The equilibrium constant for the following reaction is 1.80×10-2 at 698K. 2HI(g)H2(g) +I2(g) If an equilibrium mixture of the three gases at 698K contains 2.23×10-2 M HI(g) and 2.22×10-2 M H2, what is the equilibrium concentration of I2?   M

Hydrogen iodide decomposes according to the reaction 2HI(g) = H₂(g) + 1₂ (g) A sealed 1.50-L container initially holds 0.00623 mol of H₂, 0.00414 mol of 1₂, and 0.0244 mol of HI at 703 K. When equilibrium is reached, the concentration of H₂(g) is 0.00524 M. What are the equilibrium concentrations of HI (g) and I₂ (g)? Round each of your answers to 3 significant figures. Part 1 of 2 [HI] = M Part 2 of 2 [¹2]eq = M x10 x10 X x Ś S

Consider the reaction:  4 A (g) + 3 B (g)   2 C (g)  +  5 E (g).   The reaction is initiated with 0.60 M in A, 0.45 M in B and 0.50 M in E.  At equilibrium, the value of  [A] = 0.36 M.  What is the equilibrium value of [E]?

Consider the following reaction where K = 77.5 at 600 K. CO(g) + Cl₂(g) 2 CoCl₂(g) A reaction mixture was found to contain 1.89×10-² moles of CO(g), 4.43×10-² moles of Cl₂(g) and 0.106 moles of COCI₂(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

The equilibrium constant, K, for the following reaction is 3.46x102 at 630 K. COCI₂(g) CO(g) + Cl₂(g) An equilibrium mixture of the three gases in a 11.8 L container at 630 K contains 0.217 M COCI₂, 8.67x10-2 M CO and 8.67x10-2 M Cl₂. What will be the concentrations of the three gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 4.74 L? [COCI₂] = [co] [Cl₂] = M ΣΣ

Consider the following reaction at 400°C and its equilibrium constant: 2 HI(g) - 12(g) + H2(g) Kc = 0.0156 A reaction mixture contains 0.420M I2, 0.420 M H, and 3.36 M HI. Which of the following statements is TRUE? The reaction will shift in the direction of the products. The reaction quotient will decrease. The equilibrium constant will increase. OThe reaction will shift in the direction of the reactants. The system is at equilibrium.

7. Phosgene COCl2 is prepared from CO and Cl₂ CO (g) + Cl₂(g) COC1₂(g) An equilibrium mixture at 395 °C contains 0.012 mol CO and 0.025 mol Cl₂ per liter. If Kc at 395 °C is 1.23 X 10³, what is the concentration of COC1₂?

Consider the following equilibrium system at 817 K. SO2 Cl2 (g) 2 SO2(g) + Cl2 (g) If an equilibrium mixture of the three gases at 817 K contains 1.60 x 10-3 M SO2 Cl2, 3.57 x 10-2 SO2, and 2.12 x 10-2 M Cl2, what is the value of the equilibrium constant К? M K =

The equilibrium constant, K, for the following reaction is 5.10x10 at 548 K. NH4Cl(s) NH3(g) + HCI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.368 mol NH4Cl, 2.26x10-3 M NH₂ and 2.26×10-³ M HCl. If the concentration of HCl(g) is suddenly increased to 3.22×103 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH₂] = [HCI] M M

The equilibrium constant, K, for the following reaction is 1.29×10-2 at 600 K.COCl2 (g)  CO (g) +  Cl2 (g) An equilibrium mixture of the three gases in a 1.00 L flask at 600 K contains 0.285 M COCl2, 6.07×10-2 M CO and 6.07×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.50×10-2 mol of Cl2(g) is added to the flask?