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The following equation represents one of the reactions contributing to the massive explosion: 4NH4NO3 (s)→ 3N₂ (g) + 2NO₂ (g) + 8 H₂O (g) Table 1. Standard Thermodynamic Properties¹ (from OpenStax, Chemistry 2e) Substance NH4NO3 (S) N₂ (g) NO₂ (g) H₂O (g) AH, (kJ mol-¹) -365.56 0 +33.2 -241.82 Sº (J K¹ mol ¹) +151.08 +191.6 +240.1 +188.8 Reaction 1 AG (kJ mol-¹) -183.87 0 51.30 -228.59 Once decomposition begins a 'runaway' reaction can occur. In a runaway reaction an exothermic reaction goes out of control. The heat evolved raises the temperature of the reacting mixture leading to an increase in reaction rate, which causes a further increase in temperature and a further increase in reaction rate until an explosion occurs. 1. Use the standard enthalpies of formation, AH to calculate the enthalpy change (in kJ mol¹) for the decomposition of ammonium nitration as shown as Reaction 1 and confirm that the reaction is exothermic.

The following equation represents one of the reactions contributing to the massive explosion: 4NH4NO3 (s)→ 3N₂ (g) + 2NO₂ (g) + 8 H₂O (g) Table 1. Standard Thermodynamic Properties¹ (from OpenStax, Chemistry 2e) Substance NH4NO3 (S) N₂ (g) NO₂ (g) H₂O (g) AH, (kJ mol-¹) -365.56 0 +33.2 -241.82 Sº (J K¹ mol ¹) +151.08 +191.6 +240.1 +188.8 Reaction 1 AG (kJ mol-¹) -183.87 0 51.30 -228.59 Once decomposition begins a 'runaway' reaction can occur. In a runaway reaction an exothermic reaction goes out of control. The heat evolved raises the temperature of the reacting mixture leading to an increase in reaction rate, which causes a further increase in temperature and a further increase in reaction rate until an explosion occurs. 1. Use the standard enthalpies of formation, AH to calculate the enthalpy change (in kJ mol¹) for the decomposition of ammonium nitration as shown as Reaction 1 and confirm that the reaction is exothermic.

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Part 1. What is a runaway reaction? "On Aug. 4, a devastating explosion struck the area around a port in Beirut. Lebanese officials are blaming the blast, which has killed over 100 people and left 300,000 homeless, on the common fertilizer compound ammonium nitrate (NH4NO3)." C&EN News, August 5, 2020 Pure ammonium nitrate does not explode easily and can be handled safety. It decomposes at 230°C to produce nitrous oxide gas (N₂O) and water vapor. However, above 260°C, if confined and when contaminated, ammonium nitrate will explode to form toxic gases such as nitrogen dioxide (NO₂). This is the gas that was responsible for the red-orange smoke plume and orange-brown fireball described by witnesses. The following equation represents one of the reactions contributing to the massive explosion: 4NH4NO3 (s)→ 3N₂ (g) + 2NO2 (g) + 8 H₂O (g) Table 1. Standard Thermodynamic Properties¹ (from OpenStax, Chemistry 2e) Substance AH (kJ mol-¹) -365.56 0 +33.2 -241.82 NH4NO3 (S) N₂ (g) NO₂ (g) H₂O (g) Sº (J K₁¹ mol-¹) +151.08 +191.6 +240.1 +188.8 Reaction 1 AG (kJ mol-¹) -183.87 0 51.30 -228.59 Once decomposition begins a 'runaway' reaction can occur. In a runaway reaction an exothermic reaction goes out of control. The heat evolved raises the temperature of the reacting mixture leading to an increase in reaction rate, which causes a further increase in temperature and a further increase in reaction rate until an explosion occurs. 1. Use the standard enthalpies of formation, AHf to calculate the enthalpy change (in kJ mol¹¹) for the decomposition of ammonium nitration as shown as Reaction 1 and confirm that the reaction is exothermic.
Transcribed Image Text:Part 1. What is a runaway reaction? "On Aug. 4, a devastating explosion struck the area around a port in Beirut. Lebanese officials are blaming the blast, which has killed over 100 people and left 300,000 homeless, on the common fertilizer compound ammonium nitrate (NH4NO3)." C&EN News, August 5, 2020 Pure ammonium nitrate does not explode easily and can be handled safety. It decomposes at 230°C to produce nitrous oxide gas (N₂O) and water vapor. However, above 260°C, if confined and when contaminated, ammonium nitrate will explode to form toxic gases such as nitrogen dioxide (NO₂). This is the gas that was responsible for the red-orange smoke plume and orange-brown fireball described by witnesses. The following equation represents one of the reactions contributing to the massive explosion: 4NH4NO3 (s)→ 3N₂ (g) + 2NO2 (g) + 8 H₂O (g) Table 1. Standard Thermodynamic Properties¹ (from OpenStax, Chemistry 2e) Substance AH (kJ mol-¹) -365.56 0 +33.2 -241.82 NH4NO3 (S) N₂ (g) NO₂ (g) H₂O (g) Sº (J K₁¹ mol-¹) +151.08 +191.6 +240.1 +188.8 Reaction 1 AG (kJ mol-¹) -183.87 0 51.30 -228.59 Once decomposition begins a 'runaway' reaction can occur. In a runaway reaction an exothermic reaction goes out of control. The heat evolved raises the temperature of the reacting mixture leading to an increase in reaction rate, which causes a further increase in temperature and a further increase in reaction rate until an explosion occurs. 1. Use the standard enthalpies of formation, AHf to calculate the enthalpy change (in kJ mol¹¹) for the decomposition of ammonium nitration as shown as Reaction 1 and confirm that the reaction is exothermic.
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