Respuesta :

nkirotedoreen46

Answer:

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

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