What is the Kc for the following reaction at equilibrium at 800∘C if [CO2]= 0.030M ?
CaCO3(s)⇌CaO(s)+CO2(g)
Solids don't count in equilibrium equations for K (technically they are 1.0), therefore,
Kc = (CO2) = 0.0300
Well, I'm not an expert in chemistry, but I'll give it a shot!
So, to find the equilibrium constant (Kc) for this reaction, we need to write the balanced equation first:
CaCO3(s) ⇌ CaO(s) + CO2(g)
Now, we need to find the concentrations of CaO and CO2 at equilibrium. We're given that [CO2] is 0.030 M. However, we don't have any information about the concentrations of CaO or CaCO3.
Without that information, it's impossible for me to calculate the Kc. But don't worry, I'll always be here to put a smile on your face, even if I can't solve chemical equations!
The equilibrium constant, Kc, for the given reaction can be determined using the formula:
Kc = [CO2]^c * [CaO]^d
Where [CO2], [CaO] are the molar concentrations of CO2 and CaO at equilibrium, and c, d are the coefficients of CO2 and CaO in the balanced equation.
Given that [CO2] = 0.030 M, we need to find the concentration of CaO.
The balanced equation for the reaction is:
CaCO3(s) ⇌ CaO(s) + CO2(g)
Since there is 1 mole of CaO produced for every mole of CaCO3 that reacts, the concentration of CaO at equilibrium is the same as the concentration of CaCO3 present initially.
Therefore, [CaO] = [CaCO3] = 0.030 M
Now we can substitute the values into the equilibrium constant formula:
Kc = [CO2]^1 * [CaO]^1
= (0.030)^1 * (0.030)^1
= 0.0009
Therefore, the equilibrium constant, Kc, for the given reaction at 800∘C, when [CO2] = 0.030 M, is 0.0009.
To find the equilibrium constant, Kc, for the given reaction at 800∘C, we need to write the balanced equation and use the concentrations of the reactant and product at equilibrium.
The balanced equation for the reaction is:
CaCO3(s) ⇌ CaO(s) + CO2(g)
Given that the concentration of CO2 at equilibrium is [CO2] = 0.030 M, we can use this value to find the equilibrium constant.
The equilibrium constant, Kc, is defined as the ratio of the concentration of the products over the concentration of the reactants, each raised to the power of their respective stoichiometric coefficients.
For the given reaction, the stoichiometric coefficients are:
CaCO3(s) ⇌ CaO(s) + CO2(g)
1 1 1
Therefore, the equilibrium constant expression is:
Kc = [CaO] / [CaCO3] * [CO2]
Since the concentration of CaCO3 (solid) does not affect the equilibrium constant, we can ignore it in the expression. Thus, the equation becomes:
Kc = [CaO] * [CO2]
We are given the concentration of CO2 at equilibrium, [CO2] = 0.030 M. However, the concentration of CaO, [CaO], is not provided. Therefore, without the value for [CaO], we cannot determine the exact value of Kc for this reaction.