Question

The number of p atoms in 1.0 g of ba3(po4)2 is:

Answer 1

The number of P atoms in 1.0 g of Ba3(PO4)2 is approximately 3.8762 x 10^21 atoms.

Step-by-step explanation:

The number of p atoms in 1.0 g of Ba3(PO4)2 can be calculated using the molar mass and Avogadro's number. The formula mass of Ba3(PO4)2 is 310.177 amu. From the given information, we can calculate the number of moles of Ba3(PO4)2 as follows:

Moles of Ba3(PO4)2 = Mass of Ba3(PO4)2 / Formula mass of Ba3(PO4)2

Moles of Ba3(PO4)2 = 1.0 g / 310.177 amu

Moles of Ba3(PO4)2 = 0.003221 moles

The number of p atoms can be calculated using the mole ratio between Ba3(PO4)2 and P atoms. In 1 mole of Ba3(PO4)2, there are 2 moles of P atoms. Therefore:

Moles of P atoms = Moles of Ba3(PO4)2 x 2

Moles of P atoms = 0.003221 moles x 2

Moles of P atoms = 0.006442 moles

To convert moles to number of atoms, we can use Avogadro's number:

Number of P atoms = Moles of P atoms x Avogadro's number

Number of P atoms = 0.006442 moles x 6.022 x 10^23 atoms/mol

Number of P atoms = 3.8762 x 10^21 atoms

Answer 2

First, we determine the number of moles of barium phosphate. This is done using:

Moles = mass / Mr
Moles = 1 / 602
Moles = 0.002

Now, we see from the formula of the compound that each mole of barium phosphate has 2 moles of phosphorus (P). Therefore, the moles of phosphorus are:
0.002 * 2 = 0.004

The number of particles in one mole of substance is 6.02 x 10²³. The number of phosphorus atoms will be:
0.004 * 6.02 x 10²³

2.41 x 10²¹ atoms of phosphorus are present