Ammonium nitrate decomposes explosively upon heating...

Ammonium nitrate decomposes explosively upon heating according to the following balanced equation: $$ 2 \mathrm{NH}_{4} \mathrm{NO}_{3}(s) \longrightarrow 2 \mathrm{~N}_{2}(g)+\mathrm{O}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g) $$ Calculate the total volume of gas (at $125^{\circ} \mathrm{C}$ and $748 \mathrm{mmHg}$ ) produced by the complete decomposition of $1.55 \mathrm{~kg}$ of ammonium nitrate.

Ammonium nitrate decomposes explosively upon heating according to the following balanced equation:
$$
2 \mathrm{NH}_{4} \mathrm{NO}_{3}(s) \longrightarrow 2 \mathrm{~N}_{2}(g)+\mathrm{O}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)
$$
Calculate the total volume of gas (at $125^{\circ} \mathrm{C}$ and $748 \mathrm{mmHg}$ ) produced by the complete decomposition of $1.55 \mathrm{~kg}$ of ammonium nitrate.

Key Concepts

Stoichiometry

Stoichiometry involves using the balanced chemical equation to determine the quantitative relationships between reactants and products. It allows one to calculate the number of moles of gas produced from a given amount of a reactant by relying on the mole ratios established in the balanced equation.

Mole-Mass Conversion

Mole-mass conversion is a fundamental process in chemistry where the mass of a substance is converted to moles using its molar mass. This conversion is essential for linking the measured mass of a sample to the number of molecules or atoms involved in a chemical reaction.

Ideal Gas Law

The Ideal Gas Law (PV = nRT) is used to relate the pressure, volume, temperature, and number of moles of a gas. It is particularly useful for calculating the volume of gas produced in a reaction when the pressure and temperature conditions are known, as it connects the macroscopic properties of gases to the amount of substance present.

Unit Conversion

Unit conversion is crucial in ensuring that all quantities are expressed in consistent units before applying formulas such as the Ideal Gas Law. This includes converting temperatures from Celsius to Kelvin and pressure measurements from units like mm Hg to atmospheres or other units consistent with the gas constant used.

Transcript

00:01 Hello guys i'm here to solve question 106 you are the first one i will write i will write the equation given the chemical equation ammonium nitrates composed to form nitrogen gas and oxygen gas and water water gas steam so all the product is so my approach to solving this question is finding the photo of the product, the gaside product, finding the volume of the gaseous product at stp standard temperature and pressure.

01:05 Then from that i will use gagelor to find the volume at 25 degrees celsius and 749.

01:17 So i write my approach, find volume of gases of gaseous product formed at stp.

01:46 Then use cast law to find a volume at key phone, temperature, and product.

02:13 Okay, now i'm starting.

02:17 So from this reaction, we can say that two more of ammonium nitrate solid give two plus one okay two all the product i guess two plus one that is seven more of product so i will do why i will start my process like this one 5 5 kilogram ammonium nitrates then it compares to gram cost 1 kilogram gives 1 ,000 graph then from this from this reactor i want to calculate the nh4 nlh i want to calculate the molecular weight this to be 14 plus 1 times 4 plus 14 of the same particle everything gives me 80 grams per more so i would say 80 gram ammonium nitrate is different to one more ammonium nitrates and then from the reaction two more ammonium nitrate gives total of seven more of more of of gaseous products of gaseous products and one more of gracious products we have volume of 22 .4 theta xtp so i get this let me use my i'm going to use my calculator right now that would be 1 .555501 ,000 5x25 by 7 multiplied by 22 .4, 25, 580 and product 2.

05:50 That is 15190 liter of ks products at stp...

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