Solution Found!
Pure phosgene gas (COC12), 3.00 × 10–2 mol, was placed in
Chapter 14, Problem 26P(choose chapter or problem)
Pure phosgene gas \(\left(\mathrm{COCl}_{2}\right)\), \(3.00 \times 10^{-2}\) mol, was placed in a 1.50-L container. It was heated to 800 K, and at equilibrium the pressure of CO was found to be 0.497 atm. Calculate the equilibrium constant \(K_{P}\) for the reaction
\(\mathrm{CO}(g)+\mathrm{Cl}_{2}(g)\ \leftrightharpoons\ \mathrm{COCl}_{2}(g)\)
Questions & Answers
QUESTION:
Pure phosgene gas \(\left(\mathrm{COCl}_{2}\right)\), \(3.00 \times 10^{-2}\) mol, was placed in a 1.50-L container. It was heated to 800 K, and at equilibrium the pressure of CO was found to be 0.497 atm. Calculate the equilibrium constant \(K_{P}\) for the reaction
\(\mathrm{CO}(g)+\mathrm{Cl}_{2}(g)\ \leftrightharpoons\ \mathrm{COCl}_{2}(g)\)
ANSWER:Step 1 of 2
Given that phosgene gas has a volume of 1.50 L at a temperature of 800 K. So, we can calculate the pressure of phosgene gas using the equation,
Here,
Thus, the pressure of is: