Pure phosgene gas (COCl2), 0.0340 mol, was placed in a 1.50−L container. It was heated to 700.0 K, and at equilibrium, the pressure of CO was found to be 0.509 atm. Calculate the equilibrium constant KP for the reaction. CO(g) + Cl2(g) ⇌ COCl2(g)KP =

The value of for the given equation is 3.065

Explanation:

To calculate the partial pressure of phosgene we use the equation given by ideal gas which follows:

where,

P = pressure of the gas = ?

V = Volume of the gas = 1.50 L

T = Temperature of the gas = 700 K

R = Gas constant =

n = number of moles of phosgene = 0.0340 moles

Putting values in above equation, we get:

As, initially phosgene is present in the system. So, the reaction is going backwards.

We are given:

Equilibrium partial pressure of CO = 0.509 atm

For the given chemical equation:

Initial:                                          1.303

At eqllm:        x            x             1.303-x

Evaluating the value of 'x'

So, equilibrium partial pressure of chlorine gas = x = 0.509 atm

Equilibrium partial pressure of phosgene = 1.303 - x  = [1.303 - 0.509] = 0.794 atm

The expression of for above equation follows:

Putting values in above equation, we get:

Hence, the value of for the given equation is 3.065

that's just how they are

explanation:

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