Chloroform (CHCL3) has a normal boiling point of
61 'C and an enthalpy of vaporization of 29.24 kJ/mol. What is the value of delta Gvap (in kJ) at 61'C for chloroform?
I wonder if this is the real problem? Isn't delta G = zero at the boiling point? It would have made more sense to ask for dS vap at the normal boiling point. And how could you calculate dG anyway with no dSvap given?
29.21
To calculate the value of ΔGvap (Gibbs free energy of vaporization) at 61 °C for chloroform (CHCl3), we can use the equation:
ΔGvap = ΔHvap - TΔSvap
where:
- ΔHvap is the enthalpy of vaporization
- T is the temperature in Kelvin
- ΔSvap is the entropy change during vaporization
First, let's convert the temperature to Kelvin:
61 °C + 273.15 = 334.15 K
Next, we need to calculate the entropy change during vaporization (ΔSvap). Unfortunately, we don't have this value, but we can find it using the equation:
ΔSvap = ΔHvap / T
Substituting the values:
ΔSvap = (29.24 kJ/mol) / (334.15 K)
Now we can calculate ΔSvap by converting kJ to J:
ΔSvap = (29.24 × 10^3 J/mol) / (334.15 K)
Finally, we can calculate ΔGvap by substituting the values into the first equation:
ΔGvap = (29.24 × 10^3 J/mol) - (334.15 K) × [(29.24 × 10^3 J/mol) / (334.15 K)]
To get the answer in kJ, divide the result by 1000:
ΔGvap = [(29.24 × 10^3 J/mol) - (334.15 K) × (29.24 × 10^3 J/mol)] / 1000
Please note that the final answer will depend on the exact value of ΔSvap, which was not provided in the question. You can use the given equation and the conversion to calculate the value of ΔGvap.
To find the value of delta Gvap (Gibbs free energy of vaporization) at 61°C for chloroform (CHCl3), we can use the following equation:
ΔGvap = ΔHvap - TΔSvap
Where:
- ΔGvap is the change in Gibbs free energy during vaporization
- ΔHvap is the enthalpy of vaporization
- T is the temperature in Kelvin
- ΔSvap is the change in entropy during vaporization
Before we can plug the values into the equation, we need to convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
Thus, T(K) = 61°C + 273.15 = 334.15 K
Now we can calculate ΔGvap:
ΔGvap = ΔHvap - TΔSvap
Given:
ΔHvap = 29.24 kJ/mol
To find ΔSvap, we need to use the equation:
ΔSvap = ΔHvap / T
ΔSvap = (29.24 kJ/mol) / 334.15 K
Now we can calculate ΔGvap:
ΔGvap = 29.24 kJ/mol - (334.15 K) * [(29.24 kJ/mol) / 334.15 K]
ΔGvap = 29.24 kJ/mol - 29.24 kJ/mol
ΔGvap = 0 kJ/mol
Therefore, the value of delta Gvap at 61°C for chloroform is 0 kJ.