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26 September, 22:47

Calculate the mass of 8.22x10^23 atoms of rubidium

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  1. 26 September, 23:16
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    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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