Calculate the mass of 8.22x10^23 atoms of rubidium

116.67 g of rubidium

Explanation:

Concept tested: Moles of an element and the Avogadro's constant

An element is made up of similar atoms. One mole of an element contains atoms that are equivalent to the Avogadro's number. Avogadro's number is 6.022 * 10^23 Therefore; 1 mole of an element = 6.022 * 10^23 atoms

In this case;

Element is Rubidium

1 mole of Rubidium = 6.022 * 10^23 atoms

Step 1: Number of moles of Rubidium

Moles = Number of atoms : Avogadro's constant

Thus;

Moles of Rubidium = 8.22 * 10^23 atoms : 6.022 * 10^23 atoms

= 1.365 moles

Step 2: Mass of rubidium

Mass = Number of moles * Molar mass

Molar mass of rubidium = 85.47 g/mol

Therefore;

Mass of rubidium = 1.365 moles * 85.47 moles

= 116.67 g

Therefore, the mass of 8.22 * 10^23 atoms of rubidium is 116.67 g