(Silberberg, Problem 4.108) Ammonium nitrate, a common fertilizer, is used as an explosive in fireworks and...

(Silberberg, Problem 4.108) Ammonium nitrate, a common fertilizer, is used as an explosive in fireworks and by terrorists. In 2006, the RCMP set up a sting operation in Toronto where they arrested 18 members of an alleged terrorist cell who had ordered three metric tonnes (1 tonne = 1000 kg) of ammonium nitrate. If this quantity of ammonium nitrate decomposes explosively to nitrogen, oxygen, and water vapour, calculate the partial pressures (in atm) of each gas formed.

Solutions

Expert Solution

The calculations of this question uploaded as images.

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

A common method to produce ammonium nitrate, an important agricultural fertilizer, is to combine ammonium sulfate,...

A common method to produce ammonium nitrate, an important agricultural fertilizer, is to combine ammonium sulfate, (NH4)2SO4, with sodium nitrate, NaNO3, as shown in the following balanced equation. (NH4)2SO4(s) + 2 NaNO3(s) → Na2SO4(s) + 2 NH4NO3(s) If 684.7 g (NH4)2SO4 is reacted with excess NaNO3 and produces 772.1 g NH4NO3, what is the percent yield?

Ammonium nitrate, NH4NO3, is used as a N fertilizer and has the potential to degrade water...

Ammonium nitrate, NH4NO3, is used as a N fertilizer and has the potential to degrade water quality due to its solubility. The US EPA mean contaminant level (MCL) for nitrate concentrations in drinking water is 10 mg NO3 L-1. First, calculate the Ksp for NH4NO3. Express your answer as a number rather than in a power of 10 (e.g., 100 instead of 10^2). The Ksp does not need units. Next, calculate the molarity of the equilbirum concentration of NO3. Units...

Ammonium nitrate (NH4NO3) is a high explosive because it is unstable and decomposes into several substances...

Ammonium nitrate (NH4NO3) is a high explosive because it is unstable and decomposes into several substances as follows: _NH4NO3--> _N2 + _O2 + _H2O. Balance the equation and then find the number of grams of each product if 42.54g of ammonium nitrate reacted.

What compound provides the explosive force in aerial fireworks?

Ammonium nitrate (NH4NO3(s) decomposes into nitrogen, oxygen and water. If 10 g of ammonium nitrate decompose...

Ammonium nitrate (NH4NO3(s) decomposes into nitrogen, oxygen and water. If 10 g of ammonium nitrate decompose entirely at 350 *C with ΔrxnHo = -289. kJ - How much heat is liberated? - How much work would be done by the system? - What will be the pressure of the system if, after completion of the reaction, the volume is 1.0 L and the temperature is 120°C?

Chemical cold packs used for sports injuries are made with solid ammonium nitrate (NH4NO3) and a...

Chemical cold packs used for sports injuries are made with solid ammonium nitrate (NH4NO3) and a plastic bag of water. When the bag of water is broken the ammonium nitrate dissolves. NH4NO3(s) --> NH4+ (aq) + NO3- (aq) As the solution forms, the water and bag get colder. Which of the following is true for this process. ( Assume the reaction above is our system) Chose all that apply Select one or more: a. The process is endothermic. b. Δ...

Copper salts are used for fireworks. Copper(II) nitrate has a strong emission at 450nm. Calculate the...

Copper salts are used for fireworks. Copper(II) nitrate has a strong emission at 450nm. Calculate the total energy (in kJ) of the emission for 5.00g. What is the frequency and the color of the light emitted?

Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and...

Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction: NH4NO3(s)→NH+4(aq)+NO−3(aq) In order to measure the enthalpy change for this reaction, 1.50 g of ammonium nitrate is dissolved in enough water to make 30.0 mL of solution. The initial temperature is 23.7 ∘C and the final temperature (after the solid dissolves) is...

nstant cold packs sometimes used to treat athletic injuries contain solid ammonium nitrate and liquid water...

nstant cold packs sometimes used to treat athletic injuries contain solid ammonium nitrate and liquid water separatedbya thin divider. When the divider is broken, the ammonium nitrate dissolves endothermically: NH4NO3(s) NH4+(aq) + NO3–(aq) To measure the enthalpy of this reaction, you dissolve 1.25 g of ammonium nitrate in enough water to make 25.0 mL of solution. The initial temperature is 25.8 °C, and the final temperature is 21.9 °C. (Assume that the density of the solution is 1.00 g /mL...

Ammonium nitrate is the most commercially important chemical product containing the ammonium ion. 1.List and describe...

Ammonium nitrate is the most commercially important chemical product containing the ammonium ion. 1.List and describe at least two grades of commercially available ammonium nitrate.. 2.Why does OSHA require employers to store bulk quantities of ammonium nitrate within a bin that is clean and free of contaminants? Give an example of a contaminant, and describe its interaction with ammonium nitrate.. Your total response must be at least 200 words in length.

Subjects