A chemist wants to prepare phosgene, COCl2, by the following reaction:

He places 4.00 g of chlorine, Cl2, and an equal molar amount of carbon monoxide, CO, into a 10.00-L reaction vessel at 395oC. After the reaction comes to equilibrium, he adds another 4.00 g of chlorine to the vessel in order to push the reaction to the right to get more product. What is the partial pressure of phosgene when the reaction again comes to equilibrium? Kc = 1.23× 103.

Transcribed Image Text:

Co(g) + Cl2(g) = COCI,(g)