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23 August, 17:41

A 7.337 gram sample of chromium is heated in the presence of excess oxygen. A metal oxide is formed with a mass of 9.595 g. Determine

the empirical formula of the metal oxide.

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  1. 23 August, 17:56
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    Empirical formula is CrO

    Explanation:

    We are given;

    Mass of sample of Chromium as 7.337 gram Mass of the metal oxide formed as 9.595 g

    We are required to determine the empirical formula of the metal oxide.

    Step 1; Determine the mass of oxygen used

    Mass of oxygen = Mass of the metal oxide - mass of the metal

    = 9.595 g - 7.337 g

    = 2.258 g

    Step 2: Determine the moles of chromium and oxygen

    Moles of chromium metal

    Molar mass of chromium = 51.996 g/mol

    Moles of Chromium = 7.337 g : 51.996 g/mol

    = 0.141 moles

    Moles of oxygen

    Molar mass of oxygen = 16.0 g/mol

    Moles of Oxygen = 2.258 g : 16.0 g/mol

    = 0.141 moles

    Step 3: Determine the simplest mole number ratio of Chromium to Oxygen

    Mole ratio of Chromium to Oxygen

    Cr : O

    0.141 mol : 0.141 mol

    1 : 1

    Empirical formula is the simplest whole number ratio of elements in a compound.

    Thus the empirical formula of the metal oxide is CrO
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