Consider the following reaction: 2SO3(g) =2SO2(g) + O2(g) If 0.313 moles of SO3(g), 0.562 moles of SO2, and 0.642 moles of 02 are at equilibrium in a 19.8 L container at 1.23×10° K, the value of the equilibrium constant, Kc, is

6) A mixture of 9.00 moles of A, 10.00 moles of B, and 28 moles of C is placed in a one liter container at room temperature. The reaction is allowed to reach equilibrium at which point the number of moles of B is 18.00. Calculate the equilibrium constant, Kc, for this reaction: A (g) + 2 B (g) « 3 C (g)​​​​Kc = ?

Suppose a 250. mL flask is filled with 0.60 mol of Br₂, 1.9 mol of BrOCI and 1.3 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOC1 (g) + BrC1 (g) The equilibrium constant K for this reaction is 1.98 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.

In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g) = CO, (g) + H2 (g) In an experiment, 0.35 mol of CO and 0.40 mol of H20 were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.16 mol of CO remaining. Keq at the temperature of the experimnent is

Suppose a 250. mL flask is filled with 0.30 mol of O, and 1.5 mol of NO. This reaction becomes possible: N, (g) +0,(g) = 2NO(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. alo Ar N2 O2 NO initial change equilibrium

3. If the equilibrium constant K, for the reaction 2 NO (g) + O2(g) = 2 NO2 (g) is 5.0 x 1012 at a given temperature, what is the value of the equilibrium constant K, for each of the following reactions at the same temperature? a) NO (g) + ½ O2 (g) → NO2 (g) b) 2 NO2 (g) = 2 NO (g) + 02 (g) c) NO2(g) = NO (g) + ½ 02 (g)

Suppose a 250. mL flask is filled with 1.9 mol of O, and 1.5 mol of NO. The following reaction becomes possible: N2 (g) +0,(g) =2NO(g) The equilibrium constant K for this reaction is 8.51 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. OM

For the reaction 2 NO2 (g) <=> N2O4 (g),  K= 0.67. If [NO2] = 2.0 M, and the [N2O4] = 1.0 M  , which of the following is true?     The reaction is at equilibrium     The reaction will move to the reactant side     The reaction cannot reach equilibrium     The reaction will move to the product side

Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g)  2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. The equilibrium will not shift The equilibrium will shift toward product but Keq will not change The equilibrium will shift toward reactant but Keq will not change The equilibrium will shift toward product but Keq will will increase         The equilibrium will shift toward reactant but Keq will decrease(b) The reaction mixture is cooled.        (c) The volume of the reaction vessel is reduced by 50%.

Consider the following reaction: 2CH₂Cl2 (9) ⇒ CH4 (9) + CCl4 (9) If 0.436 moles of CH₂Cl2 (g), 0.335 moles of CH4, and 0.406 moles of CC14 are at equilibrium in a 17.4 L container at 599 K, the value of the equilibrium constant, Kc, is