If Kc 0.042 for PCI3 (g) + Cl2 (g) = PCIS (g) for at 500 K, what is the value of Kp for this reaction at this temperature? Select one: O a. 1.0x10-5 Ob. 1.0x10-3 O c. 0.042 Od. 4.2x10-3

Consider the following reaction: CO2 (g) + C (graphite) = 2 CO (g) A reaction mixture initially contains 0.83 atm CO, and 0.45 atm CO. Determine the equilibrium pressure of CO if K, for the reaction at this temperature is 4.66.

F5 -5 At 35°C, K = 1.8 x 10 for the reaction 2 NOCI(g) 2 NO(g) + Cl₂ (g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.4 moles of pure NOCI in a 2.0-L flask. [NOCI] = M [NO] = [Cl₂] = = M b. 1.0 mole of NOC1 and 1.0 mole of NO in a 1.0-L flask [NOCI] = [NO] = M [Cl₂] = M c. 2.0 mole of NOCI and 1.0 mole of Cl₂ in a 1.0-L flask [NOCI] = = M [NO] = [Cl₂] Submit Answer 6 Show Hint H F6 & 7 = Retry Entire Group KI F7 * 8 DII FB Topics] K M M 9 M ( M 9 more group attempts remaining D F9 [References] O ) O F10 P J F11 Previous Next Save and Exit F12 delete

46. The following equilibrium pressures were determined for the reaction CO (g) + H₂O (g) PCO = PH20 = 0.44 atm CO₂ (g) + H₂ (g) Pco2 PH2 = 0.556 atm = Calculate dGº for the reaction.

30. For the equilibrium N2O4(g) = 2NO2(g), at 298 K, Kp = 0.15. For this reaction system, it is found that the partial pressure of N,O4 is 3.7 × 10- atm at equilibrium. What is the partial pressure of NO2 at equilibrium? %3D a) 4.9 atm b) 24 atm c) 0.0016 atm d) 0.0055 atm e) 0.074 atm f) none of the above

Which of the following equilibrium systems will shift to the right (toward the products) when pressure isincreased? A. 2 PbS(s) + 3 O2(g) ⇋ 2 PbO(s) + 2 SO2(g)B. PCl5(g) ⇋ PCl3(g) + Cl2(g)C. H2(g) + CO2(g) ⇋ H2O(g) + CO(g)D. All of these will shift to the right.E. None of these will shift to the right.

P4(s)+5 O2(g) P4010(s) Kp = 0.0112 A reaction vessel initially contains 2.5 mol of P4010(s). What is the expression for Kp that would be derived from the ICE table. A. Kp = 2.5 - - x x(5x)5 1 2.5 + x B. Kp = x(5x)5 C. Kp = D. (5x)5 Kp = (5x)5

+60130 11. The reaction SbFs (g) + 4 Cl2 (g) SbCl3 (g) + 5 CIF (g) has an equilibrium constant of 0.02 at 300°C. Portions of the SbFs (g) and Cl2 (g) are mixed at 300°C and each have a partial pressure of 0.12 atm before the reaction. What is the reaction quotient, Q, before the reaction? b a. 0.02 d. 0.12 b. 1 e. 0 4/7 c. 2.5x10-5

4. The atmospheric oxidation of nitrogen monoxide, 2 NO (g) + O2 (g) = 2NO2 (g), was studied at 184°C with initial pressures of 1.00 atm of NO and 1.000 atm of O2. At equilibrium Po,- 0.56 atm. Calculate Kp.

Consider these three reactions and equilibrium constants. Assume all components are gases. 1. C2 20 K1 = 100 wwwww. 2. 2D + D2 K2 = 0.001 3. 2C2 + 2D 4C + D2 K3 =? What is the value for K3 for reaction 3? O 0.1 O 100,000 О 100 O 100.001 O 10