At 25°C, K = 0.090 for the reaction H2O(g) + Cl20(g) = 2 HOCI(9) Calculate the concentrations of all species at equilibrium for each of the following cases. a. 1.0 g H2O and 2.0 g Cl2O are mixed in a 1.0-L flask. [H2O] =| M [Cl½O] =[ M [HOCI] =| M b. 1.0 mole of pure HOC1 is placed in a 2.0-L flask. [H2O] M = [Cl20] = M [HOCI] M

The equilibrium constant, K, for the following reaction is 1.37×10-2 at 503 K. PCl5 (g)  PCl3 (g) +  Cl2 (g) An equilibrium mixture of the three gases in a 13.9 L container at 503 K contains 0.303 M PCl5,   6.44×10-2 M PCl3 and 6.44×10-2 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 6.07 L? [PCl5] =  M [PCl3] =  M [Cl2] =  M

The equilibrium constant, K, for the following reaction is 2.53×10-2 at 519 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 17.8 L container at 519 K contains 0.233 M PCl5,   7.68×10-2 M PCl3 and 7.68×10-2 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 8.95 L? [PCl5] =  M [PCl3] =  M [Cl2] =  M

A sample of HI was placed in a container and the following reaction was allowed to come equilibrium. H₂(g) + 1₂(g) = 2 HI(g) The equilibrium concentrations were found to be [HI] = 3.88 M and [H₂] = [1₂] = 0.556. Calculate the equilibrium const Kc, for the reaction. Note Kc is often called K.

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

Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 3.0 L reaction vessel contained a mixture of 1.37 x 10-2 M HI, 6.47 × 10-3 M H2, and 5.94 × 10-4 M I, at 740 K. What are the values of Kc and Kp for the reaction at this temperature? H2(g) + 12(g) = 2 HI(g) 1 NEXT > Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms. K. = 2 RESET [1.37 x 10-2] [6.47 x 10-3] [5.94 × 10-4] [4.57 × 10-3] [2.16 х 10-3] [2.31 x 10-4] 2[1.37 x 10-2] 2[6.47 x 10-3] 2[5.94 x 10-4] [1.37 х 10-7)2 [6.47 x 10-312 [5.94 x 10-4]2 3.56 x 103 2.81 × 10-4 48.8 2.05 x 10-2

CO(g) + H₂O(g) ⇒ H₂(g) + CO₂(g) K = 7.3@823 K A closed 5.0 L container initially holds 3.0 moles CO and 6.0 moles H2O. Calculate the concentrations of each material at equilibrium. What is the equilibrium concentration of H₂O? [H₂O] = [?] M

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.

At 25°C, K= 0.090 for the reaction H20(g) + Cl20(9) = 2 HOCI(9) Calculate the concentrations of al1 species at equilibrium for each of the following cases. a. 1.0 g H20 and 2.0 g Cl2 0 are mixed in a 1.0-L flask. [H2O] =| M [CL,0] = M [HOC1] = M b. 1.2 mole of pure HOCI is placed in a 2.0-L flask. [H2O] = M [Cl20] = M %D [HOCI] = M

Determine the concentration of all species at equilibrium for each of the following original mixtures. At 40C K= 1.7*10^-5 2NOCl(g) ——-(reversible)—— 2NO(g) + Cl2(g) a) 2moles of NOCl 2 moles of NO 1 mole or Cl2 in 1.0L flask b) 1M concentration of all three gases