Consider the decomposition of barium carbonate: BaCO₃(s) ⇌ BaO(s) + CO₂(g) Using data from Appendix C, calculate the equilibrium pressure of CO₂ at (b) 1100 K.

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Identify the reaction: BaCO_3(s) \(\rightleftharpoons\) BaO(s) + CO_2(g).

Use the standard Gibbs free energy change equation: \(\Delta\) G^\(\circ\) = \(\Delta\) H^\(\circ\) - T\(\Delta\) S^\(\circ\).

Find \(\Delta\) H^\(\circ\) and \(\Delta\) S^\(\circ\) for the reaction using Appendix C data.

Calculate \(\Delta\) G^\(\circ\) at 1100 K using the values from the previous step.

Use the relationship \(\Delta\) G^\(\circ\) = -RT\(\ln\) K to find the equilibrium constant K, and then determine the equilibrium pressure of CO_2.

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Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In the context of the decomposition of barium carbonate, the system reaches equilibrium when the amount of BaCO3 decomposing into BaO and CO2 is balanced by the amount of CO2 and BaO reverting back to BaCO3.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. In this case, increasing the temperature may shift the equilibrium position of the decomposition reaction, affecting the pressure of CO2 produced.

Equilibrium Constant (Kp)

The equilibrium constant (Kp) for a gaseous reaction is defined in terms of the partial pressures of the products and reactants at equilibrium. For the decomposition of barium carbonate, Kp can be expressed as the ratio of the partial pressure of CO2 to the concentration of BaCO3, allowing for the calculation of CO2 pressure at a given temperature, such as 1100 K.

Consider the decomposition of barium carbonate: BaCO3(s) ⇌ BaO(s) + CO2(g) Using data from Appendix C, calculate the equilibrium pressure of CO2 at (b) 1100 K.