3 K= 2 Substitute the given values for the equilibrium concentrations of the products and the equilibrium constant and solve for.
Given: 2 ClF3(g) # !" ! Cl2(g) + 3 F2(g) equilibrium = 1.62 × 10 mol/L equilibrium = 1.85 × 10−1 mol/L K = 3.72 × 10−2 Required: equilibrium Solution: Write the equilibrium law equation using the balanced chemical equation. Then, substitute the equilibrium concentrations into the equilibrium law equation and solve for K. Given: Cl2(g) + CO(g) # !" ! COCl2(g) equilibrium = 1.11 × 10 mol/L equilibrium = 1.03 × 10−1 mol/L = 1.17 × 10−1 mol/L Required: K Solution: Write the equilibrium law equation using the balanced chemical equation.
In a homogeneous equilibrium, all reactants and products are in the same state, but in a heterogeneous equilibrium, reactants and products are present in at least two different states. = (1.00 mol/L) – (0.016 mol/L) equilibrium = 9.8×10 −1 mol/L Statement: The equilibrium concentration of diatomic bromine gas is 9.8 × 10–1 mol/L. Solution: x represents the change in concentration of Br2(g). Given: initial = 1.00 mol/L initial = 0.00 mol/L equilibrium = 0.032mol/L Required: equilibrium Analysis: Use an ICE table to determine the relationship between the equilibrium concentrations of the reactant and the product. = 0.5(1.00 mol/L) equilibrium = 5.00 ×10 −1 mol/L equilibrium = (3.00 mol/L) – 2 x = (3.00 mol/L) – 2(1.00 mol/L) equilibrium = 1.00 mol/L equilibrium = 3.00 mol/L – 2x Statement: The equilibrium concentration of dinitrogen monoxide gas is 1.00 mol/L the equilibrium concentration of oxygen gas is 5.00 × 10–1 mol/L and the equilibrium concentration of nitric oxide gas is 1.00 mol/L. 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.