the formula: Ca(ClO3)2 --> CaCl2 + 3O2
what mass pf O2 results from the decomposition of 1.00 kg of calcium carbonate
Convert kg to g.
Convert g Ca(ClO3)2 to moles. moles = g/molar mass.
Using the coefficients in the balanced question, convert moles Ca(ClO3)2 to moles O2.
Convert moles O2 to grams. grams = moles x molar mass. Post your work if you get stuck.
i dont undersatand
the answer
To find the mass of O2 produced from the decomposition of 1.00 kg of calcium carbonate, you need to follow these steps:
Step 1: Determine the molar mass of calcium carbonate (CaCO3).
Calcium carbonate (CaCO3) consists of one calcium atom (Ca), one carbon atom (C), and three oxygen atoms (O). The molar masses of calcium, carbon, and oxygen are approximately 40.08 g/mol, 12.01 g/mol, and 16.00 g/mol, respectively.
So, the molar mass of CaCO3 is calculated as:
(1 × 40.08 g/mol) + (1 × 12.01 g/mol) + (3 × 16.00 g/mol) = 100.09 g/mol
Step 2: Calculate the number of moles of CaCO3 in 1.00 kg.
To convert mass to moles, divide the mass (in grams) by the molar mass (in grams per mole).
Number of moles = Mass (in grams) / Molar mass (in g/mol)
Number of moles of CaCO3 = 1000 g / 100.09 g/mol ≈ 9.9978 mol
Step 3: Determine the stoichiometry of the reaction.
According to the balanced equation:
1 mole of Ca(ClO3)2 produces 3 moles of O2.
Step 4: Calculate the number of moles of O2 produced.
From the stoichiometry, we can conclude that:
9.9978 moles of CaCO3 will produce 3 × 9.9978 = 29.9934 moles of O2.
Step 5: Convert moles of O2 to mass.
To convert moles to mass, multiply the number of moles by the molar mass of O2, which is 32.00 g/mol.
Mass of O2 = Number of moles × Molar mass of O2
Mass of O2 = 29.9934 mol × 32.00 g/mol ≈ 959.8 g
Therefore, the mass of O2 produced from the decomposition of 1.00 kg of calcium carbonate is approximately 959.8 grams.