Question

Use the periodic table to determine how many atoms of phosphorus (P) are in a sample that has a mass of 172.90 g

Answer 1

3.36 × 1024 atoms

Next ones are:

9.01g

0.276g

78,600g

Step-by-step explanation:

Answer 2

3.36 × 10^24 atoms

Step-by-step explanation:

We are given;

• Mass of phosphorus is 172.90 g

We are supposed to calculate the number of atoms of phosphorus;

• Note that 1 mole of an element contains 6.022 × 10^23 atoms

In this case;

• 1 mole of phosphorus contains 6.022 × 10^23 atoms

• But; Molar mass of phosphorus is 30.97 g/mol

Therefore;

30.97 g contain 6.022 × 10^23 atoms

Thus, for 172.90 g

= (172.90 g /30.97 g) × 6.022 × 10^23 atoms/mol

= 3.36 × 10^24 atoms

Thus, 172.90 g of phosphorus contains 3.36 × 10^24 atoms