Solution Found!
Answer: The equilibrium constant Kc for the decomposition
Chapter 14, Problem 45P(choose chapter or problem)
The equilibrium constant \(K_{c}\) for the decomposition of phosgene, \(\mathrm{COCl}_{2}\), is \(4.63 \times 10^{-3}\) at \(527^{\circ} \mathrm{C}\):
\(\mathrm{COCl}_{2}(g)\ \leftrightharpoons\ \mathrm{CO}(g)+\mathrm{Cl}_{2}(g)\)
Calculate the equilibrium partial pressure of all the components, starting with pure phosgene at 0.760 atm.
Questions & Answers
QUESTION:
The equilibrium constant \(K_{c}\) for the decomposition of phosgene, \(\mathrm{COCl}_{2}\), is \(4.63 \times 10^{-3}\) at \(527^{\circ} \mathrm{C}\):
\(\mathrm{COCl}_{2}(g)\ \leftrightharpoons\ \mathrm{CO}(g)+\mathrm{Cl}_{2}(g)\)
Calculate the equilibrium partial pressure of all the components, starting with pure phosgene at 0.760 atm.
ANSWER:Step 1 of 3
The given reaction is as follows;
The partial pressure constant of the reaction will be;
...............(1)