University:
University of Ottawa
Course:
CHM1321 | Organic Chemistry I
Academic year:

2024
Views:

162

Pages:

4
Author:

Noodle D.

NOV 15: PRINCIPLES OF CHEMICAL EQUILIBRIUM 14.9 - Write the equilibrium constant expression for each of the following reactions a. I! (s) + 5 F! (g) ⇌ 2 IF% (g) b. BaCO$ (s) + C (s) ⇌ BaO (s) + 2 CO (g) c. CO (g) + 2 H! (g) ⇌ CH$ OH (l) & d. H$ PO# (aq) + 3 H! O (l) ⇌ PO$" # (aq) + 3 H$ O (aq) 14.11 - Write each of the chemical reactions of Problem 14.9 in the opposite direction and determine the equilibrium constant expressions for these reactions. 14.25 - For each equilibrium presented below, predict the effect of injecting additional CO(g) into the system. a. CO (g) + H! O (l) ⇌ CO! (g) + H! (g) b. 2 CO (g) + O! (g) ⇌ 2 CO! (g) c. BaCO$ (s) + C (s, graphite) ⇌ BaO (s) + 2 CO (g) d. 3 CO (g) + 6 H! (g) ⇌ C$ H' (g) + 3 H! O (l) 14.31 - An industrial chemist puts 1.00 mole each of H2 (g) and CO2 (g) in a 1.00 L container at constant temperature of 800 °C. This reaction occurs H! (g) + CO! (g) ⇌ H! O (g) + CO (g) When equilibrium is reached, 0.49 mole of CO (g) is in the container. Find the value of Keq. 14.33 - When 0.0500 mol of propanoic acid (C2H5CO2H) is dissolved in 0.500 L of water, proton transfer occurs: & C! H% CO! H + H! O ⇌ C! H% CO" ! + H$ O The equilibrium concentration of H3O+ ions is 1.15 x 10−3. Evaluate Keq. 14.37 - At 1000 °C, Keq = 0.403 for the following reaction FeO (s) + CO (g) ⇌ Fe (s) + CO! (g) If CO gas at 5.0 bar is injected into a container at 1000 °C that contains excess FeO, what are the partial pressures of all gases present at equilibrium? 14.38 - Keq for the Haber reaction is 2.81 x 10−5 at 472 °C. If a reaction starts with 3.0 bar of H2 and 5.0 bar of N2 at 472 °C, what is the equilibrium pressure of NH3? 14.82 - A key step in the synthesis of sulphuric acid is the combustion of SO2 to give SO3: 2 SO! (g) + O! (g) ⇌ 2 SO$ (g) K () = 5.60 x 10# at 350 °C SO2 and oxygen are mixed initially at 0.350 bar and 0.762 bar, respectively, at 350 °C. What are the partial pressures of the three gases when the mixture reaches equilibrium? For this question, using the mol amounts instead of pressure would also get you the correct answer because all the units cancel out. This won’t always be the case though (hence why I converted mols into pressures)! PA = propanoic acid When Keq is small/large, any x values that are being added or subtracted can be removed First table is done to find out how much of each chemical is left at the end of the reaction Second table is done to find the equilibrium amounts after the reaction goes to completion (hence why products are consumed and reactants are formed)