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20 January, 18:21

Yet a third pair of compounds of manganese and oxygen is 50.48% and 36.81% oxygen respectively. In what small whole number ratio do masses of oxygen combine with a fixed mass of manganese in these two compounds

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  1. 20 January, 18:42
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    The number ratio is 4:7

    Explanation:

    Step 1: Data given

    Compound 1 has 50.48 % oxygen

    Compound 2 has 36.81 % oxygen

    Molar mass oxygen = 16 g/mol

    Molar mass manganese = 54.94 g/mol

    Step 2: Calculate % manganes

    Compound 1: 100 - 50.48 = 49.52 %

    Compound 2: 100 - 36.81 = 63.19 %

    Step 3: Calculate mass

    Suppose mass of compounds = 100 grams

    Compound 1:

    50.48 % O = 50.48 grams

    49.52 % Mn = 49.52 grams

    Compound 2:

    36.81 % O = 36.81 grams

    63.19 % Mn = 63.19 grams

    Step 4: Calculate moles

    Compound 1

    Moles O = 50.48 grams / 16.0 g/mol = 3.155 moles

    Moles Mn = 49.52 grams / 54.94 g/mol = 0.9013 moles

    Compound 2

    Moles O = 36.81 grams / 16.0 g/mol = 2.301 moles

    Moles Mn = 63.19 grams / 54.94 g/mol = 1.150 moles

    Step 5: calculate mol ratio

    We will divide by the smallest amount of moles

    Compound 1

    O: 3.155/0.9013 = 3.5

    Mn: 0.9013 / 0.9013 = 1

    Mn2O7

    Compound 2

    O: 2.301 / 1.150 = 2

    Mn: 1.150 / 1.150 = 1

    MnO2

    The number ratio is 2:3.5 or 4:7
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