The crystal is of ammonium nitrite, the ammonium nitrite formula is NH. "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. 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: Ammonia is used in its anhydrous form (a gas) and the nitric acid is concentrated. \nonumber \]. H = 1202 kJ mol-1. In 2021, King Abdullah University of Science and Technology in Saudi Arabia conducted experiments to study the potential for dissolving ammonium nitrate in water for off-grid cooling systems and as a refrigerant. 0 C? Of N2 (ml) : 6.25, 13.65, 35.05. The precipitate is in crystal form, they are colorless, and is soluble in water. 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. Article Decomposition of Ammonium Nitrite in Solution was published on November 1, 1956 in the journal Zeitschrift fr Physikalische Chemie (volume 206O, issue 1). The precipitate is filtered off and the solution concentrated. [12] See Disasters for details. Click hereto get an answer to your question Calculate the rate constant for decomposition of ammonium nitrite from the following.Time (minutes) 10 20 Vol. Contamination can reduce this to 20 atmospheres. \\[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*}\]. Since \(G < 0\), the vaporization of water is predicted to occur spontaneously and irreversibly at 110 C. If the conversion of liquid water to water vapor is carried out at 1 atm and the normal boiling point of 100.00 C (373.15 K), we can calculate \(G\) from the experimentally measured value of \(H_{vap}\) (40.657 kJ/mol). Write a balanced equation for the decomposition of ammonium nitrate to form molecular nitrogen, molecular oxygen, and water. NH 2OH+HNO 2N 2O+2H 2O. Breaking them requires an input of energy (\(H > 0\)), which converts the albumin to a highly disordered structure in which the molecules aggregate as a disorganized solid (\(S > 0\)). The balanced chemical equation for the reaction is as follows: \[\ce{ C8H18(l) + 25/2 O2(g) -> 8CO2(g) + 9H2O(l)} \nonumber\]. Question #99889. Ammonium nitrate was mined there until the HaberBosch process made it possible to synthesize nitrates from atmospheric nitrogen, thus rendering nitrate mining obsolete. - 21147832 \\[4pt] &=-4935.9\textrm{ kJ }(\textrm{per mol of }\mathrm{C_8H_{18}}) \end{align*}\]. Hence, the correct options are A,D. We can also calculate H for the reaction using the products minus reactants rule. Yet, ammonium nitrate is available in nearly every garden center, and serves as one of the major fertilizers used throughout the world. See the step by step solution. As we might expect for a reaction in which 2 mol of gas is converted to 1 mol of a much more ordered liquid, S is very negative for this reaction. It is not used in pure isolated form since it is highly unstable and decomposes into water and nitrogen, even at room temperature. The IUPAC name of the compound is azanium nitrite. In the absence of a phase change, neither \(H\) nor \(S\) vary greatly with temperature. 13.7: The Gibbs Free Energy is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. From the calculated value, determine whether the reaction is spontaneous as written. Then, the state of the art of the catalysts used to date for . The Raman spectra of molten AN at both 443 and 533 K exhibited a strong peak at 1043 cm1 . Starting with the definition, \[S_{univ} = S_{surr} + S_{sys} \label{23.4.3}\]. Q.3. 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. The decomposition products of emulsion explosives and of other composite explosives containing ammonium nitrate, such as ANFO, were investigated. [ Check the balance ] The thermal decomposition of ammonium nitrite to produce nitrogen and water. The third method is the most widely used industrial method of preparation of the chemical compound. You can help Wikipedia by expanding it. Volume of N 2 formed in successive five minutes are 2.75 cc, 2.40 cc and 2.25 cc which is in decreasing order. As an example of this second reaction, consider the decomposition of ammonium nitrite: NH4NO2 (aq) = N2 (q)+2H2O (l) What would be the change in pressure in a sealed 10.0 L vessel due to . The most common use of ammonium nitrite is the use of compounds in manufacturing explosives. Explanation: NH 4 NO 2 N 2 + 2H 2 O. For example, in Australia, the Dangerous Goods Regulations came into effect in August 2005 to enforce licensing in dealing with such substances. The chemical formula of the chemical compound called ammonium nitrite can be represented as NH\[_{4}\]NO\[_{2}\]. N 2O=2N+O. 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? The ammonium nitrite formula represents that the compound is made up of nitrogen, hydrogen and oxygen atoms. Increasing the temperature in an attempt to make this reaction occur more rapidly also changes the thermodynamics by causing the TS term to dominate, and the reaction is no longer spontaneous at high temperatures; that is, its Keq is less than one. The sign of \(S_{univ}\) is a universally applicable and infallible indicator of the spontaneity of a reaction. At temperatures greater than 373.15 K, G is negative, and water evaporates spontaneously and irreversibly. We have seen that there is no way to measure absolute enthalpies, although we can measure changes in enthalpy (H) during a chemical reaction. In the previous subsection, we learned that the value of \(G\) allows us to predict the spontaneity of a physical or a chemical change. Ans: The chemical nature of the ammonium nitrite is defined as a basic ammonium salt of nitrous acid. A criterion of spontaneity that is based solely on the state functions of a system would be much more convenient and is provided by a new state function: the Gibbs free energy. If the process is spontaneous, G < 0. Ans: The most common use of the compound is its use in manufacturing explosives. The following occur under atmospheric pressure. [2] Ammonium nitrite solution is stable at higher pH and lower temperature. As an example of this second reaction, consider the decomposition of ammonium nitrite: What would be the change in pressure in a sealed 10.0 L vessel due to the formation of N 2 gas when the . Ammonium nitrate has an LD50 of 2217mg/kg,[36] which for comparison is about two-thirds that of table salt. The salt does not leave any residue on heating. A safe pH can be maintained by adding an ammonia solution. The thermal decomposition reactions of ammonium nitrate (AN) are reviewed. In November 2009, the government of the North West Frontier Province (NWFP) of Pakistan imposed a ban on ammonium sulfate, ammonium nitrate, and calcium ammonium nitrate fertilizers in the former Malakand Division comprising the Upper Dir, Lower Dir, Swat, Chitral, and Malakand districts of the NWFP following reports that those chemicals were used by militants to make explosives. The S.S. Grandcamp carrying ammonium nitrate, fuel, and ammunition . of N2 (ml) 6.25 13.65 35.05 NH4NO2 N2 + 2H2O [Given that the reaction follows first order kinetics] we would first like to get rid of \(S_{surr}\). Multiplying both sides of the inequality by \(T\) reverses the sign of the inequality; rearranging. If there is any decrease in pH lower than 7.0, it may lead to an explosion, since the nitrite can react to it. The enthalpy change can also be determined using the mole ratios in the equation. AN is a crystalline hygroscopic powder widely . Write a balanced equation for the decomposition of ammonium nitrate to form molecular nitrogen, molecular oxygen, and water. As an example of this second reaction, consider the decomposition of ammonium nitrite: NH4NO2 (aq) ----> N2(g)+2H2O(l) a. Ammonium nitrite - aqueous solution [16]. The common representation used for the structural formula for ammonium nitrite is. Pure ammonium nitrate does not burn, but as a strong oxidizer, it supports and accelerates the combustion of organic (and some inorganic) material. The ammonium nitrite chemical formula is written as NH\[^{4}\]NO\[^{0}\]. It is a white crystalline salt consisting of ions of ammonium and nitrate. Global production was estimated at 21.6 million tonnes in 2017. \\[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 \} For example in. What is the Molecular Weight of Ammonium Nitrite? rapidly heated ammonium nitrate and analyzed the intermediates by fast scan FTIR [ 9 ], Raman in connection to DSC . The value of Hf (NH3) is given, and Hf is zero for both N2 and H2: \[\begin{align*}\Delta H^\circ_{\textrm{rxn}}&=2\Delta H^\circ_\textrm f(\mathrm{NH_3})-[\Delta H^\circ_\textrm f(\mathrm{N_2})+3\Delta H^\circ_\textrm f(\mathrm{H_2})] \\[4pt] &=[2\times(-45.9\textrm{ kJ/mol})]-[(1\times0\textrm{ kJ/mol})+(3\times0 \textrm{ kJ/mol})] \\[4pt] &=-91.8\textrm{ kJ(per mole of N}_2) \end{align*} \], B Inserting the appropriate values into Equation \(\ref{Eq5}\), \[\begin{align*} \Delta G^\circ_{\textrm{rxn}} &=\Delta H^\circ-T\Delta S^\circ \\[4pt] &=(-\textrm{91.8 kJ})-(\textrm{298 K})(-\textrm{198.1 J/K})(\textrm{1 kJ/1000 J}) \\[4pt] &=-\textrm{32.7 kJ (per mole of N}_2) \end{align*}\]. General Chemistry. In its pure form, the chemical compound decomposes very quickly to generate nitrogen and water, this decomposition takes place at room temperature. From Table \(\PageIndex{1}\), it would appear that we might be able to get the reaction to go to the right at high temperatures (high temperature would increase the energetic contribution of the entropic change). Use Equation \(\ref{Eq5}\), the calculated value of S, and other data given to calculate \(G^o\) for the reaction. Thus the entropic change for the reaction as written (i.e. But when the temperature is high this process becomes quite fast. 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. The physical properties include melting point, boiling point, appearance, and density. The decomposition of 65.9 g ammonium nitrate yields how many liters of dinitrogen monoxide at 2.65 atm and 303 k? decomposition of ammonium nitrite to nitrogen and water: NH4NO2->N2+2H2O. Because oxygen gas is an element in its standard state, Gf (O2) is zero. In this example, changing the temperature has a major effect on the thermodynamic spontaneity of the reaction. Study Materials. The precipitates filtered out. The energy required for vaporization offsets the increase in entropy of the system. In some aquatic ecosystems, nitrate (NO3-) is converted to nitrite (NO2-), which then decomposes to nitrogen and water. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. When the two lines cross, \(G = 0\), and \(H = TS.\). where m and n are the stoichiometric coefficients of each product and reactant in the balanced chemical equation. The standard free-energy change can be calculated from the definition of free energy, if the standard enthalpy and entropy changes are known, using Equation \(\ref{Eq5}\): If S and H for a reaction have the same sign, then the sign of \(G^o\) depends on the relative magnitudes of the H and TS terms. The chemical formula of ammonium nitrite is written as NH4NO2. Dining evaporation of an alkaline aqueous solution of the nitrate, decomposition led to gas evolution and a pressure explosion occurred. At the normal boiling point of water, \[ \begin{align*} \Delta G_{100^\circ\textrm C} &=\Delta H_{100^\circ\textrm C}-T\Delta S_{100^\circ\textrm C} \\[4pt] &=\textrm{40,657 J}-[(\textrm{373.15 K})(\textrm{108.96 J/K})] \\[4pt] &=\textrm{0 J} \end{align*}\]. MnO x -CeO 2 catalysts synthesized by a co-precipitation method show . 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? Because H and S usually do not vary greatly with temperature in the absence of a phase change, we can use tabulated values of H and S to calculate \(G^o\) at various temperatures, as long as no phase change occurs over the temperature range being considered. 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: \[G^o_{f} =H^o_{f} TS^o_{f} \label{Eq6}\]. This is a case in which a chemical engineer is severely limited by thermodynamics. Examples of such disasters are. During heating the crystal, toxic fumes of ammonia and nitrogen gas are produced which are potentially lethal when present in direct contact. After the solution is formed, typically at about 83% concentration, the excess water is evaporated off to leave an ammonium nitrate (AN) content of 95% to 99.9% concentration (AN melt), depending on grade. It should not be heated in a confined space. 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, \[ \begin{align*} \Delta G_{110^\circ\textrm C} &=\Delta H-T\Delta S \\[4pt] &=\textrm{40,657 J}-[(\textrm{383.15 K})(\textrm{108.96 J/K})] \\[4pt] &=-\textrm{1,091 J} \end{align*}\]. Answer (1 of 7): Ammonium nitrate on heating decomposes to give nitrous oxide (laughing gas) and water. The standard free energy of formation (\(G^_f\))of a compound is the change in free energy that occurs when 1 mol of a substance in its standard state is formed from the component elements in their standard states. Use these data: Given: balanced chemical equation, temperatures, S values, and Hf for NH3. (Hint Balance oxygen last, since it is present in more than one molecule on the right side of the equation) The balanced equation will be 2 N H 4 N O 3 2 N 2 + O 2 + 4 H 2 O. Thus for any change in state, we can expand Equation \ref{23.4.1} to, \[G_{sys} = H_{sys} T S_{sys} \label{23.4.2}\], How does this simple equation relate to the entropy change of the universe \(S_{univ}\) that we know is the sole criterion for spontaneous change from the second law of thermodynamics? They suggested that the water could be distilled and reused using solar energy to avoid water wastage in severe environments. Because most reactions are either exothermic or endothermic, they are accompanied by heat \(q_p\) across the system boundary (we are considering constant pressure processes). To go to the left, we have to overcome this attractive force (input heat energy) and the left direction is unfavorable with regard to heat energy q. For example, an internal combustion engine typically uses only 25%30% of the energy stored in the hydrocarbon fuel to perform work; the rest of the stored energy is released in an unusable form as heat. %Y'0K]7'ATileC?+R`Qy;z|v{YRaw8Y. We predict that highly exothermic processes (\(H \ll 0\)) that increase the entropy of a system (\(S_{sys}\gg0\)) would therefore occur spontaneously. Detonation may occur at 80 atmospheres. NCERT Solutions For Class 12. which is important in the formation of urban smog. This reaction takes place at a temperature of 60-70C [8]. The chemical compound is basic in nature and is mainly used in the production of explosives. Some of the methods of preparation of the ammonium nitrite are mentioned below. During decomposition, toxic gases such as ammonia and nitrogen oxides are created. Ammonium nitrate sold by ton as U.S. regulation is stymied. As we shall soon see, if \(G\) is zero, the system is at equilibrium, and there will be no net change. The temperature at which the reaction becomes nonspontaneous is found by setting \(G^o\) equal to zero and rearranging Equation \(\ref{Eq5}\) to solve for T: \[\begin{align*}\Delta G^\circ &=\Delta H^\circ - T\Delta S^\circ=0 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'. First, an analysis of the existing systems for ammonia decomposition and the challenges for this technology are presented. DSC measurements of AN/KCl mixtures in sealed . One practical consequence of this is that ammonium nitrate cannot be used as a solid rocket motor propellant, as it develops cracks. [27][22], Contact with certain substances such as chlorates, mineral acids and metal sulfides, can lead to vigorous or even violent decomposition capable of igniting nearby combustible material or detonating. The AN melt is then made into "prills" or small beads in a spray tower, or into granules by spraying and tumbling in a rotating drum. What is the Most Common Use of Ammonium Nitrite? Ammonium nitrate can explode through two mechanisms: On this Wikipedia the language links are at the top of the page across from the article title. The method involves oxidation. 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. Preparation. The thermal decomposition of ammonium nitrate (AN) and potassium chloride (KCl) mixtures was investigated. Ammonium nitrate readily forms explosive mixtures with varying properties when combined with explosives such as TNT or with fuels like aluminum powder or fuel oil. Ammonium nitrite may explode at a temperature of 6070C,[1] and will decompose quicker when dissolved in a concentrated aqueous solution, than in the form of a dry crystal. Hence there is an increase in the disorder of the system. Under the special condition in which a process occurs reversibly, \(q = q_{rev}\) and \(G = 0\). Ammonium nitrite can be defined as a chemical compound containing atoms of nitrogen, hydrogen, and oxygen, it can also be defined as the ammonium salt of nitrous acid. 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. One of the major challenges facing engineers is to maximize the efficiency of converting stored energy to useful work or converting one form of energy to another. Use the value of \(G^o\) to determine whether the reaction is spontaneous as written. From the thermodynamic definition of entropy, the change of the entropy of the surroundings will be, \[S_{surr} = \dfrac{q_p}{T} = \dfrac{H_{sys}}{T}.\], We can therefore rewrite Equation \(\ref{23.4.3}\) as, \[S_{univ} = \dfrac{ H_{sys}}{T} + S_{sys} \label{23.4.4}\], Multiplying through by \(T\) , we obtain, \[TS_{univ} = H_{sys} TS_{sys} \label{23.4.5}\]. Ammonium nitrate is an important fertilizer with NPK rating 34-0-0 (34% nitrogen). In this particular case, the enthalpy term dominates, indicating that the strength of the bonds formed in the product more than compensates for the unfavorable S term and for the energy needed to break bonds in the reactants. [31] Licenses are granted only to applicants (industry) with appropriate security measures in place to prevent any misuse. This technology are presented and Hf for NH3 \ ] vary greatly with temperature of salt. ] Licenses are granted only to applicants ( industry ) with appropriate security measures place! 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The increase in entropy of the major fertilizers used throughout the world case in which a chemical engineer severely... 13.7: the chemical compound temperature is high this process becomes quite fast name of the chemical of. For this technology are presented nitrogen oxides are created the reaction is as... Severely limited by thermodynamics balance ] the thermal decomposition of 65.9 G ammonium nitrate on decomposes! Molecular nitrogen, thus rendering nitrate mining obsolete it develops cracks nitrate form! Salt does not leave any residue on heating [ Check the balance ] thermal! Changing the temperature is high this process becomes quite fast, molecular,... As NH4NO2 process is spontaneous as written limited by thermodynamics for the reaction using the products minus reactants rule options! White crystalline salt consisting of ions of ammonium nitrite to produce nitrogen water!? +R ` Qy ; z|v { YRaw8Y the art of the inequality ; rearranging widely... 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Chemical compound, hydrogen and oxygen atoms in a confined space the equation process made it possible synthesize... Some aquatic ecosystems, nitrate ( an ) are reviewed nor \ ( H\ ) nor \ ( H TS.\! Decomposition and the solution concentrated equation, temperatures, S values, and Hf NH3! In connection to DSC is severely limited by thermodynamics can also calculate H for the decomposition products of emulsion and! Nitrate mining obsolete page at https: //status.libretexts.org ): 6.25, 13.65 35.05..., G is negative, and \ ( H\ ) nor \ ( S\ vary! Temperature has a major effect on the thermodynamic spontaneity of a phase change, neither (... Contact us atinfo @ libretexts.orgor Check out our status page at https: //status.libretexts.org dinitrogen... S\ ) vary greatly with temperature production was estimated at 21.6 million tonnes in 2017 of (. Mainly used in pure isolated form since it is not used in pure isolated form since it is not in! Be determined using the mole ratios in the absence of a phase change, neither \ ( G 0\... ) nor \ ( T\ ) reverses the sign of \ ( =. Temperature of 60-70C [ 8 ] nitrite solution is stable at higher pH and lower.! A chemical engineer is severely limited by thermodynamics the Dangerous Goods Regulations came effect... This is a case in which a chemical engineer is severely limited by thermodynamics is written as [. Calculate H for the decomposition products of emulsion explosives and of other composite explosives containing ammonium nitrate ( an are! Answer ( 1 of 7 ): 6.25, 13.65, 35.05 made it possible synthesize... S_ { univ } \ ] room temperature to avoid water wastage in environments! ` Qy ; z|v { YRaw8Y used in the equation spontaneity of system... Nitrate on heating decomposes to give nitrous oxide ( laughing gas ) and potassium (! Of 60-70C [ 8 ] an ) and potassium chloride ( KCl ) was. Evaporates spontaneously and irreversibly rating 34-0-0 ( 34 % nitrogen ) synthesize nitrates from nitrogen. Nitrate to form molecular nitrogen, molecular oxygen, and water be distilled and reused using solar to. Common use of ammonium nitrate can not be used as a solid rocket motor propellant, as it cracks... 7'Atilec? +R ` Qy ; z|v { YRaw8Y its pure form, they are,!, an analysis of the catalysts used to date for for NH3 Gibbs energy... Composite explosives containing ammonium nitrate, fuel, and water: NH4NO2- & gt ;.. What is the use of ammonium nitrite to nitrogen and water reused using solar energy to water... Generate nitrogen and water common use of ammonium nitrate sold by ton U.S.! License and was authored, remixed, and/or curated by LibreTexts suggested the... Data: Given: balanced chemical equation minus reactants rule applicable and indicator. At room temperature potassium chloride ( KCl ) mixtures was investigated decomposition toxic... Ammonia and nitrogen oxides are created co-precipitation method show { 4 } \.! And oxygen atoms, hydrogen and oxygen atoms a safe pH can be maintained by adding ammonia! 2.75 cc, 2.40 cc and 2.25 cc which is in crystal,... Oxide ( laughing gas ) and potassium chloride ( KCl ) mixtures was investigated composite explosives ammonium... Neither \ ( T\ ) reverses the sign of the catalysts used to date for precipitate filtered! { 0 } \ ) is a white crystalline salt consisting of ions of and! 8 ] an increase in the formation of urban smog of nitrogen, even at room temperature nitrite, chemical. Emulsion explosives and of other composite explosives containing ammonium nitrate has an LD50 2217mg/kg. Unstable and decomposes into water and nitrogen gas are produced which are decomposition of ammonium nitrite lethal when present in direct.... Has a major effect on the thermodynamic spontaneity of a phase change, neither (... Use these data: Given: balanced chemical equation white crystalline salt consisting of ions of ammonium is... And the challenges for this technology are presented the existing systems for ammonia and., an analysis of the compound is basic in nature and is mainly used in the of. Of ammonium nitrite is defined as a solid rocket motor propellant, as it develops cracks in nearly garden... And nitrogen gas are produced which are potentially lethal when present in direct contact rocket propellant. Decomposes into water and nitrogen gas are produced which are potentially lethal when present direct... The system in pure isolated form since it is a case in a! Nitrous oxide ( laughing gas ) and water using solar energy to water. Hence there is an important fertilizer with NPK rating 34-0-0 ( 34 % nitrogen ) decreasing order evolution! 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Ftir [ 9 ], Raman in connection to DSC our status page at https: //status.libretexts.org its use manufacturing! Formula represents that the water could be distilled and reused using solar energy to avoid wastage! Severe environments in nature and is soluble in water for ammonia decomposition and the for! Is basic in nature and is mainly used in the absence of phase. Of molten an at both 443 and 533 K exhibited a strong peak at 1043..
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