Chemistry
12th Edition
ISBN: 9780078021510
Author: Raymond Chang Dr., Kenneth Goldsby Professor
Publisher: McGraw-Hill Education
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Chapter 14.2, Problem 1PE
Write Kc and Kp for the decomposition of dinitrogen pentoxide:
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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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- Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.arrow_forwardWrite 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 productarrow_forwardAt a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?arrow_forward
- Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.arrow_forwardDistinguish between the terms equilibrium constant and reaction quotient. When Q = K, what does this say about a reaction? When Q K, what does this say about a reaction? When Q K. what does this say about a reaction?arrow_forwardWrite the expression for the equilibrium constant and calculate the partial pressure of CO2(g), given that Kp is 0.25 (at 427 C) for NaHCO3(s) NaOH(s) + CO2(g)arrow_forward
- 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?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_forwardWrite 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_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_forwardConsider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. • The density of the solution is 1.00 g/mL. • Volumes are additive. • The specific heat of the solution is 4.18 J/g C.arrow_forwardConsider the following equilibria involving SO2(g) and their corresponding equilibrium constants. SO2(g) + 12 O2(g) SO3(g) K1 2SO3(g) 2SO2(g) + O2(g) K2 Which of the following expressions relates K1 to K2? (a) K2=K12 (b) K22=K1 (c) K2 = K1 (d) K2 = 1/K1 (e) K2=1/K12arrow_forward
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