To determine the mass of nitrogen(V) oxide produced by heating lead trioxonitrate(V), we need to balance the chemical equation.
The chemical formula for lead trioxonitrate(V) is Pb(NO3)2, and when heated, it decomposes into lead(II) oxide (PbO), nitrogen(IV) oxide (NO2), and oxygen gas (O2).
The balanced chemical equation for this reaction is:
2Pb(NO3)2 → 2PbO + 4NO2 + O2
From the balanced equation, we can see that for every 2 moles of lead trioxonitrate(V) decomposed, we obtain 4 moles of nitrogen(IV) oxide.
First, let's convert the given mass of lead trioxonitrate(V) (33.3g) into moles:
Using the molar mass of Pb(NO3)2, which is approximately 331.21 g/mol:
33.3g Pb(NO3)2 * (1 mol / 331.21 g) ≈ 0.1005 mol Pb(NO3)2
According to the balanced chemical equation, for every 2 moles of Pb(NO3)2, we obtain 4 moles of NO2.
So, we can calculate the moles of NO2 produced:
0.1005mol Pb(NO3)2 * (4 mol NO2 / 2 mol Pb(NO3)2) = 0.201 mol NO2
Finally, let's convert the moles of NO2 into grams, using the molar mass of NO2, which is approximately 46.01 g/mol:
0.201 mol NO2 * 46.01 g/mol ≈ 9.255 g NO2
Therefore, heating 33.3g of lead trioxonitrate(V) would produce approximately 9.255 grams of nitrogen(IV) oxide.