x = equilibrium ! initial = 1.00 mol/L ! 0.00 mol/L x = 1.00 mol/L equilibrium = 0.5 x Solution: x represents the change in concentration of N2O(g). Given: initial = 3.00 mol/L initial = 0.00 mol/L initial = 0.00 mol/L equilibrium = 1.00 mol/L Required: equilibrium equilibrium Analysis: Use an ICE table to determine the relationship between the equilibrium concentrations of the reactants and the product. The equilibrium position of a chemical reaction is the point at which the concentrations of reactants and products in an equilibrium system stop changing. Reaction A: Products are favoured Reaction B: Reactants are favoured. If the reaction quotient, Q, is less than the equilibrium constant, K, the system will shift toward products to achieve equilibrium. Fritz Haber was able to increase the rate of synthesis of ammonia gas, NH3(g), from gaseous hydrogen, H2(g), and nitrogen, N2(g), by adding a catalyst to the reaction. The equilibrium constant for any chemical reaction system varies with temperature. A reversible chemical reaction produces the same set of equilibrium concentrations of reactants and products in the forward direction as in the reverse direction. Chapter 7 Review, pages 480–485 Knowledgeġ.
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