Consider the following reaction where K. = 83.3 at 500 K: PC13(g) + Cl2(g)=PCl{(g) A reaction mixture was found to contain 2.20x102 moles of PClą(g), 4.34x102 moles of Clh(g) and 0.124 moles of PCl(g), in a 1.00 Liter container.

Part A The equilibrium constant, Kc, for the decomposition of COC2 to CO and Cl2 is 0.68. If an equilibrium mixture contains 0.38 M CÓ and 0.55 M Cl2, what is the molar concentration of COCl2 ? COC2 (g) = CO(g) + Cl2 (g) Express your answer to two significant figures and include the appropriate units.

The equilibrium constant, K., for the following reaction is 83.3 at 500 K. PCI3(g) + Cl2(9)=PCI5(g) Calculate the equilibrium concentrations of reactant and products when 0.242 moles of PCI3 and 0.242 moles of Cl, are introduced into a 1.00 L vessel at 500 K. [PCI3] =| [Cl2] = [PCI5] = M M

Consider the following reaction where K. = 5.10×10-6 at 548 K. NHẠCI(s)ENH3(g) + HCl(g) A reaction mixture was found to contain 5.15x10² moles of NHCI(s), 1.56×103 moles of NH3(g), and 2.26x103 moles of HCI(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)