the aim of this experiment is to determine how much lead oxide can be made from 4,0g of lead nitrate.calculate the mass of lead oxide you should make.
Each mole of Pb(NO3)2 will make one mole of PbO
So, how many moles of Pb(NO3)2 are in 4.0 grams?
What is the mass of that many moles of PbO
To calculate the mass of lead oxide that can be made from 4.0g of lead nitrate, we need to use stoichiometry. The balanced chemical equation for the reaction between lead nitrate (Pb(NO3)2) and lead oxide (PbO) is as follows:
3 Pb(NO3)2 → Pb3O4 + 6 NO2 + O2
From the equation, we can see that 3 moles of lead nitrate react to form 1 mole of lead oxide. Therefore, we need to convert the mass of lead nitrate to moles using its molar mass, and then calculate the moles of lead oxide formed.
1. Calculate the molar mass of lead nitrate (Pb(NO3)2):
- Atomic mass of Pb = 207.2 g/mol
- Atomic mass of N = 14.0 g/mol
- Atomic mass of O = 16.0 g/mol
- Molar mass of Pb(NO3)2 = (207.2 + (14.0 × 2) + (16.0 × 6)) g/mol = 331.2 g/mol
2. Convert the mass of lead nitrate to moles:
- Moles of Pb(NO3)2 = Mass / Molar mass
- Moles of Pb(NO3)2 = 4.0 g / 331.2 g/mol ≈ 0.012 mol
3. Use the stoichiometric ratio to find the moles of lead oxide produced:
- Moles of PbO = Moles of Pb(NO3)2 × (1 mol PbO / 3 mol Pb(NO3)2)
- Moles of PbO = 0.012 mol × (1/3) mol = 0.004 mol
4. Calculate the mass of lead oxide formed:
- Mass of PbO = Moles of PbO × Molar mass of PbO
- Molar mass of PbO = 207.2 g/mol
- Mass of PbO = 0.004 mol × 207.2 g/mol ≈ 0.8288 g
Therefore, the mass of lead oxide that can be made from 4.0g of lead nitrate is approximately 0.8288 grams.