Chemistry with Access Code, Hybrid Edition
9th Edition
ISBN: 9781285188492
Author: Steven S. Zumdahl
Publisher: CENGAGE L
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Chapter 13, Problem 35E
For which reactions in Exercise 33 is Kp equal to K
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Chapter 13 Solutions
Chemistry with Access Code, Hybrid Edition
Ch. 13 - Characterize a system at chemical equilibrium with...Ch. 13 - What is the law of mass action? Is it true that...Ch. 13 - Consider the following reactions at some...Ch. 13 - What is the difference between K and Kp? When doc...Ch. 13 - What are homogeneous equilibria? Heterogeneous...Ch. 13 - Distinguish between the terms equilibrium constant...Ch. 13 - Summarize the steps for solving equilibrium...Ch. 13 - A common type of reaction we will study is that...Ch. 13 - What is Le Chteliers principle? Consider the...Ch. 13 - The only stress (change) that also changes the...
Ch. 13 - Consider an equilibrium mixture of four chemicals...Ch. 13 - The boxes shown below represent a set of initial...Ch. 13 - For the reactionH2(g)+I2(g)2HI(g), consider two...Ch. 13 - Given the reactionA(g)+B(g)C(g)+D(g), consider the...Ch. 13 - Consider the reaction A(g)+2B(g)C(g)+D(g) in a...Ch. 13 - Consider the reactionA(g)+B(g)C(g)+D(g). A friend...Ch. 13 - Consider the following statements: Consider the...Ch. 13 - Le Chteliers principle is stated (Section 12-7) as...Ch. 13 - The value of the equilibrium constant K depends on...Ch. 13 - Consider an initial mixture of N2 and H2 gases...Ch. 13 - Consider the following reaction:...Ch. 13 - Consider the same reaction as in Question 11. In...Ch. 13 - Suppose a reaction has the equilibrium constant K...Ch. 13 - Suppose a reaction has the equilibrium constant K...Ch. 13 - Consider the following reaction at some...Ch. 13 - Consider the following generic reaction:...Ch. 13 - Explain the difference between K, Kp, and Q.Ch. 13 - Consider the following reactions:...Ch. 13 - For a typical equilibrium problem, the value of K...Ch. 13 - Which of the following statements is(are) true?...Ch. 13 - Write the equilibrium expression (K) for each of...Ch. 13 - Write the equilibrium expression (Kp) for each...Ch. 13 - At a given temperature, K = 1.3 102 for the...Ch. 13 - For the reaction H2(g)+Br2(g)2HBr(g) Kp = 3.5 104...Ch. 13 - For the reaction 2NO(g)+2H2(g)N2(g)+2H2O(g) it is...Ch. 13 - At high temperatures, elemental nitrogen and...Ch. 13 - At a particular temperature, a 3.0-L flask...Ch. 13 - At a particular temperature a 2.00-L flask at...Ch. 13 - The following equilibrium pressures at a certain...Ch. 13 - The following equilibrium pressures were observed...Ch. 13 - At 327c, the equilibrium concentrations are...Ch. 13 - At 1100 K, Kp = 0.25 for the reaction...Ch. 13 - Write expressions for K and Kp for the following...Ch. 13 - Write expressions for Kp for the following...Ch. 13 - For which reactions in Exercise 33 is Kp equal to...Ch. 13 - For which reactions in Exercise 34 is Kp equal to...Ch. 13 - Consider the following reaction at a certain...Ch. 13 - In a study of the reaction...Ch. 13 - The equilibrium constant is 0.0900 at 25C for the...Ch. 13 - The equilibrium constant is 0.0900 at 25C for the...Ch. 13 - Ethyl acetate is synthesized in a nonreacting...Ch. 13 - For the reaction 2H2O(g)2H2(g)+O2(g) K = 2.4 103...Ch. 13 - The reaction 2NO(g)+Br2(g)2NOBr(g) has Kp = 109 at...Ch. 13 - A 1.00-L flask was filled with 2.00 moles of...Ch. 13 - A sample of S8(g) is placed in an otherwise empty...Ch. 13 - At a particular temperature, 12.0 moles of SO3 is...Ch. 13 - At a particular temperature, 8.0 moles of NO2 is...Ch. 13 - An initial mixture of nitrogen gas and hydrogen...Ch. 13 - Nitrogen gas (N2) reacts with hydrogen gas (H2) to...Ch. 13 - At a particular temperature, K = 3.75 for the...Ch. 13 - At 2200C, Kp = 0.050 for the reaction...Ch. 13 - At 25c, K = 0.090 for the reaction...Ch. 13 - At 1100 K, KP = 0.25 for the reaction...Ch. 13 - At a particular temperature, Kp = 0.25 for the...Ch. 13 - At 35C, K = 1.6 105 for the reaction...Ch. 13 - At a particular temperature, K = 4.0 107 for the...Ch. 13 - At a particular temperature, K = 2.0 106 for the...Ch. 13 - Lexan is a plastic used to make compact discs,...Ch. 13 - Prob. 61ECh. 13 - Prob. 62ECh. 13 - Suppose the reaction system...Ch. 13 - Predict the shift in the equilibrium position that...Ch. 13 - An important reaction in the commercial production...Ch. 13 - What will happen to the number of moles of SO3 in...Ch. 13 - In which direction will the position of the...Ch. 13 - Hydrogen for use in ammonia production is produced...Ch. 13 - Old-fashioned smelling salts consist of ammonium...Ch. 13 - Ammonia is produced by the Haber process, in which...Ch. 13 - Prob. 71AECh. 13 - Given the following equilibrium constants at...Ch. 13 - Consider the decomposition of the compound C5H6O3...Ch. 13 - At 25C. Kp 1 1031 for the reaction a. Calculate...Ch. 13 - The gas arsine, AsH3, decomposes as follows:...Ch. 13 - At a certain temperature, K = 9.1 10-4 for the...Ch. 13 - At a certain temperature, K = 1.1 l03 for the...Ch. 13 - For the reaction PCl5(g)PCl3(g)+Cl2(g) at 600. K,...Ch. 13 - At 25C, gaseous SO2Cl2 decomposes to SO2(g) and...Ch. 13 - For the following reaction at a certain...Ch. 13 - Novelty devices for predicting rain contain...Ch. 13 - Consider the reaction Fe3+(aq)+SCN(aq)FeSCN2+(aq)...Ch. 13 - Chromium(VI) forms two different oxyanions, the...Ch. 13 - Prob. 84AECh. 13 - Suppose K = 4.5 103 at a certain temperature for...Ch. 13 - For the reaction below, Kp = 1.16 at 800C....Ch. 13 - Many sugars undergo a process called mutarotation,...Ch. 13 - Peptide decomposition is one of the key processes...Ch. 13 - Prob. 89AECh. 13 - Methanol, a common laboratory solvent, poses a...Ch. 13 - An equilibrium mixture contains 0.60 g solid...Ch. 13 - At a particular temperature, 8.1 moles of NO2 gas...Ch. 13 - A sample of solid ammonium chloride was placed in...Ch. 13 - In a given experiment, 5.2 moles of pure NOCl was...Ch. 13 - For the reactionN2O4(g)2NO2(g),Kp=0.25 at a...Ch. 13 - Consider the following exothermic reaction at...Ch. 13 - For the following endothermic reaction at...Ch. 13 - A 1.604-g sample of methane (CH4) gas and 6.400 g...Ch. 13 - A 4.72-g sample of methanol (CH3OH) was placed in...Ch. 13 - At 35C, K = 1.6 105 for the reaction...Ch. 13 - Nitric oxide and bromine at initial partial...Ch. 13 - At 25C. Kp = 5.3 105 for the reaction...Ch. 13 - Consider the reaction P4(g)2P2(g) where Kp = 1.00 ...Ch. 13 - The partial pressures of an equilibrium mixture of...Ch. 13 - At 125C, KP = 0.25 for the reaction...Ch. 13 - A mixture of N2, H2, and NH3 is at equilibrium...Ch. 13 - Consider the decomposition equilibrium for...Ch. 13 - An 8.00-g sample of SO3 was placed in an evacuated...Ch. 13 - A sample of iron(II) sulfate was heated in an...Ch. 13 - Prob. 111CPCh. 13 - A sample of N2O4(g) is placed in an empty cylinder...Ch. 13 - A sample of gaseous nitrosyl bromide (NOBr) was...Ch. 13 - The equilibrium constant Kp for the reaction...Ch. 13 - For the reaction NH3(g)+H2S(g)NH4HS(s) K = 400. at...Ch. 13 - Given K = 3.50 at 45C for the reaction...Ch. 13 - In a solution with carbon tetrachloride as the...Ch. 13 - The hydrocarbon naphthalene was frequently used in...Ch. 13 - A gaseous material XY(g) dissociates to some...
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- The following reaction occurs in pure water: H2O(l)+H2O(l)H3O+(aq)+OH-(aq) which is often abbreviated as H2O(l)H+(aq)+OH-(aq) For this reaction, G = 79.9 kJ/mol at 25C. Calculate the value of G for this reaction at 25C when [OH] = 0.15 M and [H+] = 0.71 M.arrow_forward5.11. Determine the numerical value of Q for the reaction conditions indicated.arrow_forwardDescribe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.arrow_forward
- Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25Carrow_forwardCalculate K at 25°C for each of the reactions referred to in Question 32. Assume smallest whole-number coefficients.arrow_forwardFor the given chemical equilibrium, these data are determined experimentally: T K 350K 3.76102 450K 1.86101 Determine H for this reaction.arrow_forward
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- Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.arrow_forwardConsider the equilibrium system HF(aq)H+(aq)+F(aq) Given HfHF(aq)=320.1kJ/mol , HfF(aq)=332.6kJ/mol ; SF(aq)=13.8kJ/molK ; KaHF=6.9104 at 25°C calculate S° for HF(aq).arrow_forwardDetermine the equilibrium constant for the reaction Sn+Pb2+Sn2++Pbarrow_forward
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