![40. Calculate the percentage of nitrogen in ammonium nitrate, (NH4NO3). (N = 14, H = 1, 0 = 16) - Brainly.in 40. Calculate the percentage of nitrogen in ammonium nitrate, (NH4NO3). (N = 14, H = 1, 0 = 16) - Brainly.in](https://hi-static.z-dn.net/files/d3b/e8231d142773abc817ff358623354438.jpg)
40. Calculate the percentage of nitrogen in ammonium nitrate, (NH4NO3). (N = 14, H = 1, 0 = 16) - Brainly.in
![Calculate the percentage of nitrogen and oxygen in ammonium nitrate. (relative molecular mass of ammonium nitrate is 80, H=1, N=14, O=16.) - Zigya Calculate the percentage of nitrogen and oxygen in ammonium nitrate. (relative molecular mass of ammonium nitrate is 80, H=1, N=14, O=16.) - Zigya](https://www.zigya.com/application/zrc/images/qvar/ICHEN10108015.png)
Calculate the percentage of nitrogen and oxygen in ammonium nitrate. (relative molecular mass of ammonium nitrate is 80, H=1, N=14, O=16.) - Zigya
![SOLVED: The last step is to calculate the percent by mass of each element in ammonium nitrate (NH4NO3). The masses of the elements in one mole of the compound are: mass N = SOLVED: The last step is to calculate the percent by mass of each element in ammonium nitrate (NH4NO3). The masses of the elements in one mole of the compound are: mass N =](https://cdn.numerade.com/ask_previews/b61f7211-313b-4bfc-b918-e47cb1d3e3b2_large.jpg)
SOLVED: The last step is to calculate the percent by mass of each element in ammonium nitrate (NH4NO3). The masses of the elements in one mole of the compound are: mass N =
![SOLVED: Ammonium nitrate, NH4 NO3, is used as a nitrogen fertilizer and in explosives. What is the molar mass of NHA NO3 ? | Numerade SOLVED: Ammonium nitrate, NH4 NO3, is used as a nitrogen fertilizer and in explosives. What is the molar mass of NHA NO3 ? | Numerade](https://cdn.numerade.com/previews/8249599e-eaa4-4a52-9549-465ce9b19351_large.jpg)
SOLVED: Ammonium nitrate, NH4 NO3, is used as a nitrogen fertilizer and in explosives. What is the molar mass of NHA NO3 ? | Numerade
![PPT - Calculate the Mass of nitrogen gas produced from the decomposition of 1.25 g of Ammonium Nitrate PowerPoint Presentation - ID:2338772 PPT - Calculate the Mass of nitrogen gas produced from the decomposition of 1.25 g of Ammonium Nitrate PowerPoint Presentation - ID:2338772](https://cdn1.slideserve.com/2338772/calculate-the-mass-of-nitrogen-gas-produced-from-the-decomposition-of-1-25-g-of-ammonium-nitrate-n.jpg)
PPT - Calculate the Mass of nitrogen gas produced from the decomposition of 1.25 g of Ammonium Nitrate PowerPoint Presentation - ID:2338772
![An aqueous solution is to be prepared that will be 7.51% by mass ammonium nitrate. What mass of NH_4NO_3 and what mass of water will be needed to prepare 1.25 kg of An aqueous solution is to be prepared that will be 7.51% by mass ammonium nitrate. What mass of NH_4NO_3 and what mass of water will be needed to prepare 1.25 kg of](https://homework.study.com/cimages/videopreview/videopreview-full/5.76_101840.jpg)
An aqueous solution is to be prepared that will be 7.51% by mass ammonium nitrate. What mass of NH_4NO_3 and what mass of water will be needed to prepare 1.25 kg of
![Determine the percentage of oxygen in Ammonium nitrate [Relative molecular mass of ammonium nitrate is 80, O = 16] - Chemistry - Analytical Chemistry Uses of Ammonium Hydroxide and Sodium Hydroxide - 14439229 | Meritnation.com Determine the percentage of oxygen in Ammonium nitrate [Relative molecular mass of ammonium nitrate is 80, O = 16] - Chemistry - Analytical Chemistry Uses of Ammonium Hydroxide and Sodium Hydroxide - 14439229 | Meritnation.com](https://s3mn.mnimgs.com/img/shared/content_ck_images/ck_8dbf6cc00f3eb3e37314e6d8d70b3d39.png)
Determine the percentage of oxygen in Ammonium nitrate [Relative molecular mass of ammonium nitrate is 80, O = 16] - Chemistry - Analytical Chemistry Uses of Ammonium Hydroxide and Sodium Hydroxide - 14439229 | Meritnation.com
![If the molecular mass of the compound 'X' is found to be 108 g/mol, then its molecular formula is:C_{12}H_{16}N_{4}C_{6}H_{6}N_{2}C_{9}H_{12}N_{3}C_{6}H_{8}N_{2} If the molecular mass of the compound 'X' is found to be 108 g/mol, then its molecular formula is:C_{12}H_{16}N_{4}C_{6}H_{6}N_{2}C_{9}H_{12}N_{3}C_{6}H_{8}N_{2}](https://search-static.byjusweb.com/question-images/toppr_ext/questions/1397337_1246643_ans_dd2ef076d84c44e1a00dcf30ee19bea5.jpg)
If the molecular mass of the compound 'X' is found to be 108 g/mol, then its molecular formula is:C_{12}H_{16}N_{4}C_{6}H_{6}N_{2}C_{9}H_{12}N_{3}C_{6}H_{8}N_{2}
![OneClass: An aqueous solution of ammonium nitrate,NH4NO3 , contains 2.16 grams of ammonium nitrate an... OneClass: An aqueous solution of ammonium nitrate,NH4NO3 , contains 2.16 grams of ammonium nitrate an...](https://prealliance-textbook-qa.oneclass.com/qa_images/homework_help/question/qa_images/115/11563733.webp)
OneClass: An aqueous solution of ammonium nitrate,NH4NO3 , contains 2.16 grams of ammonium nitrate an...
Calculate the percentage of nitrogen and oxygen in ammonium nitrate. [Relative molecular mass of ammonium nitrate is 80, H = 1, N = 14, O = 16] - Sarthaks eConnect | Largest Online Education Community
![Fertilizers are added to the soil to improve crop yields. A farmer has a choice of two fertilizers, ammonium nitrate NH<sub>4</sub>NO<sub>3</sub> or diammonium hydrogen phosphate (NH<sub>4)2</sub>HPO<sub>4</sub>) (video) | Nitrogen and its Compounds Fertilizers are added to the soil to improve crop yields. A farmer has a choice of two fertilizers, ammonium nitrate NH<sub>4</sub>NO<sub>3</sub> or diammonium hydrogen phosphate (NH<sub>4)2</sub>HPO<sub>4</sub>) (video) | Nitrogen and its Compounds](https://www.kenyaplex.com/videolessons/uploads/q4532019845.png)
Fertilizers are added to the soil to improve crop yields. A farmer has a choice of two fertilizers, ammonium nitrate NH<sub>4</sub>NO<sub>3</sub> or diammonium hydrogen phosphate (NH<sub>4)2</sub>HPO<sub>4</sub>) (video) | Nitrogen and its Compounds
![OneClass: Ammonium nitrate has been used as a high explosive because it is very unstable and decompos... OneClass: Ammonium nitrate has been used as a high explosive because it is very unstable and decompos...](https://prealliance-textbook-qa.oneclass.com/qa_images/homework_help/question/qa_images/120/12076969.png)