Ammonium nitrate decomposes explosively upon heating according
to the following balanced equation:
2NH4NO3(s)→2N2(g)+O2(g)+4H2O(g)
Calculate the total volume of gas (at 122 ∘C and 730 mmHg ) produced by the complete decomposition of 1.37 kg of ammonium nitrate.
Ammonium nitrate decomposes explosively upon heating according to the following balanced equation: 2NH4NO3(s)→2N2(g)+O2(g)+4H2O(g) Calculate the total...
Ammonium nitrate decomposes explosively upon heating according to the following balanced equation: 2NH4NO3(s)→2N2(g)+O2(g)+4H2O(g) Calculate the total volume of gas (at 119 ∘C and 761 mmHg ) produced by the complete decomposition of 1.71 kg of ammonium nitrate.
12) Ammonium nitrate decomposes explosively upon heating according to the following balanced equation: 2NH4NO3(s)→2N2(g)+O2(g)+4H2O(g) Calculate the total volume of gas (at 127 ∘C and 733 mmHg ) produced by the complete decomposition of 1.54 kg of ammonium nitrate.
Ammonium nitrate can decompose explosively when heated according to the following equation: 2NH4NO3(s) → 2N2(g)+4H2O(g)+O2(g) How many liters of gas would be formed at 430 Celcius and 1.00 atm pressure from an explosion of 430 g of NH4NO3?
Ammonium carbonate decomposes upon heating according to the following balanced equation: (NH4)2CO3(s)→2NH3(g)+CO2(g)+H2O(g) Calculate the total volume of gas produced at 24.0 ∘C and 1.01 atm by the complete decomposition of 11.8 g of ammonium carbonate.
1 Review Ammonium nitrate can decompose explosively when heated according to the equation 2NH4NO3(s) +2 N2(g) + 4H2O(g) + O2(g) Part A How many liters of gas would be formed at 510 °C and 1.00 atm pressure by explosion of 585 g of NH4NO3? 10 AP R O 2 ? 1 Bass Submit Request Answer
Given the balanced equation 2NH4NO3(g) ⟶ 2N2(g) + O2(g) + 4H2O(g), if the rate of appearance of steam (H2O(g)) is 0.58 M/s, what is the rate of appearance of nitrogen? Group of answer choices 2.3 M/s 0.29 M/s 0.15 M/s 1.2 M/s
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) Part A How many liters of water vapor are produced when 25.7 g of NH4NO3 decomposes? Express your answer with the appropriate units. V = Part B How many grams of NH4NO3 are needed to produce 11.4 L of oxygen? Express your answer with the appropriate units. m = When solid CaCO3 is heated, it decomposes to give solid CaO and...
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.
Ammonium nitrite, NH4NO2, decomposes upon heating to form N2 gas according to the following balanced chemical equation. When a sample of NH4NO2 was decomposed in a test tube, 813.9 mL of N2 gas was collected over water at 47.64 °C and the total pressure was 765.9 torr. NH4NO2(s) → N2(g) + 2 H2O(l). How many grams of N2 were collected?
The balanced equation for the decomposition of ammonium nitrate is2 NH₄ NO₃(s) → 2 N₂(g)+O₂(g)+4 H₂ O(g)(a) Select the mole ratios that relate moles of each product to the reactant NH₄ NO₃.1 mol O₂/2 mol NH₄ NO₃ 4 mol H₂ O/2 mol NH₄ NO₃2 mol NH₄ NO₃/4 mol H₂ O 2 mol N₂/2 mol NH₄ NO₃2 mol NH4 NO₃/1 mol O₂ 2 mol NH₄ NO₃/2 mol N₂(b) How many moles of each product...