Final answer:
To calculate the mass of nitrogen dioxide from 0.750 moles of mercury (II) nitrate, we use the molar ratio from the decomposition reaction and find that 69.00825 grams of nitrogen dioxide should be produced.
Step-by-step explanation:
When solid mercury (II) nitrate is heated, it decomposes to form solid mercury (II) oxide, gaseous nitrogen dioxide, and oxygen gas. To calculate the mass of nitrogen dioxide produced from 0.750 moles of mercury (II) nitrate, we first need a balanced chemical equation for the decomposition:
Hg(NO3)2 (s) → HgO (s) + 2 NO2 (g) + 1/2 O2 (g)
This equation shows that from each mole of mercury (II) nitrate, we get 2 moles of nitrogen dioxide (NO2). Consequently, 0.750 moles of mercury (II) nitrate will produce 1.5 moles of NO2. We then use the molar mass of NO2 (46.0055 g/mol) to find the mass:
Mass of NO2 = moles of NO2 × molar mass of NO2
Mass of NO2 = 1.5 moles × 46.0055 g/mol = 69.00825 g of NO2
Therefore, 0.750 moles of mercury (II) nitrate should produce 69.00825 grams of nitrogen dioxide upon decomposition.