![]() Production, reactions and crystalline phases Ammonium nitrate was mined there until the Haber–Bosch process made it possible to synthesize nitrates from atmospheric nitrogen, thus rendering nitrate mining obsolete. Occurrence Īmmonium nitrate is found as the natural mineral gwihabaite (formerly known as nitrammite) – the ammonium analogue of saltpetre (mineralogical name: niter) – in the driest regions of the Atacama Desert in Chile, often as a crust on the ground or in conjunction with other nitrate, iodate, and halide minerals. By 2021, global production of ammonium nitrate was down to 16.7 million tonnes. Global production was estimated at 21.6 million tonnes in 2017. Accidental ammonium nitrate explosions have killed thousands of people since the early 20th century. Many countries are phasing out its use in consumer applications due to concerns over its potential for misuse. It is the major constituent of ANFO, a popular industrial explosive which accounts for 80% of explosives used in North America similar formulations have been used in improvised explosive devices. Its other major use is as a component of explosive mixtures used in mining, quarrying, and civil construction. It is predominantly used in agriculture as a high-nitrogen fertilizer. It is highly soluble in water and hygroscopic as a solid, although it does not form hydrates. It is a white crystalline salt consisting of ions of ammonium and nitrate. Ammonium nitrate is a chemical compound with the formula NH 4NO 3. Textbook content produced by OpenStax is licensed under a Creative Commons Attribution License. We recommend using aĪuthors: Paul Flowers, Klaus Theopold, Richard Langley, William R. Use the information below to generate a citation. Then you must include on every digital page view the following attribution: If you are redistributing all or part of this book in a digital format, Then you must include on every physical page the following attribution: If you are redistributing all or part of this book in a print format, Want to cite, share, or modify this book? This book uses the This book may not be used in the training of large language models or otherwise be ingested into large language models or generative AI offerings without OpenStax's permission. If the molecular (or molar) mass of the substance is known, it may be divided by the empirical formula mass to yield the number of empirical formula units per molecule ( n): As the name suggests, an empirical formula mass is the sum of the average atomic masses of all the atoms represented in an empirical formula. Molecular formulas are derived by comparing the compound’s molecular or molar mass to its empirical formula mass. ![]() Molar mass can be measured by a number of experimental methods, many of which will be introduced in later chapters of this text. Molecular mass, for example, is often derived from the mass spectrum of the compound (see discussion of this technique in the previous chapter on atoms and molecules). These quantities may be determined experimentally by various measurement techniques. Determining the absolute numbers of atoms that compose a single molecule of a covalent compound requires knowledge of both its empirical formula and its molecular mass or molar mass. ![]() Recall that empirical formulas are symbols representing the relative numbers of a compound’s elements. The percent composition of this compound could be represented as follows: For example, consider a gaseous compound composed solely of carbon and hydrogen. The results of these measurements permit the calculation of the compound’s percent composition, defined as the percentage by mass of each element in the compound. When a compound’s formula is unknown, measuring the mass of each of its constituent elements is often the first step in the process of determining the formula experimentally. The elemental makeup of a compound defines its chemical identity, and chemical formulas are the most succinct way of representing this elemental makeup. But what if the chemical formula of a substance is unknown? In this section, these same principles will be applied to derive the chemical formulas of unknown substances from experimental mass measurements. Given the chemical formula of the substance, one may determine the amount of the substance (moles) from its mass, and vice versa. ![]() The previous section discussed the relationship between the bulk mass of a substance and the number of atoms or molecules it contains (moles). Determine the molecular formula of a compound.Determine the empirical formula of a compound.Compute the percent composition of a compound.By the end of this section, you will be able to: ![]()
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