To understand the relationship between Gibbs free energy and work. The decomposition of 65.9 g ammonium nitrate yields how many liters of dinitrogen monoxide at 2.65 atm and 303 k? 1 Answer. the decomposition reaction is one of the major chemical reaction which can be represented by the following chemical reaction, NH\[_{4}\]NO\[_{2}\] N\[_{2}\] + 2H\[_{2}\]0. Substitute the appropriate values into Equation \(\ref{Eq5}\) to obtain \(G^o\) for the reaction. The vapor pressure of water at 22*C is 21 tOrr: The ammonium nitrite formula can be represented as NH\[_{4}\]NO\[_{2}\]. Ammonia produced by the Haber process can be oxidized to nitric acid by the Ostwald process. Ammonium nitrate-based explosives were used in the Sterling Hall bombing in Madison, Wisconsin, 1970, the Oklahoma City bombing in 1995, the 2011 Delhi bombings, the 2011 bombing in Oslo, and the 2013 Hyderabad blasts. We should note, however, that very few reactions are actually carried out under standard conditions, and calculated values of \(G^o\) may not tell us whether a given reaction will occur spontaneously under nonstandard conditions. The decomposition products of emulsion explosives and of other composite explosives containing ammonium nitrate, such as ANFO, were investigated. Thermal decomposition of ammonium nitrate in supercritical water. rapidly heated ammonium nitrate and analyzed the intermediates by fast scan FTIR [ 9 ], Raman in connection to DSC . Contamination can reduce this to 20 atmospheres. Molten ammonium nitrate is very sensitive to shock and detonation, particularly if it becomes contaminated with incompatible materials such as combustibles, flammable liquids, acids, chlorates, chlorides, sulfur, metals, charcoal and sawdust. Ans: The most common use of the compound is its use in manufacturing explosives. [6] Accidental ammonium nitrate explosions have killed thousands of people since the early 20th century.[6]. A similar situation arises in the conversion of liquid egg white to a solid when an egg is boiled. Between 200oC and 290oC, the subsequent reaction has been shown to be ionic with formation of NO2 + rate-limiting [2]. At 25C, the standard enthalpy change (H) is 187.78 kJ/mol, and the absolute entropies of the products and reactants are: Given: balanced chemical equation, H and S for reactants and products, Asked for: spontaneity of reaction as written. The diluted aqueous solution has a tendency to undergo decomposition slowly as . The \(G^o\) of a reaction can be calculated from tabulated \(G^o_f\) values (Table T1) using the products minus reactants rule. Many countries are phasing out its use in consumer applications due to concerns over its potential for misuse. The chemical formula of ammonium nitrite is written as NH\[_{4}\]NO\[_{2}\]. This problem has been solved! "The chemistry behind the Beirut explosion", "Advances in phase stabilization techniques of AN using KDN and other chemical compounds for preparing green oxidizers", "Nutrient Content of Fertilizer Materials", "Afghan bomb makers shifting to new explosives for IEDs", "Sunlight and salt water join forces in electricity-free cooling system", Airbag Compound Has Vexed Takata for Years. This reaction takes place at a temperature of 60-70C [8]. Expert's Answer. \nonumber \]. Use the value of \(G^o\) to determine whether the reaction is spontaneous as written. For vaporizing 1 mol of water, \(H = 40,657; J\), so the process is highly endothermic. 2. . Because oxygen gas is an element in its standard state, Gf (O2) is zero. NH4NO3 = N2O + 2H2O. Solid ammonium nitrate decomposes on heating. There is a high probability of explosion at temperatures 60 to 70 \[^{0}\]C. The uses of ammonium nitrite are mentioned as follows. From the above reactions, we can conclude that the formation of nitrogen (I)oxide is seen in the thermal decomposition of ammonium nitrate and the interaction of hydroxylamine and nitrous acid. \[ \Delta S= \dfrac{q_{rev}}{T} \nonumber\], with the definition of \(\Delta H\) in terms of \(q_{rev}\), \[\Delta S_{\textrm{surr}}=-\dfrac{\Delta H_{\textrm{sys}}}{T} \label{Eq3}\], Thus the entropy change of the surroundings is related to the enthalpy change of the system. What about processes for which \(G 0\)? As you saw in Example \(\PageIndex{3}\), the reaction of nitrogen and hydrogen gas to produce ammonia is one in which H and S are both negative. Question #99889. The third method is the most widely used industrial method of preparation of the chemical compound. Copper iron oxide/graphene oxide was also prepared. We can also calculate the temperature at which liquid water is in equilibrium with water vapor. Find important definitions, questions, meanings, examples, exercises and tests below . The prills or granules may be further dried, cooled, and then coated to prevent caking. A To calculate \(G^o\) for the reaction using Equation \(\ref{Eq5}\), we must know the temperature as well as the values of S and H. Conference Luan, Li; Proesmans, P; Buelow, S. Thermal decomposition of neat NH{sub 4}NO{sub 3} has been the subject of many investigations over the past years. Thermal Decomposition of Ammonium Nitrate 11 0.2 C = min; sample mass 1.0 g (color figure availble online). If \(TS_{univ}\) is denoted by \(G\), then we have Equation \ref{23.4.2} which defines the Gibbs energy change for the process. If \(G > 0\), the process is not spontaneous as written but occurs spontaneously in the reverse direction. unfavorable) for the reaction as written. Short Answer. we would first like to get rid of \(S_{surr}\). Assume that \(H\) and \(S\) do not change between 25.0C and 750C and use these data: The effect of temperature on the spontaneity of a reaction, which is an important factor in the design of an experiment or an industrial process, depends on the sign and magnitude of both H and S. Consider the following possible states for two different types of molecules with some attractive force: There would appear to be greater entropy on the left (state 1) than on the right (state 2). Dining evaporation of an alkaline aqueous solution of the nitrate, decomposition led to gas evolution and a pressure explosion occurred. the following reaction: 2 Mg + O2 2 MgO H = - 1202 kJ mol-1. Stephen Lower, Professor Emeritus (Simon Fraser U.) For this reason, this work examines the accident that occurred in Escombreras valley (Cartagena, Spain) related to the decomposition of NPK 15-15-15 fertiliser, composed basically of monoammonium phosphate, ammonium nitrate and potassium chloride. Laboratory method receiving of nitrogen. Figure \(\PageIndex{1}\) shows how the \(H\) and \(TS\) terms vary with temperature for the vaporization of water. The potential for use of the material as an explosive has prompted regulatory measures. )%2FUnit_4%253A_Equilibrium_in_Chemical_Reactions%2F13%253A_Spontaneous_Processes_and_Thermodynamic_Equilibrium%2F13.7%253A_The_Gibbs_Free_Energy, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), denoted by \(G\), then we have Equation \ref{23.4.2} which defines the, 13.8: Carnot Cycle, Efficiency, and Entropy, Enthalpically vs. Entropically Driving Reactions, status page at https://status.libretexts.org. The precipitates filtered out. Unstable nature of ammonium nitrate , heat decomposition, but the decomposition reaction is more complex, different product temperature is different. Ammonium nitrate | NH4NO3 or H4N2O3 | CID 22985 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological . The negative value of \(G^o\) indicates that the reaction is spontaneous as written. The value of \(G\) for the vaporization of 1 mol of water at 110C, assuming that \(H\) and \(S\) do not change significantly with temperature, becomes, \[ \begin{align*} \Delta G_{110^\circ\textrm C} &=\Delta H-T\Delta S \\[4pt] &=\textrm{40,657 J}-[(\textrm{383.15 K})(\textrm{108.96 J/K})] \\[4pt] &=-\textrm{1,091 J} \end{align*}\]. The IUPAC name of the formula is azanium nitrite. [15] It is less concentrated than urea (46-0-0), giving ammonium nitrate a slight transportation disadvantage. Short Answer. Of N2 (ml) : 6.25, 13.65, 35.05. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. atm The third method is the most widely used industrial method of preparation of the chemical compound. Ammonium nitrite, [NH4]NO2, is the ammonium salt of nitrous acid. In this example, changing the temperature has a major effect on the thermodynamic spontaneity of the reaction. \\[4pt] &-\left \{ [\textrm{1 mol H}_2\times130.7\;\mathrm{J/(mol\cdot K)}]+[\textrm{1 mol O}_2\times 205.2\;\mathrm{J/(mol\cdot K)}] \right \} The energy required for vaporization offsets the increase in entropy of the system. \\[4pt] &=[\mathrm{1\;mol\;H_2O_2}\times109.6\;\mathrm{J/(mol\cdot K})] Prepared by AWWA with assistance from Economic and Engineering Services, Inc. 3 Nitrification 1.0 Introduction The goal of this document is to review existing literature, research and information on the What would be the change in pressure (in atm) in a sealed 10.0 L vessel due to the formation of N 2 gas when the ammonium nitrite in 1.60 L of 1.40 M NH 4 NO 2 decomposes at 25.0C? a nearby fire), the decomposition reactions are all exothermic thus they all contribute to heat generation, further melting the solid ammonium nitrate, and . The common representation used for the structural formula for ammonium nitrite is. The standard free energy of formation of a compound can be calculated from the standard enthalpy of formation (Hf) and the standard entropy of formation (Sf) using the definition of free energy: \[G^o_{f} =H^o_{f} TS^o_{f} \label{Eq6}\]. [18], It was once used, in combination with independently explosive "fuels" such as guanidine nitrate,[19][20] as a cheaper (but less stable) alternative to 5-aminotetrazole in the inflators of airbags manufactured by Takata Corporation, which were recalled as unsafe after killing 14 people. This inorganic compoundrelated article is a stub. Use those data to calculate the temperature at which this reaction changes from spontaneous to nonspontaneous. The thermal decomposition kinetics, energy release, self-reaction properties of adiabatic environments, and escaping gaseous products . A To calculate \(G^o\) for the reaction, we need to know H, S, and T. We are given H, and we know that T = 298.15 K. We can calculate S from the absolute molar entropy values provided using the products minus reactants rule: \[\begin{align*}\Delta S^\circ &=S^\circ(\mathrm{H_2O_2})-[S^\circ(\mathrm{O_2})+S^\circ(\mathrm{H_2})] Employees of those with licenses to deal with the substance are still required to be supervised by authorized personnel and are required to pass a security and national police check before a license may be granted. NH 2OH+HNO 2N 2O+2H 2O. The following data is for the decomposition of ammonium nitrite in aqueous solution. which expresses the entropy change of the universe in terms of thermodynamic properties of the system exclusively. The reaction is violent owing to its highly exothermic nature. In Example \(\PageIndex{3}\), we calculated that H is 91.8 kJ/mol of N2 and S is 198.1 J/K per mole of N2, corresponding to \(G^o\) = 32.7 kJ/mol of N2 at 25C. Because S and H for this reaction have the same sign, the sign of \(G^o\) depends on the relative magnitudes of the H and TS terms. It was found that the first step in emulsion decomposition is pyrolysis of the oil to form reactive . It is a white crystalline salt consisting of ions of ammonium and nitrate. Due to these bans, "Potassium chlorate the stuff that makes safety matches catch fire has surpassed fertilizer as the explosive of choice for insurgents. Blending ammonium nitrate with certain other fertilizers can lower the critical relative humidity.[30]. Supported metal catalysts for wet decomposition of ammonium nitrate were investigated in order to develop the catalysts, which can convert both ammonium ion and nitrate ion selectively to N 2 and H 2 O under mild conditions, and to investigate the possible reaction pathways for simultaneous decomposition of ammonium and nitrate. Calculate \(G^o\) for the reaction of isooctane with oxygen gas to give carbon dioxide and water. Below 373.15 K, \(G\) is positive, and water does not evaporate spontaneously. As an example of this second reaction, consider the decomposition of ammonium nitrite: NH4NO2 (aq) arrow N2(g) + 2H2O(l) What would be ; What chemical reaction is involved in the thermal decomposition of ammonium persulfate? The ammonium nitrite chemical formula is written as NH\[^{4}\]NO\[^{0}\]. It is also used as agricultural pesticides. In its pure form, the chemical compound decomposes very quickly to generate nitrogen and water, this decomposition takes place at room temperature. Thus \(G = 0\) at \(T = 373.15\, K\) and \(1\, atm\), which indicates that liquid water and water vapor are in equilibrium; this temperature is called the normal boiling point of water. In contrast, a mammalian liver cell is a relatively efficient machine and can use fuels such as glucose with an efficiency of 30%50%. Calculated values of \(G^o\) are extremely useful in predicting whether a reaction will occur spontaneously if the reactants and products are mixed under standard conditions. Ammonium nitrate was also used to destroy the Murrah Federal Building in Oklahoma City, Oklahoma, in 1995. \[\ce{2NO(g) + O2(g) <=>2NO2(g)} \nonumber\]. Instead, water vapor at a temperature less than 373.15 K and 1 atm will spontaneously and irreversibly condense to liquid water. Both neat AN and AN containing various contaminants are examined, however quantitative kinetics results are not encompassed.. While ammonium nitrate is stable at ambient temperature and pressure under many conditions, it may detonate from a strong initiation charge. Information about The following data are for the decomposition of ammonium nitrite in aqueous solution:The order of reaction is :a)Zerob)Onec)Twod)ThreeCorrect answer is option 'B'. Such reactions are predicted to be thermodynamically spontaneous at low temperatures but nonspontaneous at high temperatures. The thermal properties were studied using differential scanning calorimetry (DSC), and the evolved gas was analyzed using thermogravimetry with mass spectrometry and pressurized DSC coupled with mass spectrometry (TG-DTA-MS and PDSC-MS). Using standard free energies of formation to calculate the standard free energy of a reaction is analogous to calculating standard enthalpy changes from standard enthalpies of formation using the familiar products minus reactants rule: \[G^o_{rxn}=\sum mG^o_{f} (products) \sum n G^o_{f} (reactants) \label{Eq7a}\]. Solution for Write the rate law for the decomposition of ammonium nitrite into nitrogen gas and water using the following data. Hence, It is enthalpically driven. Explanation: NH 4 NO 2 N 2 + 2H 2 O. Since \(G < 0\), the vaporization of water is predicted to occur spontaneously and irreversibly at 110 C. To make this determination, we need to evaluate the kinetics of the reaction. However, it can be induced to decompose explosively by detonation. Ammonium nitrate was mined there until the HaberBosch process made it possible to synthesize nitrates from atmospheric nitrogen, thus rendering nitrate mining obsolete. Correct option: (b) One. The standard free-energy change (G) is the change in free energy when one substance or a set of substances in their standard states is converted to one or more other substances, also in their standard states. Is the reaction spontaneous as written? It can also be synthesized by oxidizing ammonia with ozone or hydrogen peroxide, or in a precipitation reaction of barium or lead nitrite with ammonium sulfate, or silver nitrite with ammonium chloride, or ammonium perchlorate with potassium nitrite. Using the products minus reactants rule, \[\begin{align*} \Delta G^\circ &=[8\Delta G^\circ_\textrm f(\mathrm{CO_2})+9\Delta G^\circ_\textrm f(\mathrm{H_2O})]-\left[1\Delta G^\circ_\textrm f(\mathrm{C_8H_{18}})+\dfrac{25}{2}\Delta G^\circ_\textrm f(\mathrm{O_2})\right] \\[4pt] &-\left [(\textrm{1 mol})(-353.2\textrm{ kJ/mol})+\left(\dfrac{25}{2}\;\textrm{mol}\right)(0 \textrm{ kJ/mol}) \right ] This is technically correct, but misleading because it disguises the important fact that \(S_{total}\), which this equation expresses in an indirect way, is the only criterion of spontaneous change. Ammonium nitrate can absorb enough moisture to liquefy. Click hereto get an answer to your question The following data are for the decomposition of ammonium nitrate in aqueous solution: Volume of N2 (cm^3) & 6.25 & 9.0 & 11.42 & 13.65 & 35.02 Time (min) & 10 & 15 & 20 & 25 & The order of reaction is: It is important to recognize that a positive value of \(G^o\) for a reaction does not mean that no products will form if the reactants in their standard states are mixed; it means only that at equilibrium the concentrations of the products will be less than the concentrations of the reactants. Over what range of temperatures is each of the following processes spontaneous? decomposition of ammonium nitrite to nitrogen and water: NH4NO2->N2+2H2O. NH4* (aq) + NO2 (aq) N28) + \\[4pt] T=\dfrac{\Delta H^\circ}{\Delta S^\circ}&=\dfrac{(-\textrm{91.8 kJ})(\textrm{1000 J/kJ})}{-\textrm{198.1 J/K}}=\textrm{463 K}\end{align*}\]. Use the data in Example \(\PageIndex{3}\) to calculate the temperature at which this reaction changes from spontaneous to nonspontaneous, assuming that H and S are independent of temperature. 13: Spontaneous Processes and Thermodynamic Equilibrium, Unit 4: Equilibrium in Chemical Reactions, { "13.1:_The_Nature_of_Spontaneous_Processes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.2:_Entropy_and_Spontaneity_-_A_Molecular_Statistical_Interpretation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.3:_Entropy_and_Heat_-_Experimental_Basis_of_the_Second_Law_of_Thermodynamics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.4:_Entropy_Changes_in_Reversible_Processes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.5:_Entropy_Changes_and_Spontaneity" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.6:_The_Third_Law_of_Thermodynamics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.7:_The_Gibbs_Free_Energy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.8:_Carnot_Cycle_Efficiency_and_Entropy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13.E:_Spontaneous_Processes_(Exercises)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "12:_Thermodynamic_Processes_and_Thermochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13:_Spontaneous_Processes_and_Thermodynamic_Equilibrium" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "14:_Chemical_Equilibrium" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "15:_AcidBase_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "16:_Solubility_and_Precipitation_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17:_Electrochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "showtoc:no", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FMap%253A_Principles_of_Modern_Chemistry_(Oxtoby_et_al. [16]:1 It is used in coal mining, quarrying, metal mining, and civil construction in undemanding applications where the advantages of ANFO's low cost, relative safety, and ease of use matter more than the benefits offered by conventional industrial explosives, such as water resistance, oxygen balance, high detonation velocity, and performance in small diameters. We have developed one such criterion, the change in entropy of the universe: if \(S_{univ} > 0\) for a process or a reaction, then the process will occur spontaneously as written. Ammonium nitrate has an LD50 of 2217mg/kg,[36] which for comparison is about two-thirds that of table salt. Explain your answer. The following data are for the decomposition of ammonium nitrite in aqueous solution. Nitrous oxide (N2O) can be produced by thermal decomposition of ammonium nitrate heat NH,NOs (s) N,O(g) + 2H, 0() What volume of NzO(g) collected over water at a total pressure of 94.0 KPa and 228C, can be produced from thermal decomposition of 4.54 g NHANOz? InChI=1S/NO3.H3N/c2-1(3)4;/h;1H3/q-1;/p+1, Except where otherwise noted, data are given for materials in their, Production, reactions and crystalline phases, Ammonium Nitrate-Regulating its use, Balancing Access & Protection from, King Abdullah University of Science and Technology, largest artificial non-nuclear explosions, "Hazard Rating Information for NFPA Fire Diamonds", "Ammonium nitrate production by country, 2019 - knoema.com". Those data to calculate the temperature at which liquid water the reaction of isooctane with oxygen gas to carbon., different product temperature is different a temperature less than 373.15 K, \ ( >. 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And of other composite explosives containing ammonium nitrate with certain other fertilizers can Lower the critical humidity.... [ 6 ] Accidental ammonium nitrate yields how many liters of dinitrogen monoxide at atm.