Ch 6 Practice Problems

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1 Ch 6 Practice Problems 1. Which of the following statements is true? A) When two opposing processes are proceeding at identical rates, the sstem is at equilibrium. B) Catalsts are an effective means of changing the position of an equilibrium. The concentration of the products equals that of the reactants and is constant at equilibrium. D) An endothermic reaction shifts toward reactants when heat is added to the reaction. E) None of the above statements is true.. Which of the following statements concerning equilibrium is not true? A) A sstem that is disturbed from an equilibrium condition responds in such a wa as to restore equilibrium. B) Equilibrium in molecular sstems is dnamic, with two opposing processes balancing one another. The value of the equilibrium constant for a given reaction mixture is the same regardless of the direction from which equilibrium is attained. D) A sstem moves spontaneousl toward a state of equilibrium. E) The equilibrium constant is independent of temperature.. If, at a given temperature, the equilibrium constant for the reaction H (g) + Cl (g) HCl(g) is 6.0, then the equilibrium constant for the reaction HCl(g) (1/)H (g) + (1/)Cl (g) can be represented as A) 6.0. B) D) E) Choose the mass action or equilibrium expression for the reaction SO (g) + O (g) SO (g) A) B) [O ] [O ] [O ] D) [SO ] [SO ] [O ] 5. The value of K p for the reaction H (g) + O (g) H O (g) is at 640K. Determine the value for K c for this reaction at 640K. A) B) D) E)

2 6. For the reaction NCl (g) N (g) + Cl (g), the equilibrium pressures are P(NCl ) = atm P(N ) =.1 atm P(Cl ) = atm Determine K p for this reaction. A) B) D) 7.75 E) The reaction H (g) + I (g) HI(g) has K p = 45.9 at 76 K. A particular equilibrium mixture at that temperature contains gaseous HI at a partial pressure of.50 atm and hdrogen gas at a partial pressure of 0.0 atm. What is the partial pressure of I? A) 0.0 atm B) 0. atm 1.16 atm D) 0.66 atm E) 8.7 atm 8. Consider the equation NOCl (g) NO(g) + Cl (g). The equilibrium constant is at 115 C. Calculate Kp. A) B) D) 0.18 E) For the reaction below, K p = 1.16 at 800. C. CaCO (s) CaO(s) + CO (g) If a 5.0-g sample of CaCO is put into a 10.-L container and heated to 800. C, what percent of the CaCO will react to reach equilibrium? A).7% B) 5.8% 1.4% D) 100.% E) 47.4% 10. Consider the reaction CaCl (s) + H O(g) CaCl H O(s) What is the equilibrium constant for the reaction as written? HO] A) K = ] [H O] 1 B) K = [H O] 1 K = ] [HO] D) K = [H O] E) HO] K = [H O]

3 11. Consider the reaction NOBr(g) NO(g) + Br (g) A 1.0-L vessel was initiall filled with pure NOBr at a pressure of.8 atm and 00 K. At equilibrium, the partial pressure of NOBr was.0 atm. Determine the value of K p for the reaction. A) 0.81 B) D) 1.6 E) Consider the equation A(g) B(g) + C(g). At a particular temperature, K = If ou mixed 5.0 mol B, 0.10 mol C, and mol A in a 1-L container, in which direction would the reaction initiall proceed? A) To the left. B) To the right. The above mixture is the equilibrium mixture. D) We cannot tell from the information given. 1. Consider the decomposition of hdrazine as shown below. N H 4(g) H (g) + N (g) At a certain temperature, K p = When pure hdrazine is placed in an otherwise empt vessel at this temperature, equilibrium is reached after 0.0% of the hdrazine has decomposed. Calculate the partial pressure of hdrogen gas at equilibrium. A) 54 atm B) 76 atm 17 atm D) 5776 atm 14. A sample of solid NH 4NO was placed in an evacuated container and then heated so that it decomposed explosivel according to the following reaction: NH 4NO (s) N O(g) + H O(g) At equilibrium, the total pressure in the container was found to be.0 atm at a temperature of 500 C. Calculate K p. A).5 B) D) 1.4 E) At 75 C, K for the reaction N O 4(g) NO (g) is We introduce 0.06 mol of N O 4 into a.1-l vessel at 75 C and let equilibrium be established. The total pressure in the sstem at equilibrium will be A) 0. atm. B) 0.8 atm atm. D) 0.56 atm. E) atm.

4 16. Consider the reaction SO (g) + O (g) SO (g) at constant temperature. Initiall a container is filled with pure SO (g) at a pressure of atm, after which equilibrium is allowed to be reached. If is the partial pressure of O at equilibrium, what is the value of K p? A) B) D) / 17. The following reaction is investigated (assume an ideal gas mixture). N O(g) + N H 4(g) N (g) + H O(g) Initiall there are 0.10 mol of N O and 0.0 mol of N H 4, in a 0.0-L container. If there is mol of N O at equilibrium, how man moles of N are present at equilibrium? A) 0.15 B) D) 0.15 E) Consider the equation A(g) B(g) + C(g). At a particular temperature, K = If ou start with.0 M of chemical A, calculate the equilibrium concentration of chemical C. A) M B).6 10 M 1.0 M D).1 10 M 19. At a certain temperature, K for the reaction is 7.5. NO N O 4 If.0 mol of NO is placed in a.0-liter container and permitted to react at this temperature, calculate the concentration of N O 4 at equilibrium. A) 0.9 mol/l B) 0.65 mol/l 0.8 mol/l D) 7.5 mol/l 0. Nitrogen gas (N ) reacts with hdrogen gas (H ) to form ammonia (NH ). At 00 C in a closed container, 1.1 atm of nitrogen gas is mixed with.1 atm of hdrogen gas. At equilibrium, the total pressure is. atm. Calculate the partial pressure of hdrogen gas at equilibrium. A).1 atm B) 0.60 atm 0.70 atm D) 0.0 atm E) 1.8 atm

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