"Equilibrium Practice Worksheet #1"
Equilibrium Practice Worksheet #1 Solve the following problems using the ICE method. 1. Carbonyl bromide, COBr2, decomposes to CO and Br2 at 73ºC. If you begin with 0.10 moles of COBr2 in a 2.5 Liter flask and find that there are 0.015 moles of COBr2 at equilibrium, calculate the equilibrium concentrations of the products. What is K for this reaction? Is this reaction reactant-favored or product-favored at equilibrium? COBr2 (g) º CO (g) + Br 2 (g) 2. Hydrogen fluoride gas can be formed from hydrogen and fluorine gases according to the balanced equation shown below. At a specific temperature, the equilibrium constant for this reaction is 37.6. What are the partial pressures of all of the gases at equilibrium when the initial partial pressures of hydrogen gas and fluorine gas are 0.600 atm? H2 (g) + F2 (g) º 2 HF (g) 3. Cyclohexane, C6H12, can isomerize (change into a compound of the same formula but different structure) to form methylcyclopentane, C5H9CH3. The equilibrium constant is 0.12 at 25ºC. If the initial concentration of cyclohexane is 0.016 M, what are the concentrations of each gas at equilibrium? C6H12 (g) º C H CH 5 9 3 (g) 4. Nitrogen gas reacts with oxygen gas at high temperature to make nitrogen oxides. This is a major source of air pollution from auto exhaust. At 1500 K, the equilibrium constant for the formation of nitrogen monoxide from its elements is 1.0 x 10-5. Calculate the equilibrium concentration of NO when the initial concentration of N2 is 0.60 M and O2 is 0.30 M. N2(g) + O2(g) º 2 NO(g) 5. The equilibrium constant, Kc, for the following reaction is 5.9 x 10-3 at 250ºC. Suppose 0.17 moles of N2O4(g) is placed in a 5.00 L flask. What is the equilibrium concentration of NO2(g)? Note: solve for x using the approximation method and then check to see if it is a valid approximation. N2O4(g) º 2 NO (g) 2