calculate kp for the reaction below. PCl3(g) + Cl2(g) ⇌ PCl5(g)
How can I calculate it?
btw, K=1.67 (at500A)
To calculate the equilibrium constant, Kp, for the reaction PCl3(g) + Cl2(g) ⇌ PCl5(g), you need to write the equilibrium expression.
The equilibrium expression is written by taking the partial pressures of the products (PCl5) raised to their stoichiometric coefficients and dividing it by the partial pressures of the reactants (PCl3 and Cl2) raised to their stoichiometric coefficients.
The equilibrium expression is:
Kp = (PCl5)^x / (PCl3)^y * (Cl2)^z
In this reaction, since there is only one molecule of each species on both sides of the equation, x = y = z = 1.
So, the equilibrium expression becomes:
Kp = (PCl5) / (PCl3)*(Cl2)
Now, to calculate Kp, you need to determine the partial pressure of each substance at equilibrium. The partial pressure of a substance can be obtained if you know the total pressure and the mole fraction of that substance.
If you have the values for the mole fractions of PCl3, Cl2, and PCl5, as well as the total pressure of the system, you can substitute these values into the equilibrium expression and calculate Kp.
Remember, Kp is only valid if you are dealing with gases. If you are given concentrations instead of partial pressures, you need to convert them to partial pressures using the ideal gas law equation:
PV = nRT
Where:
P = partial pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
By applying these equations and obtaining the needed values for partial pressures or concentrations, you can calculate Kp for the given reaction.