EQUILIBRIUM CALCULATIONS with ICE TABLES - WORKSHEET 1. Consider the reaction: 2 SO₂ (g) + O2(g) 2 SO 3 (g) 4.0 mol of SO2 and 2.2 mol of O₂ were placed in a 10 L flask and allowed to reach equilibrium. The flask was found to contain 2.6 mol SO2. Calculate the equilibrium constant K for this reaction. 2. The equilibrium constant, K, SO3(g) NO (g) = for the reaction: NO2 (g) + SO2 (g) was found to be 0.500 at a certain temperature. If 0.300 mol of SO3 and 0.300 mol NO were placed in a 2.00 L container and allowed to react, what would be the equilibrium concentration of each gas? 3. A 1.00 L reaction container initially contains 9.28 x 103 moles of H2S. At equilibrium the concentration of H₂S is 7.06 x 103 moles. Calculate the equilibrium constant for this reaction: 2 H₂S(g) S 2H2(g) + S₂ (g) 4. The equilibrium constant for the decomposition of phosphorus pentachloride gas to form phosphorus trichloride gas and chlorine gas is 0.0211. at a certain temperature. If the initial concentration of PCI, is 1.00 M, what is the equilibrium concentration of chlorine, Cl₂? You must first write a balanced chemical equation to determine the equilibrium constant equation.

EQUILIBRIUM CALCULATIONS with ICE TABLES - WORKSHEET 1. Consider the reaction: 2 SO₂ (g) + O2(g) 2 SO 3 (g) 4.0 mol of SO2 and 2.2 mol of O₂ were placed in a 10 L flask and allowed to reach equilibrium. The flask was found to contain 2.6 mol SO2. Calculate the equilibrium constant K for this reaction. 2. The equilibrium constant, K, SO3(g) NO (g) = for the reaction: NO2 (g) + SO2 (g) was found to be 0.500 at a certain temperature. If 0.300 mol of SO3 and 0.300 mol NO were placed in a 2.00 L container and allowed to react, what would be the equilibrium concentration of each gas? 3. A 1.00 L reaction container initially contains 9.28 x 103 moles of H2S. At equilibrium the concentration of H₂S is 7.06 x 103 moles. Calculate the equilibrium constant for this reaction: 2 H₂S(g) S 2H2(g) + S₂ (g) 4. The equilibrium constant for the decomposition of phosphorus pentachloride gas to form phosphorus trichloride gas and chlorine gas is 0.0211. at a certain temperature. If the initial concentration of PCI, is 1.00 M, what is the equilibrium concentration of chlorine, Cl₂? You must first write a balanced chemical equation to determine the equilibrium constant equation.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...

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Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?
What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.
Hydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]
The value of the equilibrium constant, K, is dependent on which of the following? (There may be more than one answer.) a. the initial concentrations of the reactants b. the initial concentrations of the products c. the temperature of the system d. the nature of the reactants and products Explain.
Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a product
Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium constant, Kc, is 0.60 for PCl5(g) PCl3(g) + Cl2(g) Calculate the concentrations of all species after equilibrium has been reached.
Write a chemical equation for an equilibrium system that would lead to the following expressions (ad) for K. (a) K=(PH2S)2 (PO2)3(PSO2)2 (PH2O)2 (b) K=(PF2)1/2 (PI2)1/2PIF (c) K=[ Cl ]2(Pcl2)[ Br ]2 (d) K=(PNO)2 (PH2O)4 [ Cu2+ ]3[ NO3 ]2 [ H+ ]8
Consider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.