The eqm. Constant for a reaction is 2.48 at 25°C. what is the value of ΔG° (kJ) at this temperature? (R=8.314 J/k mol)
To find the value of ΔG° (standard Gibbs free energy change), you can use the equation:
ΔG° = -RT ln(K)
Where:
- ΔG° is the standard Gibbs free energy change
- R is the gas constant (8.314 J/K mol)
- T is the temperature in Kelvin
- K is the equilibrium constant
You are given:
- T = 25°C = 25 + 273.15 = 298.15 K
- K = 2.48 (equilibrium constant)
Thus, substituting the given values into the equation:
ΔG° = - (8.314 J/K mol) * 298.15 K * ln(2.48)
To convert the answer to kJ, divide the result by 1000:
ΔG° = - (8.314 J/K mol) * 298.15 K * ln(2.48) / 1000
Calculating this expression will give you the value of ΔG° in kJ at this temperature.