A mixture of magnesium carbonate and magnesium oxide of mass $12.46*g$ underwent fierce heating. After heating, there were $8.43*g$ of salt remaining. What were the masses of magnesium carbonate, and magnesium oxide in the original sample?

Md Ariful Islam

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Md Ariful Islam

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$MgCO_3(s)+DeltararrMgO(s) + CO_2(g)$

And we would have to heat the magnesium salt VERY fiercely to get complete decarboxylation.

$"Moles of carbon dioxide LOST"$ $=$ $(4.40*g)/(44.01*g*mol^-1)$

$=0.010*mol$

And therefore in the original mixture there were $0.010*mol$ $MgCO_3$, i.e. a mass of $0.010*molxx84.31*g=8.43*g$.

The balance of the salt must have $MgO$, which is (reasonably) inert to heating.

$"Mass of MgO"$ $=$ $12.46*g-8.43*g=4.03*g$.

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