Question

October 16, 2019 Problem Set 12 CHEM 1252 5. Each part below refers to the balanced equation shown. 2CH(R) + 2H2O(g) 4HCI(R) + O2(g) (a) If you start with only reactants and no products. tell whether the total pressure will increase, decrease, or stay the same as the reaction approaches equilibrium, and explain why. (b) Under certain conditions at equilibrium, the total pressure is 0.81 bar, and the mole fractions for each gas are: 2/9 (Cla); 2/9 (H2O); 4/9 (HCI); and 1/9 (O). Calculate k. 6. The equilibrium constant for the reaction in question 2c is k = 721 M-1 (a) Assuming this reaction is at equilibrium, calculate (1") when (1) - [13"] = 0.0010 M. (b) Assuming this reaction is at equilibrium, find [13] when [12] = 0.0025 M and [14] -0.010 M. (c) Assuming this reaction is at equilibrium, find [12] when (13") = 0.00030 M and [1") - 0.10 M. (d) Before the reaction reaches equilibrium, a solution has [1] = 0.0020 M, and [19 [12] OM Calculate the concentrations of all three species after the solution reaches equilibrium. (Assume that x M of triiodide dissociates to iodide and lodine, and solve for x.)

Answer 1

6 2 + 2H₂O the to atto l h oo P, -2x P.-2x ya Petal pressure at any time = P - 2n+P2-21 tinta - Pithara 2 Total pressure increase (b) nalla P2 - 2x = 399 P, -2x = 2 PPP, PP. 1- Pit le telz= P = 0.81 yaxa kp= 18, 24) (P2 - 297 - 2% × 29/9