First, we need to calculate the number of moles of CO2 produced:
0.855 g CO2 x (1 mol CO2/44.01 g CO2) = 0.0194 mol CO2
Since the balanced chemical equation tells us that 1 mole of XCO3 produces 1 mole of CO2, we know that 0.0194 moles of XCO3 were used in the reaction.
Now, we can use the mass of XCO3 and the number of moles used to calculate its molar mass:
Molar mass of XCO3 = 2.012 g / 0.0194 mol = 103.711 g/mol
Therefore, the molar mass of the metal carbonate XCO3 is 103.711 g/mol. Answer: 103.711 g/mol.
A metal carbonate, XCO3 of mass 2.012g 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). Hint: calculate the mole of CO2 first.
123.511 g/mol
62.011 g/mol
197.311 g/mol
103.711 g/mol
1 answer
1 answer