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- 7-40 Is there any change in conditions that change the equilibrium constant, K, of a given reaction?7-22 If you add a piece of marble, CaCO3 to a 6 M HCI solution at room temperature, you will see some bubbles form around the marble as gas slowly rises. If you crush another piece of marble and add it to the same solution at the same temperature, you will see vigorous gas formation, so much so that the solution appears to be boiling. Explain.7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its equilibrium concentration. Calculate the equilibrium constant, K, for this reaction.
- 7-36 Complete the following table showing the effects of changing reaction conditions on the equilibrium and value of the equilibrium constant, K. Change in Condition How the Reacting System Changes to Achieve a New Equilibrium Does the Value of K Increase or Decrease? Addition of a reactant Shift to product formation Neither Removal of a reactant Addition of a product Removal of a product Increasing pressure7-16 A quart of milk quickly spoils if left at room temperature but keeps for several days in a refrigerator. Explain.7-17 If a certain reaction takes 16 h to go to completion at 10°C, what temperature should we run it if we want it to go to completion in 1 h?
- 7-41 The equilibrium constant at 1127°C for the following endothermic reaction is 571: If the mixture is at equilibrium, what happens to K if we: (a) Add some H2S? (b) Add some H2? (c) Lower the temperature to 1000°C?7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich are in equilibrium in aqueous solution. The equilibrium constant for the reaction is 1.5 at 30°C. (a) If you begin with a fresh 1.0 M solution of D-glucose in water, what will be its concentration when equilibrium is reached? (b) Calculate the percentage of glucose and of glucose present at equilibrium in aqueous solution at 30°C.. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
- Predict the equilibrium concentration of H₂O in the reaction described below (for which Kc = 1.79 at the reaction temperature) by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. 2 H₂S(g) + SO₂(g) = 3 S(s) + 2 H₂O(g) Initial (M) Change (M) Equilibrium (M) -3.x 0.025 + 2x The reaction mixture initially contains 0.050 M H₂S and 0.050 M SO₂. Fill in the ICE table with the appropriate value for each involved species to determine the concentrations of all reactants and products. 0 1 2 H₂S(g) + 0.050 + x 0.025 + 3x 0.050 0.050 + 2x 0.025 - Xx +X 2 SO₂(g) 0.050 + 3x 0.025 - 2x +2x 0.050 - x 0.025-3x 3 3 S(s) +3x 0.050 - 2x --X + 0.050-3x NEXT > 2 H₂O(g) RESET -2x 0.025 + xPredict the equilibrium concentration of H₂O in the reaction described below (for which Kc = 1.79 at the reaction temperature) by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. 2 H₂S(g) + SO₂(g) 3 S(s) + 2 H₂O(g) Initial (M) Change (M) Equilibrium (M) -3.x 0.025 + 2x The reaction mixture initially contains 0.050 M H₂S and 0.050 M SO₂. Fill in the ICE table with the appropriate value for each involved species to determine the concentrations of all reactants and products. 0 1 2 H₂S(g) + 0.050 + x 0.025 + 3x 0.050 0.050 + 2x 0.025 - x +X 2 SO₂(g) 0.050 + 3x 0.025 - 2x +2x 0.050- x 0.025 -3x 3 3 S(s) +3.x 0.050 - 2x -X + 0.050-3x NEXT > 2 H₂O(g) RESET -2x 0.025 + xCalculate a value for the equilibrium constant for the reaction O2 (g) + O(g) = 03 (9) given hv NO2 (g) = NO(g) + O(g) K = 5.1 × 10-49 -34 O3 (g) + NO(g)= NO,(g) + O2(g) K = 2.2 × 10- (Hint: When reactions are added together, the equilibrium expressions are multiplied.) K =