Determine the value of the equilibrium constant (Kp) at 800. K and 1 atm pressure.
SbCl3(g) + Cl2(g) -> SbCl5(g)
Delta G(o)f (SbCl5) = -334.34 kJ/mol
Delta G(o)f (SbCl3) = -301.25 kJ/mol
Delta H(o)f (SbCl5) = -394.34 kJ/mol
Delta H(o)f (SbCl3) = -313.80 kJ/mol
I got a K value of 1.14 x 10^3, am I right?
I can't confirm that. Will you post your work?
To determine the value of the equilibrium constant (Kp), you need to use the relationship between ΔG and Kp.
The equation is:
ΔG = -RTln(Kp)
Where:
ΔG is the standard Gibbs free energy change of the reaction
R is the gas constant (8.314 J/mol·K)
T is the temperature in Kelvin
First, convert the temperature from degrees Celsius to Kelvin by adding 273.15:
800 K
Now, plug the values into the equation using the ΔG values given:
ΔG(SbCl5) = -334.34 kJ/mol = -334,340 J/mol
ΔG(SbCl3) = -301.25 kJ/mol = -301,250 J/mol
R = 8.314 J/mol·K
T = 800 K
ΔG = -RTln(Kp)
-334,340 J/mol = -8.314 J/mol·K × 800 K × ln(Kp)
Now, solve for ln(Kp):
ln(Kp) = (-334,340 J/mol) / (-8.314 J/mol·K × 800 K)
ln(Kp) = 50.238
To find Kp, take the exponent of ln(Kp):
Kp = e^(ln(Kp))
Kp = e^(50.238)
Kp = 1.49 × 10^21
Therefore, the correct value of the equilibrium constant (Kp) at 800 K and 1 atm pressure is approximately 1.49 × 10^21.
To determine the value of the equilibrium constant (Kp) at 800 K and 1 atm pressure, you will need to use the equation:
ΔG° = -RTln(Kp)
Where ΔG° is the standard Gibbs free energy change, R is the ideal gas constant (8.314 J/(mol·K)), T is the temperature in Kelvin, and ln denotes the natural logarithm.
First, convert the temperature to Kelvin:
800 K
Next, substitute the values for ΔG°, R, and T into the equation and solve for ln(Kp):
-334.34 kJ/mol = -(8.314 J/(mol·K)) * (800 K) * ln(Kp)
Simplifying the equation, convert kJ to J and solve for ln(Kp):
-334,340 J/mol = -(8.314 J/(mol·K)) * (800 K) * ln(Kp)
Now, divide both sides of the equation by (-8.314 J/(mol·K)) * (800 K) to solve for ln(Kp):
ln(Kp) = -334,340 J/mol / (8.314 J/(mol·K) * 800 K)
ln(Kp) = -50.55
To get the actual value of Kp, we need to take the inverse natural logarithm (exponential function):
Kp = e^(-50.55)
Using a scientific calculator or an online calculator, we find:
Kp = 2.09 x 10^(-22)
Therefore, the correct equilibrium constant (Kp) value at 800 K and 1 atm pressure is 2.09 x 10^(-22), not 1.14 x 10^3 as you calculated.