Chemistry Homework

Question

According to the following reaction, how many grams of dinitrogen monoxide will be formed upon the complete reaction of 31.2 grams of ammonium nitrate?

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

Please show the steps on how to balance, before computing the equation.

Answer 1

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

....NH₄NO₃(aq) ===> ............ N₂O(g) ...........+ ...............H₂O(l) ... unbalanced equation

Looking at nitrogen (N), there are 2 N on each side of the equation, so that is balanced.

Looking at hydrogen (H), there are 4 H on the left but only 2 H on the right. Put a 2 in front of H2O

NH₄NO₃(aq) ===> N₂O(g) + 2H₂O(l) and now the H is balaned.

Looking at oxygen (O), there are 3 O on the left and 3 O on the right, so it it balanced.

So now every element (N, H, O) is balanced and that is the balanced equation:

NH₄NO₃(aq) ===> N₂O(g) + 2H₂O(l) ... balanced equation

Now, using the mole ratios of the balanced equation and dimensional analysis, we compute the following:

31.2 g NH₄NO₃ x 1 mol NH₄NO₃ / 80.0 g x 1 mol N₂O / 1 mol NH₄NO₃ x 44.0 g N₂O/ mol N₂O = 17.2 g N₂O

Answer 2

Use the following steps to solve this problem.

1. Replace the names of the compounds with their chemical formula (e.g. Ammonia nitrate is NH₄NO₃)
2. Balance the chemical equation.
3. Convert the grams of ammonia nitrate to moles ( moles = grams/ molar mass).
4. The ratio of the coefficients of the compounds in the balanced equation is the same as the mole ratio. Use this to determine the number of moles of dinitrogen monoxide that is produced.
5. Convert the number of moles of dinitrogen monoxide to grams (multiply moles by molar mass).