For the reaction Cl2(g)<-> 2Cl)g) Kp=2.45*10^-7 at 1000K. What is delta G (degrees) for this reaction at 1000K?
To determine the delta G (Gibbs free energy) for the reaction at 1000K, we need to use the equation:
ΔG = -RTln(Kp)
Where:
ΔG = Gibbs free energy change
R = Ideal Gas Constant (8.314 J/mol·K)
T = Absolute temperature in Kelvin
ln = Natural logarithm
Kp = Equilibrium constant (given as 2.45 * 10^-7)
Now, let's substitute the values into the equation and solve for ΔG:
ΔG = -(8.314 J/mol·K)(1000 K) × ln(2.45 × 10^-7)
First, calculate the natural logarithm:
ln(2.45 × 10^-7) ≈ -15.91
Substituting the values:
ΔG = -(8.314 J/mol·K)(1000 K) × (-15.91)
Calculating:
ΔG = 132,032 J/mol
Therefore, the delta G (degrees) for this reaction at 1000K is approximately 132,032 J/mol.
delta Go = -RT*lnK
You want to use 8.314 for R.