According to the following reaction, how many grams of dinitrogen monoxide will be formed upon the complete reaction of 24.6 grams of ammonium nitrate?

Question

ammonium nitrate (aq) dinitrogen monoxide (g) + water (l)

Answer 1

Hello, Jaden,

I'll assume this is a decomposition reaction. We need to have a balanced equation as the first step.

I arrive at:

NH₄NO₃ = N₂O + 2H₂O [Use caution storing this compound. If part starts decomposing, the released energy will set off the rest].

Next, convert 24.6 grams of ammonium nitrate into moles NH₄NO₃.

(24.6 g)/(80.0 g/mole) = 0.308 moles NH₄NO₃

The balanced equation promises 1 mole of N₂O for every 1 mole of NH₄NO₃, a molar ratio of 1:1. This means we should expect 0.308 moles of N₂O.

Convert moles N₂O into grams by multiplying times the molar mass of N₂O:

(0.308 moles)*(44.0 g/mole) = 13.6 g N₂O

Bob