Question

Write the state of matter for every substance in the chemical reaction.

Explain your limiting reactant determinations.

Mark every measured number showing the significant figures (SF).

Do not round any intermediate values. (you can show two digits past the marked SF)

Show subtraction and addition in the vertical format.

Show your final answer before rounding and then in the final form, rounded correctly.

Every number must have units and substances. You can use tables or other means to increase your efficiency, but the reader must be able to clearly identify the units and substances related to every number.

Include descriptive statements indicating what you are doing. For example: "Calculate the moles of the reactants"

EXERCISE 3.1.2: AMMONIUM NITRATE EXPLOSION

Ammonium nitrate is a common fertilizer, but under the wrong conditions it can be hazardous. In 1947, a ship loaded with ammonium nitrate caught fire during unloading and exploded, destroying the town of Texas City, Texas.

The explosion resulted from the following reaction:

2NH₄NO₃(s)→2N₂(g)+4H₂O(g)+O₂(g)

Strategy:

1. Use the coefficients from the balanced chemical equation to determine both the molecular and mole ratios.
2. Use the molar masses of the reactants and products to convert from moles to grams.
3. Use Avogadro’s number to convert from moles to the number of molecules.

Show the steps to construct a table showing how to interpret the information in the equation in terms of

1. individual molecules and ions.
2. moles of reactants and products.
3. grams of reactants and products given 2 mol of ammonium nitrate.
4. numbers of molecules or formula units of reactants and products given 2 mol of ammonium nitrate.

Answer:

	2NH4NO3(s)	→	2N2(g)	+	4H2O(g)	+	O2(g)
a.	2NH4+ ions and 2NO3− ions		2 molecules		4 molecules		1 molecule
b.	2 mol		2 mol		4 mol		1 mol
c.	160.0864 g		56.0268 g		72.0608 g		31.9988 g
d.	1.204 × 1024formula units		1.204 × 1024molecules		2.409 × 1024molecules		6.022 × 1023molecules