5.00g of an oxide of metal(M)gave 4.00g of the metal when reduced with Hydrogen. What is the empirical formula of the oxide? (M=64, O=16)
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Answer:Determine the empirical formula of the oxide. ... a compound with molar mass 60 g/mol was found to contain 12.0 g of carbon, 2.0 g of hydrogen and 16.0 g of oxygen. ... So the empirical formula is CH2O ... 12 + 2 + 16 = 30 ... Another way to approach this is to see that 0.06 to 0.08 is a 6 to 8 ratio and then reduce it to 3 to 4
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