Ammonium nitrate can decompose explosively when heated according to the equation 2 NH4NO31s2¡2 N21g2 + 4 H2O1g2 + O21g2 How many liters of gas would be formed at 450 °C and 1.00 atm pressure by explosion of 450 g of NH4NO3?

Verified step by step guidance

Convert the mass of NH_4NO_3 to moles using its molar mass.

Use the balanced chemical equation to determine the mole ratio between NH_4NO_3 and the total moles of gas produced.

Calculate the total moles of gas produced using the mole ratio from the balanced equation.

Apply the ideal gas law, PV = nRT, to find the volume of gas produced, where P is pressure, V is volume, n is moles of gas, R is the ideal gas constant, and T is temperature in Kelvin.

Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the relationships between the quantities of substances involved in a reaction. In this case, stoichiometry will help us find out how many moles of gas are produced from the decomposition of ammonium nitrate.

Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for calculating the volume of gas produced in a reaction under specific conditions of temperature and pressure. In this problem, we will use the Ideal Gas Law to convert the moles of gas produced into liters at the given temperature and pressure.

Gas Volume at STP

At standard temperature and pressure (STP), one mole of an ideal gas occupies 22.4 liters. However, in this question, we need to adjust for the given temperature of 450 °C and pressure of 1.00 atm. Understanding how to apply the Ideal Gas Law in conjunction with the concept of gas volume at STP is crucial for accurately determining the volume of gas produced from the decomposition of ammonium nitrate.

Recommended video:

Guided course

02:35

Constant-Volume Calorimetry

Related Practice

Textbook Question

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s) + 2 HCl(aq) ¡ ZnCl₂(aq) + H₂(g) (a) How many liters of H₂ would be formed at 742 mm Hg and 15 °C if 25.5 g of zinc was allowed to react?

Textbook Question

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s) + 2 HCl(aq) ¡ ZnCl₂(aq) + H₂(g) (b) How many grams of zinc would you start with if you wanted to prepare 5.00 L of H2 at 350 mm Hg and 30.0 °C?

Textbook Question

The reaction of sodium peroxide 1Na2O22 with CO2 is used in space vehicles to remove CO2 from the air and generate O2 for breathing:2 Na2O21s2 + 2 CO21g2¡2 Na2CO31s2 + O21g2(a) Assuming that air is breathed at an average rate of 4.50 L/min (25 °C; 735 mm Hg) and that the concentration of CO2 in expelled air is 3.4% by volume, how many grams of CO2 are produced in 24 h?

Textbook Question

Titanium(III) chloride, a substance used in catalysts for preparing polyethylene, is made by high-temperature reaction of TiCl₄ vapor with H₂: 2 TiCl₄(g) + H₂(g) → 2 TiCl₃(s) + 2 HCl(g) (a) How many grams of TiCl₄ are needed for complete reaction with 155 L of H₂ at 435 °C and 795 mm Hg pressure?

Textbook Question

Titanium(III) chloride, a substance used in catalysts for preparing polyethylene, is made by high-temperature reaction of TiCl₄ vapor with H₂: 2 TiCl₄(g) + H₂(g) → 2 TiCl₃(s) + 2 HCl(g) (b) How many liters of HCl gas at STP will result from the reaction described in part (a)?