1.30 mol each of CO} and Cl2 are introduced into an evacuated 1.80 L flask, and the following equilibrium is established at 668 K.
CO + Cl2 +++> COCl2 kp = 22.5
Calculate partial pressure of COCl2. i get about 30.9. but its wrong. i solved for x, COCL2/CO*Cl2, using ICE formula, converted everything to molarity, then to moles, then using ideal gas law. still cant get it.
To calculate the partial pressure of COCl2, you need to follow these steps:
Step 1: Convert the initial amounts of CO and Cl2 to moles.
Given:
Number of moles of CO = 1.30 mol
Number of moles of Cl2 = 1.30 mol
Step 2: Use the ICE (Initial-Change-Equilibrium) method to determine the change in the number of moles of COCl2. The balanced equation for the reaction is:
CO + Cl2 ↔ COCl2
The stoichiometry of the reaction is 1:1, so the change in moles of COCl2 will be "x" (assuming it is the same as the change in moles of CO and Cl2).
Step 3: Determine the equilibrium amount of COCl2.
Since the initial number of moles of COCl2 was zero and the change in moles is "x," the equilibrium number of moles of COCl2 will be "x."
Step 4: Convert the number of moles of COCl2 to concentration.
To convert from moles to concentration, divide the number of moles by the volume in liters.
Given:
Volume of flask = 1.80 L
Equilibrium amount of COCl2 = x
Concentration of COCl2 (in Molarity) = x / 1.80
Step 5: Convert the concentration of COCl2 to partial pressure.
Use the ideal gas law equation to convert concentration to partial pressure.
P = nRT / V
Given:
Temperature (K) = 668 K
Volume (L) = 1.80 L
R (the ideal gas constant) = 0.0821 L·atm/(mol·K)
Partial pressure of COCl2 = (x / 1.80) * 0.0821 * 668
By solving these equations, you can find the partial pressure of COCl2. Make sure to substitute the value of "x" obtained from the ICE table into the appropriate equation.