Chemistry
12th Edition
ISBN: 9780078021510
Author: Raymond Chang Dr., Kenneth Goldsby Professor
Publisher: McGraw-Hill Education
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Textbook Question
Chapter 14, Problem 14.48QP
The equilibrium constant Kc for the reaction
is 4.2 at 1650°C. Initially 0.80 mol H2 and 0.80 mol CO2 are injected into a 5.0-L flask. Calculate the concentration of each species at equilibrium.
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Chapter 14 Solutions
Chemistry
Ch. 14.1 - Consider the equilibrium XY, where the forward...Ch. 14.2 - Write Kc and Kp for the decomposition of...Ch. 14.2 - Carbonyl chloride (COCl2), also called phosgene,...Ch. 14.2 - Prob. 4PECh. 14.2 - Write equilibrium constant expressions for Kc and...Ch. 14.2 - Consider the following equilibrium at 395 K:...Ch. 14.2 - For which of the following reactions is Kc equal...Ch. 14.2 - You are given the equilibrium constant for the...Ch. 14.2 - Prob. 7PECh. 14.2 - From the following equilibrium constant...
Ch. 14.3 - Write the equilibrium constant expression for the...Ch. 14.4 - The equilibrium constant (Kc) for the formation of...Ch. 14.4 - The equilibrium constant (Kc) for the A2+B22AB...Ch. 14.4 - Consider the reaction in Example 14.9. Starting...Ch. 14.4 - At 1280C the equilibrium constant (Kc) for the...Ch. 14.5 - At 430C, the equilibrium constant (KP) for the...Ch. 14.5 - Consider the equilibrium reaction involving...Ch. 14.5 - The diagram here shows the gaseous reaction 2AA2...Ch. 14.5 - The diagrams shown here represent the reaction...Ch. 14.5 - Consider the equilibrium between molecular oxygen...Ch. 14 - Define equilibrium. Give two examples of a dynamic...Ch. 14 - Explain the difference between physical...Ch. 14 - What is the law of mass action?Ch. 14 - Briefly describe the importance of equilibrium in...Ch. 14 - Define homogeneous equilibrium and heterogeneous...Ch. 14 - Prob. 14.6QPCh. 14 - Write the expressions for the equilibrium...Ch. 14 - Write equilibrium constant expressions for Kc, and...Ch. 14 - Write the equilibrium constant expressions for Kc...Ch. 14 - Write the equation relating Kc to KP, and define...Ch. 14 - What is the rule for writing the equilibrium...Ch. 14 - Give an example of a multiple equilibria reaction.Ch. 14 - Problems 14.13The equilibrium constant for the...Ch. 14 - The following diagrams represent the equilibrium...Ch. 14 - The equilibrium constant (Kc) for the reaction...Ch. 14 - Consider the following equilibrium process at...Ch. 14 - What is KP at 1273C for the reaction...Ch. 14 - The equilibrium constant KP for the reaction...Ch. 14 - Consider the following reaction: N2(g)+O2(g)2NO(g)...Ch. 14 - A reaction vessel contains NH3, N2, and H2 at...Ch. 14 - The equilibrium constant Kc for the reaction...Ch. 14 - At equilibrium, the pressure of the reacting...Ch. 14 - The equilibrium constant KP for the reaction...Ch. 14 - Ammonium carbamate, NH4CO2NH2, decomposes as...Ch. 14 - Consider the following reaction at 1600C....Ch. 14 - Pure phosgene gas (COCl2), 3.00 102 mol, was...Ch. 14 - Consider the equilibrium 2NOBr(g)2NO(g)+Br2(g) If...Ch. 14 - A 2.50-mole quantity of NOCl was initially in a...Ch. 14 - The following equilibrium constants have been...Ch. 14 - The following equilibrium constants have been...Ch. 14 - The following equilibrium constants were...Ch. 14 - At a certain temperature the following reactions...Ch. 14 - Based on rate constant considerations, explain why...Ch. 14 - Explain why reactions with large equilibrium...Ch. 14 - Water is a very weak electrolyte that undergoes...Ch. 14 - Consider the following reaction, which takes place...Ch. 14 - Define reaction quotient. How does it differ from...Ch. 14 - Prob. 14.38QPCh. 14 - The equilibrium constant KP for the reaction...Ch. 14 - For the synthesis of ammonia N2(g)+2H2(g)2NH3(g)...Ch. 14 - For the reaction H2(g)+CO2(g)H2O(g)+CO(g) at 700C,...Ch. 14 - At 1000 K, a sample of pure NO2 gas decomposes:...Ch. 14 - The equilibrium constant Kc for the reaction...Ch. 14 - The dissociation of molecular iodine into iodine...Ch. 14 - The equilibrium constant Kc for the decomposition...Ch. 14 - Consider the following equilibrium process at...Ch. 14 - Consider the heterogeneous equilibrium process:...Ch. 14 - The equilibrium constant Kc for the reaction...Ch. 14 - Explain Le Chteliers principle. How can this...Ch. 14 - Use Le Chteliers principle to explain why the...Ch. 14 - List four factors that can shift the position of...Ch. 14 - Does the addition of a catalyst have any effects...Ch. 14 - Consider the following equilibrium system...Ch. 14 - Heating solid sodium bicarbonate in a closed...Ch. 14 - Consider the following equilibrium systems: (a)...Ch. 14 - Consider the equilibrium 2I(g)2I2(g) What would be...Ch. 14 - Consider the following equilibrium process:...Ch. 14 - Consider the reaction...Ch. 14 - In the uncatalyzed reaction N2O4(g)2NO2(g) the...Ch. 14 - Consider the gas-phase reaction...Ch. 14 - Consider the statement: The equilibrium constant...Ch. 14 - Pure nitrosyl chloride (NOCl) gas was heated to...Ch. 14 - Determine the initial and equilibrium...Ch. 14 - Diagram (a) shows the reaction A2(g)+B2(g)2AB(g)...Ch. 14 - The equilibrium constant (KP) for the formation of...Ch. 14 - Baking soda (sodium bicarbonate) undergoes thermal...Ch. 14 - Consider the following reaction at equilibrium:...Ch. 14 - The equilibrium constant KP for the reaction...Ch. 14 - Consider the following reacting system:...Ch. 14 - At a certain temperature and a total pressure of...Ch. 14 - Consider the reaction 2NO(g)+O2(g)2NO2(g) At 430C,...Ch. 14 - When heated, ammonium carbamate decomposes as...Ch. 14 - A mixture of 0.47 mole of H2 and 3.59 moles of HCl...Ch. 14 - When heated at high temperatures, iodine vapor...Ch. 14 - One mole of N2 and three moles of H2 are placed in...Ch. 14 - Prob. 14.79QPCh. 14 - A quantity of 6.75 g of SO2Cl2 was placed in a...Ch. 14 - Prob. 14.81QPCh. 14 - Prob. 14.82QPCh. 14 - Eggshells are composed mostly of calcium carbonate...Ch. 14 - The equilibrium constant KP for the following...Ch. 14 - When dissolved in water, glucose (corn sugar) and...Ch. 14 - At room temperature, solid iodine is in...Ch. 14 - Prob. 14.89QPCh. 14 - The equilibrium constant Kc for the reaction...Ch. 14 - When heated, a gaseous compound A dissociates as...Ch. 14 - When a gas was heated under atmospheric...Ch. 14 - Prob. 14.93QPCh. 14 - At 20C, the vapor pressure of water is 0.0231 atm....Ch. 14 - Industrially, sodium metal is obtained by...Ch. 14 - In the gas phase, nitrogen dioxide is actually a...Ch. 14 - Prob. 14.99QPCh. 14 - The equilibrium constant for the reaction 4X+Y3Z...Ch. 14 - About 75 percent of hydrogen for industrial use is...Ch. 14 - Prob. 14.102QPCh. 14 - Consider the decomposition of ammonium chloride at...Ch. 14 - At 25C, the equilibrium partial pressures of NO2...Ch. 14 - Prob. 14.105QPCh. 14 - Prob. 14.107QPCh. 14 - Prob. 14.108QPCh. 14 - At 25C, a mixture of NO2 and N2O4 gases are in...Ch. 14 - A student placed a few ice cubes in a drinking...Ch. 14 - Consider the potential energy diagrams for two...Ch. 14 - The equilibrium constant Kc for the reaction...Ch. 14 - Prob. 14.113QPCh. 14 - The equilibrium constant (KP) for the reaction...Ch. 14 - The forward and reverse rate constants for the...Ch. 14 - Consider the reaction between NO2 and N2O4 in a...Ch. 14 - Prob. 14.118QPCh. 14 - (a) Use the vant Hoff equation in Problem 14.118...Ch. 14 - The KP for the reaction SO2Cl2(g)SO2(g)+Cl2(g) is...Ch. 14 - Prob. 14.121QPCh. 14 - Consider the following equilibrium system:...Ch. 14 - Prob. 14.125QPCh. 14 - Estimate the vapor pressure of water at 60C (see...
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- 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.arrow_forwardFor the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.arrow_forwardAt 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?arrow_forward
- 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+ ]8arrow_forwardAt 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?arrow_forwardSuppose 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?arrow_forward
- Write equilibrium constant expressions for the following reactions. For gases, use either pressures or concentrations. (a) 2 H2O2(g) 2 H2O(g) + O2(g) (b) CO(g) + O2g CO2(g) (c) C(s) + CO2(g) 2 CO(g) (d) NiO(s) + CO(g) Ni(s) + CO2(g)arrow_forwardA solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.arrow_forwardKc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?arrow_forward
- Consider the equilibrium N2(g)+O2(g)2NO(g) At 2300 K the equilibrium constant Kc = 1.7 103. If 0.15 mol NO(g) is placed into an empty, sealed 10.0-L flask and heated to 2300 K, calculate the equilibrium concentrations of all three substances at this temperature.arrow_forwardNitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) Suppose you place 2.00 mol NOC1 in a 1.00–L flask, seal it, and raise the temperature to 462 °C. When equilibrium has been established, 0.66 mol NO is present. Calculate the equilibrium constant Kc for the decomposition reaction from these data.arrow_forward12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.arrow_forward
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