I really need this please!!!!!!! :
write the equilibrium-constant expression and calculate the value of the equilibrium constant for each of the following reactions at 298 K.
(a) NaHCO3(s)<--> NaOH(s) + CO2(g)
Answer: Keq = PCO2
(b)Value of the Equilibrium Constant:
Please help me find B
........ deltaHf(KJ/mol)...... d.Gf(KJ/mol)..... d.S(J/mol-K)
NaHCO3(s) -947.7...... -851.8 ......... 102.1
NaOH(s).. -425.6 ...... -379.5 ........ 64.46
CO2(g) .. -393.5 ...... -394.4 ........ 213.6
dGo = -RTlnK
You should be able to get dGo from
dGorxn = (n*dGof products) - (n*dGof reactants)
To find the equilibrium constant expression and calculate the value of the equilibrium constant for each reaction, you need to use the standard Gibbs free energy change (ΔG°) values.
(a) For the reaction NaHCO3(s) ↔ NaOH(s) + CO2(g):
1. The equilibrium constant expression (Keq) can be written as the ratio of the product concentrations raised to their stoichiometric coefficients divided by the reactant concentration raised to its stoichiometric coefficient:
Keq = [CO2]
Since NaHCO3 and NaOH are solids, they do not contribute to the equilibrium constant expression.
2. To calculate the value of Keq, you need to use the ΔG° values. The ΔG° for the reaction can be calculated using the formula:
ΔG° = ΣnΔGf°(products) - ΣmΔGf°(reactants)
where Σn is the sum of the stoichiometric coefficients of the products and Σm is the sum of the stoichiometric coefficients of the reactants.
In this case, the reaction is:
NaHCO3(s) ↔ NaOH(s) + CO2(g)
ΔG° = ΔGf°(NaOH) + ΔGf°(CO2) - ΔGf°(NaHCO3)
ΔG° = (-379.5 KJ/mol) + (-394.4 KJ/mol) - (-851.8 KJ/mol) = 77.9 KJ/mol
3. Since ΔG° = -RT ln(Keq), where R is the gas constant (8.314 J/(mol·K)), and T is the temperature in Kelvin (298 K), we can rearrange the equation to solve for Keq:
Keq = e^(-ΔG°/RT)
Substituting the values:
Keq = e^(-77900 J / (8.314 J/(mol·K) * 298 K))
Keq ≈ e^(-31.21) ≈ 1.362
So, the equilibrium constant (Keq) for the reaction NaHCO3(s) ↔ NaOH(s) + CO2(g) is approximately 1.362, and the equilibrium constant expression is Keq = [CO2].
(b) It seems that there is missing information for part B. The values you provided appear to be the enthalpy of formation (ΔHf), Gibbs free energy of formation (ΔGf), and entropy (ΔS) for the reactants and products. If you can provide the reaction equation for part B, I can help you calculate the equilibrium constant.