A mixture of 2.75e-02 mol of O3, 4.32e-02 mol of NOCI, 7.25e-02 mol of NO, and 7.59e-03 mol of Cly is placed in a 1.0-L steel pressure vessel at 1654 K. The following equilibrium is established: O;(9) + 2 NOCI(9) =2 NO(9) + Ch(9) At equilibrium 6.0le-03 mol of Clz is found in the reaction mixture. Calculate the equilibrium pressures of all gases in the reaction vessel and the value of Kp for the reaction. Pick the correct statement from the multiple choices, Use the value R= 0.0821 L-atm/mal-K for the gas constant. Oa) The equilibrium pressure of NOCI is Pyoo-6.29 atm. O b) The equilibrium pressure of O2 is Po, - 3.52 atm. O) The equilibrium constant is Kp 9.2e-02. O) The equilbnum constant is Kp 2.2e+00. O e) The equilibrium pressure of NO, is PNo, 10.3 atm.

A mixture of 0.01076 mol of Cl₂, 0.04718 mol of H₂0, 0.02718 mol of HCI, and 0.01676 mol of O₂ is placed in a 1.0-L steel pressure vessel at 1846 K. The following equilibrium is established: 2 Cl₂(g) + 2 H₂O(g) = 4 HCl(g) + 1 O₂(g) At equilibrium 0.001782 mol of Cl₂ is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of Cl₂, H₂O, HCl, and 0₂. Peq(Cl₂)= Peq(H₂O) = Peq (HCI) Peq(O₂) = = (b) Calculate Kp for this reaction. Kp =

The equilibrium constant, K. for the following reaction is 77.5 at 600 K. Co(g) + C,(g)=cOC»(g) Calculate the equilibrium concentrations of reactant and products when 0.231 moles of CO and 0.231 moles of Cl, are introduced into a 1.00 L vessel at 600K. [CO] M [CL] M [COCL] =| M

A mixture of 0.06529 mol of CH4, 0.04045 mol of H2S, 0.06585 mol of CS2, and 0.03325 mol of H2 is placed in a 1.0-L steel pressure vessel at 1304 K. The following equilibrium is established:   1 CH4(g) + 2 H2S(g)  1 CS2(g) + 4 H2(g)Peq   the equilibrium partial pressures of CH4, H2S, CS2, and H2. (CH4) =  7.5Peq(H2S) = 5.35Peq(CS2) = 6.42Peq(H2) =   1.5195   At equilibrium 0.01420 mol of H2 is found in the reaction mixture. Calculate KP for this reaction.KP = _____  .

At 25°C, the equilibrium constant for the reaction Blg) + Clg) 2A(3) is K,-0.0735.If the three gases are mixed in a rigid container having partial pressuros of 3.35, 185 and 0.693 atm for A, B and C, respectively, is the system at equilibrium? The system is at equilibrium. The reverse reaction must proceed to establish equilibrium. The volume of the container must be known to answer the question. The concentrations of all substances must be known to answer the question. The forward reaction must praceed to establish equilibrium,

14.71 Suppose 1.000 mol CO and 3.000 mol H2 are put in a 10.00-L vessel at 1200 K. The equilibrium constant K, for CO(g) + 3H2(g) CH4(g) + H2O(g) equals 3.92. Find the equilibrium composition of the reac- tion mixture.

A reaction is prepared by adding 2.000 mol each of H2, 12, and HI gases to a 1.0 L container. They are allowed to come to equilibrium, following the reaction: H2 (g) + I2(9) = 2HI(g) At the steady-state, 0.743 mol of HI remained in the container. What is the equilibrium constant Kc for this reaction under these conditions?

The equilibrium constant Kc for the reaction,I2(g) + Br2(g) <-----> 2 IBr(g)is 314.7 at 425 K. What is the value of Kc for the equilibrium,1/2 I2(g) + 1/2 Br2(g) <-----> IBr(g)at 425 K?

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

A mixture of 0.04289 mol of C2H4, 0.08501 mol of N2, 0.02401 mol of NH3, and 0.05848 mol of C6H6 is placed in a 1.0-L steel pressure vessel at 1258 K. The following equilibrium is established: 3 C2H4(g) + 1 N2(g)  2 NH3(g) + 1 C6H6(g) At equilibrium 0.005819 mol of NH3 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of C2H4, N2, NH3, and C6H6.Peq(C2H4) =  .Peq(N2) =  .Peq(NH3) =  .Peq(C6H6) =  .(b) Calculate KP for this reaction.KP =  .