To solve the problem, we need to use the law of conservation of mass. The total mass of the reactants (XCO3) must equal the total mass of the products (XO and CO2).
We can start by finding the moles of CO2 produced, using its mass and molar mass:
0.855 g CO2 x (1 mol CO2 / 44.01 g CO2) = 0.01944 mol CO2
Since the coefficient of CO2 in the balanced equation is 1, this is also the number of moles of XCO3 that reacted.
Now we can find the molar mass of XCO3 by dividing its mass by the number of moles:
2.012 g XCO3 / 0.01944 mol XCO3 = 103.711 g/mol
Therefore, the metal carbonate XCO3 has a molar mass of 103.711 g/mol.
The correct answer is option B: 103.711 g/mol.
A metal carbonate, XCO3 of mass 2.012 g was heated resulting in the formation of XO, a metal oxide and carbon dioxide with a mass of 0.855 g according to the reaction shown below:
XCO3 (s) → XO (s) + CO2 (g)
(Atomic mass of O-15.999 g/mol; H-1.008 g/mol; C-12.011 g/mol).
123.511g/mol
103.711 g/mol
197.311 g/mol
62.011 g/mol
1 answer