CHEMISTRY,AP EDITION-W/ACCESS (HS)
9th Edition
ISBN: 9781285732930
Author: ZUMDAHL
Publisher: CENGAGE L
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Chapter 13, Problem 80AE
For the following reaction at a certain temperature
it is found that the equilibrium concentrations in a 5.00-L rigid container are [H2 = 0.0500 M, [F2] = 0.0100 M, and [HF] = 0.400 M. If 0.200 mole of F2 is added to this equilibrium mixture, calculate the concentrations of all gases once equilibrium is reestablished.
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Modify the given carbon skeleton to draw the major product of the following reaction. If a racemic mixture of enantiomers is
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Sort the following into the classification for a reaction that is NOT at equilibrium versus a reaction system that has reached equilibrium.
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The forward and reverse reactions
proceed at the same rate.
Chemical equilibrium is a dynamic
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The ratio of products to reactants is
not stable.
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The state of chemical equilibrium will
remain the same unless reactants or
products escape or are introduced into
the system. This will disturb the
equilibrium.
The concentration of products is
increasing, and the concentration of
reactants is decreasing.
The ratio of products to reactants
does not change.
The rate at which products form from
reactants is equal to the rate at which
reactants form from products.
The concentrations of reactants and
products are stable and cease to
change.
The reaction has reached equilibrium.
The rate of the forward reaction is
greater than the rate of the reverse
reaction.
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Place the following characteristics into the box for the correct ion. Note that some of the characteristics will not be placed in either bin. Use your periodic table
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This anion could form a neutral
compound by forming an ionic bond
with one Ca²+.
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This ion forms ionic bonds with
nonmetals.
This ion has a 1- charge.
This is a polyatomic ion.
The neutral atom from which this ion
is formed is a metal.
The atom from which this ion is
formed gains an electron to become
an ion.
The atom from which this ion is
formed loses an electron to become
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This ion has a total of 18 electrons.
This ion has a total of 36 electrons.
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Potassium ion
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Chapter 13 Solutions
CHEMISTRY,AP EDITION-W/ACCESS (HS)
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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