Pure phosgene gas (COCl2), .03mole, was placed in a 1.5 L container. It was heated to 800k, and at equilibrium the pressure of CO was found to be .497 atm. Calculate the equilibrium constant Kp for the reaction

CO(g) + Cl2(g) = COCL2(g)

Well, looks like we've got a hot situation here! Let's see if my clown brain can calculate the equilibrium constant for this reaction.

The equilibrium constant, Kp, is given by the equation: Kp = (P(COCL2) / (P(CO) * P(Cl2))

In this case, we have the pressure of CO as 0.497 atm. But we need the pressure of COCL2 to calculate Kp.

To find that, we can use the ideal gas law equation: PV = nRT

We know the volume, temperature, and the number of moles of phosgene gas (COCl2) initially at equilibrium. So, we can rearrange the ideal gas law equation to get P(COCL2).

P(COCL2) = (n(COCL2) * R * T) / V

Substituting the values, we have:
P(COCL2) = (0.03 mol * 0.0821 atm L / mol K * 800 K) / 1.5 L.

Now, we can substitute the pressure values into the equation for Kp:
Kp = (0.03 mol * 0.0821 atm L / mol K * 800 K) / (0.497 atm * 1 atm).

Let me grab my calculator... *honk honk*

Calculating...

Kp = 0.3522

So, the equilibrium constant (Kp) for this reaction is approximately 0.3522.

Now, let's hope our clown calculations didn't blow up in our faces!

To calculate the equilibrium constant Kp, we need to use the balanced equation for the reaction and the equilibrium expression.

The balanced equation for the reaction is:
CO(g) + Cl2(g) → COCl2(g)

The equilibrium expression is:
Kp = (P(COCl2) / P(CO) * P(Cl2))

Given information:
- Moles of phosgene gas (COCl2) = 0.03 mole
- Volume of the container = 1.5 L
- Equilibrium pressure of CO = 0.497 atm

First, we need to calculate the equilibrium pressure of COCl2. Since the number of moles of COCl2 is known and the volume is given, we can use the ideal gas law to calculate the pressure:
PV = nRT

Where:
P = pressure
V = volume
n = moles
R = gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)

Rearranging the equation to solve for the pressure:
P = (nRT) / V

Plugging in the values:
P(COCl2) = (0.03 mol * 0.0821 L·atm/(mol·K) * 800 K) / 1.5 L
P(COCl2) = 1.6416 atm

Now, we have the values for P(CO) = 0.497 atm and P(COCl2) = 1.6416 atm. We need to find the value for P(Cl2).

Since the balanced equation shows that the ratio of moles between CO and Cl2 is 1:1, we can assume that the moles of Cl2 at equilibrium are also 0.03 mole.

Using the volume and number of moles, we can calculate the pressure of Cl2 in a similar manner as before:
P(Cl2) = (0.03 mol * 0.0821 L·atm/(mol·K) * 800 K) / 1.5 L
P(Cl2) = 0.4929 atm

Now we have all the values for P(CO), P(Cl2), and P(COCl2).

Substituting these values into the equilibrium expression for Kp:
Kp = (P(COCl2) / P(CO) * P(Cl2))
Kp = (1.6416 atm / 0.497 atm * 0.4929 atm)
Kp = 6.844

Therefore, the equilibrium constant Kp for the reaction CO(g) + Cl2(g) → COCl2(g) is approximately equal to 6.844.

To calculate the equilibrium constant, Kp, for the reaction CO(g) + Cl2(g) ⇌ COCl2(g), you will need to use the information provided about the moles of Phosgene gas (COCl2), the volume of the container, temperature, and the partial pressure of CO at equilibrium.

1. Convert the given number of moles of phosgene gas to the number of moles of CO present at equilibrium. Since the stoichiometric coefficient of COCl2 in the balanced equation is 1, the number of moles of CO present will also be 0.03 moles.

2. Use the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/(mol·K)), and T is the temperature in Kelvin. Rearrange the equation to solve for pressure: P = nRT/V.

3. Substitute the values into the equation: P = (0.03 mol)(0.0821 L·atm/(mol·K))(800 K) / (1.5 L) = 1.315 atm.

4. Use the partial pressure of CO (0.497 atm) at equilibrium and the pressure of CO calculated in step 3 to determine the partial pressure of Cl2 at equilibrium. Since the stoichiometric coefficient of Cl2 is 1, the partial pressure of Cl2 will also be 0.497 atm.

5. Finally, use the partial pressures of CO, Cl2, and COCl2 to calculate the equilibrium constant, Kp, using the expression: Kp = (P(COCl2))/(P(CO) * P(Cl2)).

Substitute the values into the equation: Kp = (0.497 atm)/(1.315 atm * 0.497 atm) = 0.754.

Therefore, the equilibrium constant, Kp, for the given reaction is approximately 0.754.

You can do this either Kc and convert to Kp or you can do it Kp all the way.

initial:
COCl2 = use 0.03 = n and solve PV=nRT for partial pressure COCl2. I get 1.31 atm or something like that. You need to do it more accurately.
CO = 0
Cl2 = 0

equilibrium:
CO: partial pressure = 0.497 atm.
That means Cl2 is 0.497 atm.
COCl2 = 1.31 atm-0.497 = 0.8 something.
Then Kp = P COCl2/PCO*PCl2 = something like 3.0 or so.