4. Consider the following exothermic reaction which is used as a source of O2 in some self-contained breathing devices. 4 KO2(s) + 2 CO2(g) + 2 K2CO3(s) + 3 O2(g) The above reaction is at equilibrium in a closed container. For each of the following changes, indicate whether the reaction will proceed towards products, towards reactants, or have no net reaction to reestablish equilibrium. a. CO2(g) is added b. O2(g) is removed C. Some K2CO3(s) is removed d. The temperature is increased e. The reaction is moved to a smaller vessel. f. The pressure in increased by adding N2(g) g. What general conditions of temperature and pressure favor maximum yield of O2(g)?

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Suppose a 500. mL flask is filled with 0.30 mol of SO, and 1.2 mol of SO3. This reaction becomes possible: 2SO, (g) +O,(g) 2SO3 Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity. so, SO2 O2 initial change equilibrium

Assume that the following endothermic chemical reaction is at equilibrium. C(s) + H₂O(g) + H₂(g) + CO(g) Which of the following statements is/are CORRECT? 1. Increasing the concentration of H₂(g) will cause the reaction to proceed in the backward direction, increasing the equilibrium concentration of H₂O(g). 2. Decreasing the temperature will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). 3. Increasing the amount of C(s) will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). All statements are correct. 2 only 3 only 1 only 1 & 2 only