Consider the following equilibrium system at 539 K. 2CH2C12 (g) 2 CH, (g) + CCL4 (g) If an equilibrium mixture of the three gases at 539 K contains 4.99 × 10-² M CH2C12, 5.54 × 10-2 M CH4, and 4.90 × 10-2 M CC14, what is the value of the equilibrium constant K?

A gaseous mixture contains 0.27 mol CO, 0.12 mol H2, and 0.022 mol H,O, plus an unknown amount of CH4, in each liter. This mixture is at equilibrium at a certain temperature. CO(9) + 3H, (9) = CH4 (9) + H,O(9) What is the concentration of CH4 in this mixture? The equilibrium constant K, equals 3.99.

At 400 K, an equilibrium mixture of H2, 12, and HI consists of 0.065 mol H2, 0.079 mol 12, and 0.13 mol HI in a 4.50-L flask. What is the value of K, for the following equilibrium? (R= 0.0821 L atm/(K • mol)) 2HI(g) = H2(g) + 12(8) 0.29 8.2 0.039 O 26 3.4

Use the References to access important values if needed for this question. The equilibrium constant, Kc, for the following reaction is 0.0290 at 1150 K. 2SO3 (g) ⇒ 2SO2 (g) + O2 (9) If an equilibrium mixture of the three gases in a 18.0 L container at 1150 K contains 0.356 mol of SO3(g) and 0.469 mol of SO2, the equilibrium concentration of O₂ is M. An error has been detected in your answer. Check for typos,

The following reaction has an equilibrium constant, Kc equal to 3.59 at 900 °C. CH4(g) + 2H₂S(g) — CS2(g) + 4 H2(g) At a particular time during the reaction, the following composition has been found: [CH4(g)] = 1.20 M, [CS2(g)] = 1.15 M, [H₂S(g)] = 1.31 M, [H2(g)] = 1.85. Predict the activity of the reaction during the particular time above. The reaction should go to the left (or reverse) The reaction should go to the right (or forward) The reaction is at a standstill The reaction activity cannot be determined There is no basis for prediction.

At a certain temperature, the equilibrium constant K for the following reaction is ×2.0510−7 : Br2g + OCl2g BrOCl g+BrClg Use this information to answer the following question.   What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K= 3Br2 (g) +3OCl2 (g)   3BrOCl (g) +3BrCl (g

The value of the equilibrium constant is Ke = 0.052 at 600 °C for the reaction: 2 S03 (g) = 2 S02 (g) + 02 (g). Now we mix 0.72-mol SO3, 0.31-mol SO2 (g) and 0.11-mol 02 (g) in a 1-L container. Which of the following statements is (or are) true? a) The reaction will proceed to left (shift to the reactant side) to reach equilibrium. b) The concentration of SO3 will increase during the reaction course. c) The concentration of SO2 will increase during the reaction course. %3! a) only bi only Og only Oa and b) O b) and c) O and a) O a), b) and c) Neither of the 3 statements is true.

The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K.PCl5(g) PCl3(g) + Cl2(g)Calculate the equilibrium concentrations of reactant and products when 0.246 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K. [PCl5] =  M [PCl3] =  M [Cl2] =  M

The equilibrium constant, Kc, for the following reaction is 0.00650 at 298 K. 2NOBr(g) ⇒ 2NO(g) + Br₂ (g) If an equilibrium mixture of the three gases in a 15.6 L container at 298 K contains 0.201 mol of NOBr(g) and 0.284 mol of NO, the equilibrium concentration of Br₂ is | M.

N2(g) +3H2(g) 2NH3 (g) what is the value of K. at 500 °C if the equilibrium concentrations are as follows: H2 = 0.50 M , N2] = 0.60 M , and [NH3] = 2.2 M ? Express the equilibrium constant to two significant figures. ? Ke =