There are 5.00*10^-3 moles of lead II nitrate. Calculate how man grams this is.
grams = mols x molar mass = ?
To calculate the number of grams, we need to know the molar mass of lead II nitrate (Pb(NO3)2). The molar mass is the sum of the atomic masses of each element in the compound.
To find the molar mass of Pb(NO3)2:
- The atomic mass of lead (Pb) is 207.2 g/mol.
- The atomic mass of nitrogen (N) is 14.01 g/mol.
- The atomic mass of oxygen (O) is 16.00 g/mol.
Since there are 2 nitrogen atoms and 6 oxygen atoms in lead II nitrate, we can calculate the molar mass as follows:
Molar mass = (1 x Pb) + (2 x N) + (6 x O)
= 207.2 + (2 x 14.01) + (6 x 16.00)
= 207.2 + 28.02 + 96.00
= 331.22 g/mol
Now, to calculate the mass of 5.00 x 10^-3 moles of lead II nitrate:
Mass (in grams) = Number of moles x Molar mass
= 5.00 x 10^-3 moles x 331.22 g/mol
= 1.6561 grams
Therefore, 5.00 x 10^-3 moles of lead II nitrate is equivalent to 1.6561 grams.