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
To calculate the equilibrium constant (Keq) for a given reaction, you need to write the equilibrium-constant expression and then determine the value of Keq. Here's how you can do it for each of the reactions:
(a) The balanced equation for the reaction is:
NaHCO3(s) ⇌ NaOH(s) + CO2(g)
The equilibrium-constant expression can be written using the concentrations or partial pressures of the products and reactants. In this case, as the reaction involves a solid (NaHCO3(s)), its concentration does not change, so it is not included in the expression. The expression only considers the partial pressure of CO2, denoted as PCO2:
Keq = PCO2
To calculate the value of Keq at 298 K, you would need to determine the partial pressure of CO2 at equilibrium. This value can be obtained from the given conditions or by carrying out experiments.
(b) Unfortunately, you haven't provided any specific reaction for part (b). To find the equilibrium constant value for a reaction, you would need the balanced equation for the reaction. Once you have the equation, you can follow the steps mentioned in part (a) to obtain the equilibrium-constant expression and calculate the value of Keq.
If you provide the balanced equation for the reaction in part (b), I can assist you further in calculating the equilibrium constant.
You don't have enough information posted.
........ 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
Hope that helps
dGo= -RTlnK
You should be able to get dGo from
dGorxn = (n*dGof products) - (n*dGof reactants)