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 calculate the value of ΔG° (standard Gibbs free energy change) at a given temperature using the equilibrium constant (K), we can use the equation:
ΔG° = -RT ln(K)
Where:
ΔG° is the standard Gibbs free energy change (in kJ),
R is the gas constant (8.314 J/mol·K),
T is the temperature in Kelvin,
ln is the natural logarithm function,
K is the equilibrium constant.
In this case, we are given the equilibrium constant (K = 2.48) and the temperature (25°C = 298 K).
Now, substituting the given values into the equation:
ΔG° = - (8.314 J/mol·K) * 298 K * ln(2.48)
To get the result in kJ, we need to convert from J to kJ:
ΔG° = - (8.314 J/mol·K) * 298 K * ln(2.48) / 1000
Calculating this expression:
ΔG° ≈ -2.62 kJ
Therefore, the value of ΔG° at a temperature of 25°C is approximately -2.62 kJ.