At a particular temperature, KP = 0.25 for the reaction N2O4 (g) ⇌ 2NO2 (g) a. A flask containing only N2O4 at an initial pressure of 5 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. b. A flask containing only NO2 at an initial pressure of 9.0 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. c. From your answers to parts a and b, does it matter from which direction an equilibrium position is reached?

At 35°C, K = 1.8 x 10-5 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. M Q F4 [NOCI] [NO] = M [Cl₂] = M b. 1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask F5 Submit Answer [NOCI] [NO] = [C12] M c. 2.0 mole of NOC1 and 1.0 mole of Cl2 in a 1.0-L flask [NOCI] = M [NO] = [C12] Show Hint A 6 = F6 = = & 7 Retry Entire Group K F7 8 DII FB M M M M 9 more group attempts remaining ( 9 DD F9 0 F10 Previous F11 Next Save and Exit F12

At 900.0 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2SO2 + O2 (g) →2 SO3 (g) At equilibrium, the partial pressure of SO₂ is 33.1 atm and that of O₂ is 15.0 atm. The partial pressure of SO3 is. O 172 O 6.93-10-4 38.0 75.4 O 4.57-10-3 atm.

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.

Consider the following reaction and its equilibrium constant: 12(g) 2 I(g) Kp = 0.209 A reaction mixture contains 0.89 atm 12 and 1.88 atm I. Which of the following statements is TRUE concerning this system? OA. The reaction quotient will decrease. OB. The reaction will shift in the direction of reactants. OC. The system is at equilibrium. D. The reaction will shift in the direction of products. OE. The equilibrium constant will decrease.

At 125°C, Kp = 0.25 for the reaction 2NaHCO3(s) Na2CO3 (s) + CO2 (g) + H2O(g) A 1.00-L flask containing 39.7 g NaHCO3 is evacuated and heated to 125°C. a. Calculate the partial pressures of CO2 and H2O after equilibrium is established. Partial pressure of CO2 = Partial pressure of H2O = atm atm b. Calculate the masses of NaHCO3 and Na2CO3 present at equilibrium. Mass of NaHCO3 = Mass of Na2CO3 g g c. Calculate the minimum container volume necessary for all of the NaHCO3 to decompose. Volume = L

Carbon tetrachloride can be produced by the following reaction: C5₂(g) + 3Cl₂(g) + S₂Cl₂(g) + CCl₂) In an experiment, 0.120 mol of CS₂ and 0.360 mol of Cly were placed in a 1.00-L flask at a particular temperature. After equilibrium has been achieved, the mixture contains 0.040 mol CCl Calculate the value of K under the experimental conditions

Consider the following reaction: PCI5(g) – PCI3(g) + Cl2(g) K, = 23.6 at 500 K a. Calculate the equilibrium partial pressures of the reactants and products if the initial pressures are PPCI, = 0.560 atm and PpCl, = 0.500 atm. b. If more chlorine is added after equilibrium is reached, how will the concentrations of PCls and PC13 change?

Consider the general reaction: 2A(g) + B(g) = 2C(g) If the equilibrium pressures for each substance are: A = 2 atm B = 3 atm C = 1 atm What is the value of K,? None of these are correct. O 0.083 0.16 O 12