How many molecules of water are produced when 3.14 grams of ammonium nitrate are decomposed

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Explanation:

Remark

Ammonium Nitrate decomposes as follows.

NH4NO3 → N2O + 2H2O

If this does not agree with the reaction you have, let me know.

Step One

Find the molecular Mass of Ammonium Nitrate.

N =  1 * 14  =  14

H =  1 * 3 =     3

N =  1 * 14     14

O3 = 3*16  = 48

Molar Mass =69

Note: the masses used are approximate. Every periodic table is different. When you answer this question use the masses on your periodic table. My numbers are just guides.

Step Two

Find the number of mols in Ammonium Nitrate.

Formula

mols = given mass / molar mass

Givens

given mass = 3.14

Molar Mass = 69

mols  = 3.14 / 69

mols = 0.0455

Step 3

moles of water.

1 mol of Ammonium Nitrate = 2 mols of water

0.0455 mols of Ammonium Nitrate = x mols of water

x = 2* 0.0455 mols of water.

x = 0.091 mols of water

Step 4

Find the molecules of water.

1 mol of water = 6.02*10^23 molecules of water

0.091 mol water= x

x = 0.091 * 6.02*10^23

x = 5.48 * 10^23

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increased stability in the completion of fluorine's outer shell.