Dolomite is a mixed carbonate of calcium and magnesium that decomposes to CO2 and the metal oxides MgO and CaO upon heating. When 15.42 g of dolomite is heated, 7.85 g of MgO and CaO are produced. What is percent by mass of MgCO3 in the original sample of dolomite?
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CaCO3 → CaO + CO2 [balanced as written] MgCO3 → MgO + CO2 [balanced as written] Let z be the mass of MgCO3 (in grams) to be found. Then (15.42 - z) is the mass of CaCO3 z / (84.3139 g MgCO3/mol) x (1 mol CO2 / 1 mol MgCO3) (0.0118604 z) mol CO2 from MgCO3 (15.42 - z) / (100.0875 g CaCO3/mol) x (1 mol CO2 / 1 mol CaCO3) (0.154065 - 0.00999126 z) mol CO2 from CaCO3 (15.42 g - 7.85 g) / (44.00964 g CO2/mol) 0.172008 mol CO2 total (0.0118604 z) + (0.154065 - 0.00999126 z) 0.172008 Solve for z algebraically: z ≈ 9.5996 ≈ 9.60 g MgCO3
