately 60 to 80 percent of the nitrogen in urine is in the form of urea. Most forms of organic nitrogen cannot be taken up by plants, with the exception of some small organic molecules. Calculating the mass of 1 molecule of ammonia: Mass = ( Number of hydrogen atoms x Mass of hydrogen atom) + ( Number of nitrogen atoms x Mass of nitrogen atoms), Percentage by mass of nitrogen = ( Mass of nitrogen atom / Mass of ammonia molecule ) x 100 = ( 14 / 17 ) x 100 = 82%. | EduRev Class 9 Question is disucussed on EduRev Study Group by 126 Class 9 Students. Have a Free Meeting with one of our hand picked tutors from the UK’s top universities. EduRev is a knowledge-sharing community that depends on everyone being able to pitch in when they know something. over here on EduRev! Calculating percentage by mass. If the answer is not available please wait for a while and a community member will probably answer this The Questions and Dec 19,2020 - The percentage of nitrogen in ammonia is given by the expression :-a)14 x 100/17b)(3/17 x 100)c)4x 100/34d)3/34 x 100Correct answer is option 'A'. Can you explain this answer? One to one online tution can be a great way to brush up on your Chemistry knowledge. People are searching for an answer to this question. are solved by group of students and teacher of Class 9, which is also the largest student In contrast, plants can readily take up mineral forms of nitrogen, including nitrate and ammonia. chemistry Nitrogen Nitrogen (N 2) in the environment exists primarily in the earth’s atmosphere as a colorless, tasteless, and generally inert gas Air, by volume, is composed of about 78.08% nitrogen, with oxygen (O 2) following at about 20.95% Nitrogen is assimilated (absorbed/digested) and/or fixed from the air in … The determination of Kjeldahl nitrogen is made in foods and drinks, meat, feeds, cereals and forages for the calculation of the protein content. The percentage of nitrogen in ammonia is given by the expression :-. Classically, this method is used to estimate the protein content of food and the amount of nitrogen in soil samples. Nitrogen makes up 78 percent of the air. Ammonium nitrate, a salt of ammonia and nitric acid, used widely in fertilizers and explosives. Video-Given atomic masses and chemical formulas, find the mass % [mass percentage] Correct answer is option 'A'. Can someone give me some directions as to how to reach the answer for this problem: A 0.608g sample of fertilizer contained nitrogen as ammonium sulfate, (NH4)2 SO4(s)+2NaOH(aq)-->Na2SO4(aq)+ 2H2O(l)+2NH3(g) The ammonia was collected in 46.3 mL of 0.213 M . of nitrogen in a wide range of samples. Can you explain this answer? Total ammonia-nitrogen, (NH3 - N)t = 2.20 mg/L From APPENDIX II (Reference 1), the percent un-ionized ammonia at pH = 8.3 and T = 18.5oC is 6.63%. The percentage of hydrogen in ammonia is 17,75741 %. According to the guide, ammonia is a compound of nitrogen and hydrogen and at atmospheric pressure and normal temperatures is a colorless gas with a characteristic pungent smell. Urease, an enzyme produced by microorganisms in feces, reacts with urinary urea to form ammonia. is done on EduRev Study Group by Class 9 Students. A bag of fertilizer contains 500g of ammonium sulfate, $ \small \ce{(NH4)2 SO4}$, and 500g of potassium nitrate, $\small \ce{KNO3}$. Also the Kjeldahl method is used for the nitrogen determination in wastewaters, soils and other samples. 8,941 moles o ammonium sulphide - (NH4)2S - contain 250,4678 g of nitrogen or 41,11 % nitrogen. Fertilizers supply the essential elements, nitrogen, phosphorus and potassium for plant growth. Answers of The percentage of nitrogen in ammonia is given by the expression :-a)14 x 100/17b)(3/17 x 100)c)4x 100/34d)3/34 x 100Correct answer is option 'A'. Nitrogen deposition occurs in gaseous form close to the source (dry deposition) or through rainfall (wet deposition), often many miles from the original ammonia source. The molar mass of #"N"# is #"14.007 g/mol"#. What is … Ammoniacal nitrogen (NH 3-N) is a measure for the amount of ammonia, a toxic pollutant often found in landfill leachate and in waste products, such as sewage, liquid manure and other liquid organic waste products. 22.4 L of N 2 at STP weigh 28gof N 2 . Calculate the percentage of ammonia in a sample if 0.2115 g gave rise to 0.4693 g of platinum. Calculating the mass of 1 molecule of ammonia: Mass = ( Number of hydrogen atoms x Mass of hydrogen atom) + ( Number of nitrogen atoms x Mass of nitrogen atoms) Mass = ( 3 x 1 ) + ( 1 x 14) = 17. Calculation of percentage of nitrogen. The formula indicates that in each mole of #"NH"_3#, there is one mole of #"N"# atoms. the molar mass of nitrogen/molar mass of ammonia=14.01/17.034*100 (for percentage) so =about 82.2% nitrogen. 0.4693(1/(14+1+1+1))= 0.0276 ... Nitrogen trichloride can form in small amounts when public water supplies are disinfected with monochloramine, and at given levels it can irritate mucous membranes. 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