If 10 g of CaCO3 decomposes completely, how many grams of CO2 are produced?

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Question: If 10 g of CaCO3 decomposes completely, how many grams of CO2 are produced?

Options:

Correct Answer: 44 g

Solution:

10 g of CaCO3 = 0.1 moles. CaCO3 → CaO + CO2, so 0.1 moles of CO2 = 0.1 * 44 g = 4.4 g.

If 10 g of CaCO3 decomposes completely, how many grams of CO2 are produced?

If 10 g of CaCO3 decomposes completely, how many grams of CO2 are produced?

Step 1: Identify the chemical reaction. Calcium carbonate (CaCO3) decomposes into calcium oxide (CaO) and carbon dioxide (CO2).
Step 2: Calculate the molar mass of CaCO3. The molar mass is approximately 100 g/mol (40 for Ca + 12 for C + 3*16 for O).
Step 3: Convert grams of CaCO3 to moles. Use the formula: moles = mass (g) / molar mass (g/mol). So, 10 g / 100 g/mol = 0.1 moles of CaCO3.
Step 4: Use the stoichiometry of the reaction. From the balanced equation, 1 mole of CaCO3 produces 1 mole of CO2.
Step 5: Since we have 0.1 moles of CaCO3, it will produce 0.1 moles of CO2.
Step 6: Calculate the mass of CO2 produced. The molar mass of CO2 is approximately 44 g/mol (12 for C + 2*16 for O).
Step 7: Multiply the moles of CO2 by its molar mass: 0.1 moles * 44 g/mol = 4.4 g of CO2.

Stoichiometry – The calculation of reactants and products in chemical reactions based on balanced equations.
Molar Mass Calculation – Determining the mass of a substance using its molar mass to convert between grams and moles.
Decomposition Reactions – Understanding how compounds break down into simpler substances, in this case, CaCO3 into CaO and CO2.