when 8.4 mol of PCl5 (g) is mixed with 1.8 mol of PCl3 (g) and allowed to come to equilibrium in a 10 dm3container the amount of PCl5 (g) at equilibrium is 7.2 mol.     Kc =   (b) Explain the effect of the following changes below on the value of Kc:   Increasing temperature   Lowering the concentration

For this equilibrium system, 2SO3(g) 2 25O2(g) + O2(g), Kc = 0.00407. At equilibrium, you would expect to find %3D relatively more products than reactant. relatively more reactant than products. about comparable amounts of reactant and products. no way to decide.

2. According to Le Chatelier's principle, it indicates where the balance is favored (Reactants or products) of the following unbalanced reaction H₂O(a) + Fe(s) + H₂(g) + Fe3O4(s) + Heat Write your answer on the line a) Decreases ia [H2): b) The temperature of the system decreases: c) The system pressure increases:

Km.201.

Consider the following reversible reaction at equilibrium: C6H12O6(aq) + 6 O2(g)      6 CO2(g) + 6 H2O(l). Given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?

(a) Calculate K at 298 K for the following reaction: NO(g) + O₂(g) → NO₂(g) 1 2 K= = kJ AG (M) fmol 86.60 NO(g) NO₂(g) 51 O₂(g) 0 x 10

Calculate Kc for the following equilibrium: 2SO2(g) + O2(g) ⇌ 2SO3(g);            Kp = 2.5 × 1010 at 4.5 × 102 K.

Calculate the value of Kp for the equation C(s) + CO₂(g) 2 CO(g) given that at a certain temperature Kp Kp = ? C(s) + 2 H₂O(g)CO₂(g) + 2 H₂(g) H₂(g) + CO₂(g) H₂O(g) + CO(g) Kpl = 3.13 Kp2 = 0.625

At -8.64 °C the concentration equilibrium constant K = 7.7 for a certain reaction. Here are some facts about the reaction: -1 • The initial rate of the reaction is 5.3 mol·L¯¹·s¯¹. . If the reaction is run at constant pressure, 132. kJ/mol of heat are absorbed. • The constant pressure molar heat capacity C = 2.97 J'mol K¹. Yes. Using these facts, can you calculate K at 16. °C? x10 O No. If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat 16. °C will be bigger or smaller than K at -8.64 °C? C Yes, and K will be bigger. Yes, and K will be smaller. No.

The equilibrium constant for the following reaction is 67.6 at 232 °C. PCI 3(g) + Cl₂(g) PCI5(g) K = 67.6 at 232 °C Calculate the equilibrium constant for the following reactions at 232 °C. (a) PCI5(g) PCl3(g) + Cl₂(g) K= (b) 2 PCI5(g) 2 PCI3(g) + 2 Cl₂(g) K=