use the periodic table to determine how many atoms of phosphorus (p) are in a sample that has a mass of…

use the periodic table to determine how many atoms of phosphorus (p) are in a sample that has a mass of 172.90 g.\n3.48×10²¹ atoms\n1.97×10²² atoms\n3.36×10²⁴ atoms\n1.04×10²⁶ atoms\ndone

use the periodic table to determine how many atoms of phosphorus (p) are in a sample that has a mass of 172.90 g.\n3.48×10²¹ atoms\n1.97×10²² atoms\n3.36×10²⁴ atoms\n1.04×10²⁶ atoms\ndone

Answer

Explanation:

Step1: Find molar mass of P

From periodic table, molar mass of P is 30.97 g/mol.

Step2: Calculate number of moles

Number of moles $n=\frac{m}{M}$, where $m = 172.90$ g and $M=30.97$ g/mol. So $n=\frac{172.90}{30.97}= 5.5828$ mol.

Step3: Use Avogadro's number

Avogadro's number $N_A = 6.022\times 10^{23}$ atoms/mol. Number of atoms $N=n\times N_A$. So $N = 5.5828\times6.022\times 10^{23}=3.36\times 10^{24}$ atoms.

Answer:

3.36 × 10²⁴ atoms