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Calculating Partial Pressures, Given Equilibrium Constant

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The equilibrium constant Kc for the decomposition of phosgene, COCl2, is 4.63 x 10^-3 at 527 deg C.

COCl2(g)<--->CO(g)+Cl2(g)

Calculate the equilibrium partial pressure of all the components, starting with pure phosgene at 0.760 atm

Answer should give partial pressures of COCl2, CO, Cl2.
I do not understand also what is meant by starting with phosgene at 0.760 atm.

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Solution Summary

The solution uses the relevant theoretical equations to solve the problem of finding partial pressures when given the equilibrium constant of the reaction for the decomposition of phosgene and splits up the results into a table of values to better display the thought processes behind the work.

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