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
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.
To determine the molar mass of XCO3, we first need to calculate the molar mass of CO2 produced.
1. Calculate the moles of CO2 using the given mass:
Moles of CO2 = Mass of CO2 / Molar mass of CO2
Given:
Mass of CO2 = 0.855 g
Molar mass of CO2 = 12.011 g/mol (C) + 2(15.999 g/mol) (O) = 44.011 g/mol
Moles of CO2 = 0.855 g / 44.011 g/mol ≈ 0.019 Mols
2. We know that 1 mol of XCO3 produces 1 mol of CO2. Therefore, the molar mass of XCO3 is equal to the mass of XCO3 divided by the moles of CO2 produced:
Molar mass of XCO3 = Mass of XCO3 / Moles of CO2
Given:
Mass of XCO3 = 2.012 g
Moles of CO2 = 0.019 moles
Molar mass of XCO3 = 2.012 g / 0.019 mol ≈ 105.894 g/mol
So, the molar mass of XCO3 is approximately 105.894 g/mol.
Therefore, option 103.711 g/mol is the closest value.