Ammonium Nitrate (NH4NO3), an important fertilizer, produces Dinitrogen monoxide gas (N2O) and water when it decomposes. Determine the mass of the water produced from the decomposition of 25.00 grams of solid Ammonium Nitrate.

11.23 grams of water produced from the decomposition of 25.00 grams of solid Ammonium Nitrate.

How we calculate moles from mass?

We can determine the moles of any substance by using the equation:

n = W /M, Where:

n = no. of moles

W = given mass

And M = molar mass

Given balanced equation is:

NH₄NO₃ → N₂O + 2H₂O

Also given that mass of NH₄NO₃ = 25 g

Mole of NH₄NO₃ = 25 / 80 = 0.312 mol

From the stoichiometry of the reaction, ratio between NH₄NO₃ and water is 1:2; it means one mole of NH₄NO₃ will produce 2 moles of water.

Moles of water formed = 2 × 0.312 = 0.624 mol

Now we convert this mole to grams through following way:

W = n × M

W = 0.624 × 18 = 11.23 grams

Hence, produced mass of water is 11.23 grams.

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Mass = 11.23 g

Explanation:

Given data:

Mass of water produced = ?

Mass of ammonium nitrate decomposed = 25.0 g

Solution:

Chemical equation:

NH₄NO₃     →    N₂O + 2H₂O

Number of moles of NH₄NO₃ :

Number of moles = mass/molar mass

Number of moles = 25.0 g/ 80.0 g/mol

Number of moles = 0.312 mol

Now we will compare the moles of NH₄NO₃  and H₂O

            NH₄NO₃       :        H₂O

                1               :          2

             0.312          :       2/1×0.312 = 0.624 mol

Mass of water formed:

Mass = number of moles × molar mass

Mass = 0.624 mol × 18 g/mol

Mass = 11.23 g

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