Stoichiometry of Reactions: Gram/Mole

Question

According to the following reaction, how many moles of dinitrogen monoxide will be formed upon the complete reaction of 30.7 grams of ammonium nitrate ?

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

Answer 1

Hi Sammy,

First, it will be important to come up with the chemical formula for dinitrogen monoxide and ammonium nitrate and water.

Dinitrogen Monoxide = N₂O

Ammonium Nitrate = NH₄NO₃

water = H₂O

This gives us N₂O + NH₄NO₃ + H₂O

In order to start any problem, we first need to make sure the equations are balanced. Are they balanced? If not, make sure to balance them with equal numbers of each atom on both sides. (Hint: Check N.)

Next, the question is giving us a known amount of NH₄NO₃ and asking us to find the amount of N₂O. In order to go from one compound to another on a balanced chemical reaction, we need to convert everything to moles, so 30.7g wll need to be converted to moles using the molar mass.

After you have moles of NH₄NO₃ you can multiply by the molar ratio in the balanced chemical reaction to get moles of N₂O which is the answer to the question.

Hope this helps!

-Winn