Chemistry: According to the following reaction, how many moles of ammonium nitrite are necessary to form 0.298 moles water?

Question

According to the following reaction, how many moles of ammonium nitrite are necessary to form 0.298 moles water?

ammonium nitrite (aq) ———-> nitrogen (g) + water (I)

= moles ammonium nitrite

Answer 1

@Jay K. I notice that you have posted several questions of the same type. I will attempt to answer this one, and any of the others that may be different. But if they are the same as this one, I'm hoping you can follow this methodology and do the others yourself. If not, you can repost them.

ammonium nitrite (aq) ==> nitrogen(g) + water(l)

ammonium nitrite = NH₄NO₂

nitrogen gas = N₂

water = H₂O

NH₄NO₂(aq) ==> N₂(g) + H₂O ... unbalanced equation

NH₄NO₂(aq) ==> N₂(g) + 2H₂O .. balanced equation

Now, use the stoichiometry (mole ratios) of this balanced equation, along with dimensional analysis, to find the answer to the question. The stoichiometry shows us that 1 mol ammonium nitrite (NH₄NO₂) produces 2 mols of water (H₂O)

0.298 mols H₂O x 1 mol NH₄NO₂ / 2 mols H₂O = 0.149 mols NH₄NO₂