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Pure phosgene gas (COC12), 3.00 × 10–2 mol, was placed in

Chapter 14, Problem 26P

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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

\(\mathrm{CO}(g)+\mathrm{Cl}_{2}(g)\ \leftrightharpoons\ \mathrm{COCl}_{2}(g)\)

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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:

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