Final answer:
The formula for the lead oxide formed when 207 g of lead reacts with oxygen to produce 239 g of lead oxide, based on their relative atomic masses, is PbO. This is determined by calculating the molar ratios of lead and oxygen, which are both 1:1. Final answer. Hence, The relative molecular mass of Lead II trioxonitrate V is 232 g/mol.
Step-by-step explanation:
The question seeks to determine the formula of the lead oxide that forms when lead combines with oxygen, given the masses of lead and the resulting lead oxide as well as the relative atomic masses for lead (Pb) and oxygen (O).
When 207 g of lead (Pb) reacts with oxygen (O), the mass of the resulting lead oxide is 239 g. The increase in mass (239 g - 207 g) indicates that 32 g of oxygen has combined with the lead. We must first find the moles of lead and oxygen. For lead, we use its relative atomic mass of 207 g/mol, and for oxygen, we use the atomic mass of 16 g/mol (since oxygen normally forms molecules of O2, we use 32 g/mol for a molecule of oxygen).
Moles of Pb = mass of Pb / relative atomic mass of Pb = 207 g / 207 g/mol = 1 mol
Moles of O = mass of O / relative atomic mass of O = 32 g / 32 g/mol = 1 mol
The mole ratio of Pb to O is 1:1, which suggests that the formula for the lead oxide is PbO.
The relative molecular mass of Lead II trioxonitrate V can be calculated by summing the atomic masses of its constituent elements. From the given information, the atomic masses of Pb, N, and O are 108, 14, and 16, respectively. Since the formula for the compound is Pb(NO3)2, we have:
108 + (2 * 14) + (6 * 16) = 108 + 28 + 96
= 232 g/mol
The molecular mass of Lead II trioxonitrate V is 232 g/mol.