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, we can use the equation:
ΔG° = -RTln(K)
Where:
ΔG° is the standard Gibbs free energy change in joules (J)
R is the gas constant (8.314 J/K mol)
T is the temperature in Kelvin (K)
K is the equilibrium constant
In this case, we are given that the equilibrium constant (K) is 2.48 and the temperature (T) is 25 degrees Celsius. To convert Celsius to Kelvin, we can use the formula:
T(K) = T(°C) + 273.15
T(K) = 25 + 273.15 = 298.15 K
Substituting the given values into the equation, we have:
ΔG° = - (8.314 J/K mol) (298.15 K) ln(2.48)
To convert the result to kilojoules, we divide the answer by 1000:
ΔG° = (- (8.314 J/K mol) (298.15 K) ln(2.48)) / 1000
Calculating the expression, we get the value of ΔG° in kilojoules (kJ) at this temperature.