Calculate the mass of 8.22x10^23 atoms of rubidium

116.67 g of rubidium

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

In this case;

Element is Rubidium

1 mole of Rubidium = 6.022 × 10^23 atoms

Moles = Number of atoms ÷ Avogadro's constant

Thus;

Moles of Rubidium = 8.22 × 10^23 atoms ÷ 6.022 × 10^23 atoms

                                = 1.365 moles

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

58750.08068 is the answer i think

thats how its supposed to be