CHEM 113 Study Guide - Final Guide: Equilibrium Constant, Hydrogen Iodide
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The equilibrium constant, kp, for the reaction described by the equation here is 55. 2 at 425 c. H2 (g) + i2 (g) 2hi (g) A rigid container at that temperature contains 0. 127 atm of hydrogen, 0. 134 atm of iodine, and. Calculate the pressures of all species at equilibrium. Q is larger than k shift left. 55. 2 = (1. 055 - 2x)2 / (0. 127 + x)(0. 134 + x) 55. 2 = (1. 055 2x)(1. 055 2x) / (0. 127 + x)(0. 134 + x) 55. 2 = 1. 113025 4. 22x + 4x2 / 0. 017018 + 0. 261 + x2. 55. 2 (0. 017018 + 0. 261 + x2) = 1. 113025 4. 22x + 4x2. 2h2s (g) 2h2 (g) + s2 (g) Kc = 1. 67 x 10-7 at 800 c. A flask is loaded with 0. 250 m h2s. Calculate the concentrations of all species present once the system has reached equilibrium. 1. 67 x 10-7 = (2x)2(x) / (0. 25 + 2x)2. The shift is essentially 0 for the reactant.
