This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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6.5 6.5.1 The value of K_c. The equilibrium constant K_c is only affected by temperature. Since the temperature is kept constant at 600 °C, the value of K_c will not change. REMAINS THE SAME 6.5.2 The mass of Cl_2(g) in the container. Decreasing the volume of the container increases the pressure. The equilibrium will shift to the side with fewer moles of gas. Reactants: 4HCl(g) + O_2(g) (5 moles of gas) Products: 2H_2O(g) + 2Cl_2(g) (4 moles of gas) Since the product side has fewer moles of gas, the equilibrium will shift to the right, favoring the formation of products, including Cl_2(g). INCREASES 6.6 Explain the answer to QUESTION 6.5.2 by referring to Le Chatelier's Principle. When the volume of the container is decreased, the total pressure of the system increases. According to Le Chatelier's Principle, the equilibrium will shift in the direction that reduces the number of moles of gas to counteract this increase in pressure. In the given reaction, the product side has 4 moles of gas, while the reactant side has 5 moles of gas. Therefore, the equilibrium shifts to the right (towards the products), leading to an increase in the concentration and thus the mass of Cl_2(g). 6.7 6.7.1 Is the heat of the forward reaction, ( H), POSITIVE or NEGATIVE? The temperature was increased, and the value of K_c increased from 81 (from previous context) to 450. An increase in K_c indicates that the equilibrium shifted to the right (towards products). According to Le Chatelier's Principle, an increase in temperature favors the endothermic reaction. Therefore, the forward reaction is endothermic. POSITIVE 6.7.2 Explain the answer to QUESTION 6.7.1 by referring to Le Chatelier's Principle. When the temperature of the container is increased, the equilibrium shifts to counteract this change. Since the value of K_c increased, it indicates that the equilibrium shifted to the right, favoring the formation of products. According to Le Chatelier's Principle, an increase in temperature favors the endothermic reaction (the reaction that absorbs heat). Therefore, the forward reaction must be endothermic, meaning its heat of reaction ( H) is positive. Last free one today — make it count tomorrow, or type /upgrade for unlimited.