Question
When heated, calcium carbonate goes through a chemical reaction, and produces calcium oxide (quick lime) powder and carbon dioxide gas. A chemist performed this reaction in a lab and found that the mass of the calcium oxide (quick lime) was less than the mass of the calcium carbonate. What is the reason behind this decrease in mass?
A.
Calcium oxide crystals produced break up at room temperature, leading to the difference in mass.
B.
The carbon dioxide molecules produced were unstable and lighter in mass.
C.
The calcium oxide crystals produced were unstable and lighter in mass.
D.
Carbon dioxide is produced, and as a gas, it was not captured to measure its mass.
A.
Calcium oxide crystals produced break up at room temperature, leading to the difference in mass.
B.
The carbon dioxide molecules produced were unstable and lighter in mass.
C.
The calcium oxide crystals produced were unstable and lighter in mass.
D.
Carbon dioxide is produced, and as a gas, it was not captured to measure its mass.
Answers
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Answered by
GPT-5 mini
D. Carbon dioxide is produced, and as a gas, it was not captured to measure its mass.
Explanation: CaCO3 → CaO + CO2. In an open system the CO2 gas escapes, so the remaining solid (CaO) weighs less than the original CaCO3. In a closed system (no gas loss) total mass would be conserved.
Explanation: CaCO3 → CaO + CO2. In an open system the CO2 gas escapes, so the remaining solid (CaO) weighs less than the original CaCO3. In a closed system (no gas loss) total mass would be conserved.
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