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° (kJ) at a given temperature, we need to 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, and
K is the equilibrium constant.
In this case, the equilibrium constant (K) is given as 2.48, and the temperature (T) is 25°C, which needs to be converted to Kelvin.
To convert from Celsius to Kelvin, we add 273.15 to the Celsius value:
T(K) = 25°C + 273.15 = 298.15 K
Plugging in the values into the equation:
ΔG° = - (8.314 J/K mol) * 298.15 K * ln(2.48)
Now, we need to convert the result from Joules (J) to kilojoules (kJ). Since 1 kJ = 1000 J, we divide the result by 1000:
ΔG° (kJ) = (-8.314 J/K mol * 298.15 K * ln(2.48)) / 1000
Calculating this expression gives us the value of ΔG° at 25°C in kilojoules (kJ).