Barium carbonate, baco3, is stable at ambient temperatures, but decomposes to barium oxide and carbon dioxide at higher temperatures. baco3 (s) bao (s) + co2 (g) at a certain temperature, this system is in equilibrium in a closed system and contains appreciable amounts of all three compounds. which changes will lead to an increase in the pressure of co2 present at equilibrium? i. adding more baco3 (s) ii. increasing the volume of the container

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Chemistry

Babbles

Yesterday, 17:35

Barium carbonate, baco3, is stable at ambient temperatures, but decomposes to barium oxide and carbon dioxide at higher temperatures. baco3 (s) bao (s) + co2 (g) at a certain temperature, this system is in equilibrium in a closed system and contains appreciable amounts of all three compounds. which changes will lead to an increase in the pressure of co2 present at equilibrium? i. adding more baco3 (s) ii. increasing the volume of the container

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Taffy · Answer 1

Answer is: i. adding more baco3 (s).

Balanced chemical reaction: BaCO ₃ (s) → BaO (s) + CO₂ (g).

If more barium carbonate (BaCO₃) is added, more carbon (IV) oxide would be produced. According to the gas law (pV = nRT), preesure (p) is proportional to amount of substance (n), more gas the higher is the pressure.