The equilibrium constant kc for the decomposition of phosgene, cocl2, is 4.63x10^-3 at 527 c. calculate the equilibrium partial pressure of all the components, starting with pure phosgene at 0.760 atm

The partial pressure of the are 0.352 atm, 0.352 atm and 0.408 atm respectively.

Explanation:

We are given:

Relation of with is given by the formula:

Where,

= equilibrium constant in terms of partial pressure = ?

= equilibrium constant in terms of concentration =

R = Gas constant =

T = temperature =

= change in number of moles of gas particles =

Putting values in above equation, we get:

The chemical reaction for the decomposition of phosgene follows the equation:

At t = 0          0.760            0     0  

At      0.760-x          x      x

The expression for for the given reaction follows:

We are given:

Putting values in above equation, we get:

Negative value of 'x' is neglected because partial pressure cannot be negative.

So, the partial pressure for the components at equilibrium are:

Hence, the partial pressure of the are 0.352 atm, 0.352 atm and 0.408 atm respectively.

do u have any choices to choose from ? ?

sorry i was late, but i don't know what assignment your talking about, i'm in flvs as well, im in earth space science. but u are behind pace bc every class should be in the 3's or 4'