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When 0.288g of an oxide of metal M was reduced using suitable reducing agent, 0.256 of pure metal was formed. Determine the empirical formula of the oxide of the metal M. [M=64 O=16]

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Element      M          O
Mass        0.256     0.032
RAM            64        16
Moles       0.256    0.032
                  64         16  
                0.004    0.002
Ratio of    0.004     0.002
moles       0.002     0.002
                   2            1
Empirical Formula = M2O

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