A 1.871 gram sample of an unknown metallic carbonate is decomposed by heating to form the metallic oxide and 0.656 g of carbon dioxide according to the equation
MCO3(s) -> MO(s) + CO2(g)
What is the metal?
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Mole mass in `g/(mol)`
`CO_2 : MCO_3 =1:1`
Amount of `CO_2` produced `=0.656/(12+32) =0.015`
Amount of `MCO_3`reacted =0.015 mol
It is given that 1.871g of the unknown metal carbonate reacted. If the molar mass of M is X g/mol.
According to the molar mass the metal the metal can be Copper (Cu=63.5) Or Zinc(Zn=65.4).
- The metal carbonate sample is pure and without impurities .
- The sample is fully decomposed at the heating process.
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