THE EQUILIBRIUM CONSTANT FOR A REACTION IS 2.48 AT 25 DEGREES CELSIUS. 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) in kilojoules (KJ) at a given temperature, 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
However, in order to use this equation, we need to convert the temperature from degrees Celsius to Kelvin using the formula:
T(K) = T(°C) + 273.15
Let's calculate ΔG° at 25 degrees Celsius:
1. Convert the temperature from degrees Celsius to Kelvin:
T(K) = 25°C + 273.15 = 298.15 K
2. Plug the values into the equation:
ΔG° = - (8.314 J/K mol) * 298.15 K * ln(2.48)
3. Calculate ΔG°:
ΔG° = - (8.314 J/K mol) * 298.15 K * ln(2.48) = - 6169.01 J ≈ - 6.169 KJ
Therefore, the value of ΔG° at 25 degrees Celsius is approximately -6.169 KJ.