Ammonium nitrate is commonly used as an explosive. It decomposes by the following reaction:
NH4NO3 → N2O + 2H2O ∆ H= -37.0 kJ
Calculate the energy (kJ) released when 2.50 grams of ammonium
nitrate decomposes
Calculate the energy (kJ) released when 1.00 grams of water is formed by the reaction.
Ammonium nitrate is commonly used as an explosive. It decomposes by the following reaction: NH4NO3 →...
Ammonium nitrate decomposes to give dinitrogen monoxide and water as shown in the following reaction: NH4NO3 + NO + 2H2O If a 108 g sample of NH.NO, decomposes to give 23 g of NO(g), what percent of the original sample remains? Ammonium nitrate decomposes to give dinitrogen monoxide and water as shown in the following reaction: NH4NO3-N2O + 2H2O If a 108 g sample of NH.NO, decomposes to give 23 g of N2O(g), what percent of the original sample remains?
Ammonium nitrate has been used as a high explosive because it is unstable and decomposes into several gaseous substances. The rapid expansion of the gaseous substances produces the explosive force. NH4NO3(s) + N2(g) + O2(g) + H2O(9) Calculate the mass of each product gas if 84.6 g of ammonium nitrate reacts. g N₂ 802 gH,0
Ammonium nitrate, a common fertilizer, is used as an explosive in fireworks and by terrorists. It was the material used in the tragic explosion at the Oklahoma City federal building in 1995. How many liters of gas at 307°C and 1.00 atm are formed by the explosive decomposition of 65.8 kg of ammonium nitrate to nitrogen, oxygen, and water vapor? L gas
The decomposition of ammonium nitrate is first-order. NH4NO3 (aq) → N2O(g) + 2H2O(g) The rate constant of this reaction is 0.110 min-1. If the initial concentration of ammonium nitrate is 0.551 M, what is the concentration after 38.5 minutes?
The following thermochemical equation is for the reaction of ammonium nitrate(s) to form dinitrogen monoxide(g) and water(g) NH,NO3() N2O(g) + 2H2O(g) AH = -35.9 kJ How many grams of NH NO,(s) would have to react to produce 12.1 kJ of energy? grams The following thermochemical equation is for the reaction of hydrogen sulfide(g) with oxygen(g) to form water(g) and sulfur dioxide(g). 2H2S(g) + 302(g)—2H2O(g) + 2802(8) AH=-1.04x109 kJ When 9.64 grams of hydrogen sulfide(g) react with excess oxygen(g), -588.8 kJ...
When heated to 350 ∘C at 0.950 atm, ammonium nitrate decomposes to produce nitrogen, water, and oxygen gases: 2NH4NO3(s)→2N2(g)+4H2O(g)+O2(g) a)How many liters of water vapor are produced when 26.4 g of NH4NO3 decomposes? Express your answer with the appropriate units. b)How many grams of NH4NO3 are needed to produce 15.7 L of oxygen? Express your answer with the appropriate units.
A sample of solid NH4NO3 is placed in an empty container. It decomposes according to the following reaction: NH4NO3(s) ⇔ N2O(g) + 2H2O(g) At equilibrium, the total pressure in the container is 2.25 atm. Calculate Kp.
To give water and dinitrogen monoxide, 0.500g of ammonium nitrate decomposes. How much water is formed, in grams?
Enter your answer in the provided box. Repo Guid Ammonium nitrate, a common fertilizer, is used as an explosive in fireworks and by terrorists. It was the material used in the tragic explosion at the Oklahoma City federal building in 1995. How many liters of gas at 307°C and 1.00 atm are formed by the explosive decomposition of 75.9 kg of ammonium nitrate to nitrogen, oxygen, and water vapor? gas
The dissolution of ammonium nitrate is given by the reaction: NH4NO3 (s) ----> NH4+ (aq) + NO3- (aq) Assuming that the values of ΔH° and ΔS° do not change appreciably with temperature, calculate the ΔG° value for the reaction from the polyatomic ion data in standard thermodynamic property tables. ΔG°: -4.1 kJ Predict the lowest temperature at which the reaction is spontaneous. T= _____ degrees Celsius