Using ƒ´Hfo and So values, calculate the standard molar free energy of formation for
each of the following:
a. CuSO4(s)
b. ZnSO4(s
To calculate the standard molar free energy of formation for each compound, we need to use the equation:
ΔG°f = ΔH°f - TΔS°
where:
ΔG°f = standard molar free energy of formation
ΔH°f = standard molar enthalpy of formation
T = temperature in Kelvin
ΔS° = standard molar entropy of formation
a. CuSO4(s):
To find the ΔH°f and ΔS° values for CuSO4(s), you can refer to a reliable source such as a thermodynamics database or handbook. Let's assume the values are:
ΔH°f = -769 kJ/mol
ΔS° = 239 J/(mol·K)
Now, let's assume the temperature is 298 K:
ΔG°f = (-769 kJ/mol) - (298 K) * (0.239 kJ/(mol·K))
ΔG°f = -769 kJ/mol - 71.362 kJ/mol
ΔG°f = -840.362 kJ/mol
Therefore, the standard molar free energy of formation for CuSO4(s) is -840.362 kJ/mol.
b. ZnSO4(s):
Similarly, you will need to find the ΔH°f and ΔS° values for ZnSO4(s) and then substitute them into the equation. Assuming the values are:
ΔH°f = -983 kJ/mol
ΔS° = 193 J/(mol·K)
Using the same temperature of 298 K:
ΔG°f = (-983 kJ/mol) - (298 K) * (0.193 kJ/(mol·K))
ΔG°f = -983 kJ/mol - 57.514 kJ/mol
ΔG°f = -1040.514 kJ/mol
Therefore, the standard molar free energy of formation for ZnSO4(s) is -1040.514 kJ/mol.