What is the Kc for the following reaction at equilibrium at 800∘C if [CO2]= 0.030M ?
CaCO3(s)⇌CaO(s)+CO2(g)
To calculate the equilibrium constant (Kc) for the given reaction, we need the concentrations of the products and reactants at equilibrium.
Given:
[CO2] = 0.030M
Since there is no information provided about the concentrations of CaCO3(s) and CaO(s), we cannot directly calculate the equilibrium constant (Kc). However, we can make some assumptions and proceed with the calculations.
Assuming the reaction reached equilibrium, we can say that the amount of CaCO3(s) reacted to form CaO(s) and CO2(g) would be equal and can be represented as a variable, let's say 'x'. Therefore, the concentration of CO2(g) can be considered as [CO2] = 0.030 - x M.
Remember that the concentration of a solid (CaCO3(s) and CaO(s)) is not included in the equilibrium expression, so we don't need their concentrations.
The equilibrium constant (Kc) for the reaction is given by the ratio of the products' concentrations to the reactants' concentrations, each raised to their respective stoichiometric coefficients.
Kc = [CO2] / ([CaO] * [CO2])
Plugging in the given concentration values:
Kc = (0.030 - x) / ([CaO] * (0.030 - x))
Since the exact concentrations of CaCO3(s) and CaO(s) are unknown, we cannot determine an exact value for Kc without further information. The value of Kc will depend on the actual concentrations of CaCO3(s) and CaO(s) at equilibrium.
Therefore, we need additional information or experimental data to calculate the exact value of Kc for this reaction at 800∘C.