Question

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

Answer 1

Increasing the volume of the container will lead to an increase in the pressure of CO2 present at equilibrium.

Step-by-step explanation:

To increase the pressure of CO2 present at equilibrium, we need to shift the equilibrium towards the side with more CO2(g) molecules. According to Le Chatelier's principle, increasing the pressure of a system favors the side with fewer moles of gas. In this case, adding more BaCO3(s) does not change the number of moles of gas since the reaction does not involve CO2(g) directly, so it will not increase the pressure of CO2. However, increasing the volume of the container will decrease the pressure, causing the system to shift towards the side with more moles of gas, which is the decomposition of BaCO3(s) to BaO(s) and CO2(g). Therefore, increasing the volume of the container will increase the pressure of CO2 present at equilibrium.

Answer 2

Answer is: i. adding more baco3(s).
Balanced chemical reaction: BaCO₃(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.