Introductory Chemistry: A Foundation
9th Edition
ISBN: 9781337399425
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chapter 17, Problem 8ALQ
You are browsing through the Handbook of Hypothetical Chemistry when you come across a solid that is reported to have a value of zero in water at 25 °C. What does this mean?
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Consider the reaction 3A(g)+2B(g)=2C(g)+1D(aq). In 3.1L, 2.79mol A and 2.72mol B are mixed. At
equilibrium, 0.573mol D are detected. What is the concentration equilibrium constant (K) of the
reaction?
Enter your answer to four decimal places if it is less than 1, otherwise answer with a minimum of four digits
(ie: 2543, 153.4, 12.52, or 6.523). If your last digit is a trailing zero remember that it's okay that canvas
removes it. If it is smaller than 0.0001, enter "0" and make sure you indicate your actual answer clearly on
your work.
Consider the equilibrium system described by the chemical reaction below. If
8.98 × 104 moles of KOH(aq), 8.98 × 104 moles of HCN(aq), and 0.0500 moles
of KCN(aq) are present in a 1.00 L aqueous solution at equilibrium at 298 K,
what is the value of K of the reaction at this temperature?
KCN(aq) + H,O(I) = KOH(aq) + HCN(aq)
[8.98 × 104]
K
||
[0.0500]
[1.80 x 10-²]
1
[8.06 x 10-7]
1.80 x 10-²
RESET
1.61 x 10-5
3. Hydrogen can react with elemental sulfur to give the toxic gas H₂S according to the
equation
H2(g) + 1/8 S8(s) = H2S(g)
If the equilibrium constant Kc for this reaction is 7.6 x 105 at 25°C, determine the value
for the equilibrium constant for the reaction written as 2 H₂(g) + 4 S8(s) = 2 H2S(g)
Ans: 5.8 x 1011
2022 S'2303 0
BIO-Focused CH 1244018
Chapter 17 Solutions
Introductory Chemistry: A Foundation
Ch. 17.2 - Most modern refrigerators have an internal...Ch. 17.2 - Many conditions need to be met to produce a...Ch. 17.5 - Prob. 17.1SCCh. 17.6 - Prob. 17.2SCCh. 17.7 - Prob. 17.3SCCh. 17.7 - Prob. 17.4SCCh. 17.7 - Exercise 17.5 For the exothermic reaction...Ch. 17.9 - Prob. 17.6SCCh. 17.9 - Prob. 17.7SCCh. 17.9 - The Kspvalue for lead chromate, PbCrO4, is...
Ch. 17 - Consider an equilibrium mixture of four chemicals...Ch. 17 - The boxes shown below represent a set of initial...Ch. 17 - For the reaction H2+I22HI, consider two...Ch. 17 - Given the reaction A+BC+D, consider the following...Ch. 17 - Consider the reaction A+BC+D. A friend asks the...Ch. 17 - Prob. 6ALQCh. 17 - The value of the equilibrium constant, K, is...Ch. 17 - You are browsing through the Handbook of...Ch. 17 - What do you suppose happens to the Ksp, value of a...Ch. 17 - . Consider an equilibrium mixture consisting of...Ch. 17 - . Equilibrium is microscopically dynamic but...Ch. 17 - In Section 17.3 of your text, it is mentioned that...Ch. 17 - Prob. 13ALQCh. 17 - . Consider the figure below in answering the...Ch. 17 - For a chemical reaction to take place, some or all...Ch. 17 - For the simple reaction 2H2(g)+O2(g)2H2O(l)list...Ch. 17 - How do chemists envision reactions taking place in...Ch. 17 - When molecules collide, a certain minimum energy...Ch. 17 - How does a catalyst work to speed up a chemical...Ch. 17 - Why are enzymes important? For example, what is...Ch. 17 - How does equilibrium represent the balancing of...Ch. 17 - Consider the equilibrium process depicted in Fig....Ch. 17 - When writing a chemical equation for a reaction...Ch. 17 - . How do chemists recognize a system that has...Ch. 17 - . What does it mean to say that a state of...Ch. 17 - . Consider an initial mixture of N2 and H2 gases...Ch. 17 - . In general terms. what does the equilibrium...Ch. 17 - . There is only one value of the equilibrium...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Suppose that for the reaction...Ch. 17 - . Ammonia. a very important industrial chemical....Ch. 17 - . At high temperatures, elemental nitrogen and...Ch. 17 - . Suppose that for the reaction...Ch. 17 - . What is a homogeneous equilibrium system? Give...Ch. 17 - . True or false? The position of a heterogeneous...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Indicate whether the stated equilibrium...Ch. 17 - . In your own words, describe what Le Châtelier’s...Ch. 17 - . Consider the reaction 2CO(g)+O2(g)2CO2(g)Suppose...Ch. 17 - . For an equilibrium involving gaseous substances,...Ch. 17 - . What is the effect on the equilibrium position...Ch. 17 - . For the reaction system...Ch. 17 - . For the reaction system P4(s)+6F2(g)4PF3(g)which...Ch. 17 - . Suppose the reaction system...Ch. 17 - . Consider the general reaction...Ch. 17 - . Hydrogen gas and chlorine gas in the presence of...Ch. 17 - . Hydrogen gas, oxygen gas, and water vapor are in...Ch. 17 - . The reaction C2H2(g)+2Br2(g)C2H2Br4(g)is...Ch. 17 - . Old fashioned “smelling salts” consist of...Ch. 17 - . Plants synthesize the sugar dextrose according...Ch. 17 - . Consider the exothermic reaction...Ch. 17 - . Suppose are action has the equilibrium constant...Ch. 17 - . Suppose a reaction has the equilibrium constant...Ch. 17 - . For the reaction Br2(g)+5F2(g)2BrF5(g)the system...Ch. 17 - . Consider the reaction...Ch. 17 - . For the reaction 2CO(g)+O2(g)2CO2(g)it is found...Ch. 17 - . For the reaction CO2(g)+H2(g)CO(g)+H2O(g)the...Ch. 17 - . The equilibrium constant for the reaction...Ch. 17 - . For the reaction 2H2O(g)2H2(g)+O2(g)K=2.4103at a...Ch. 17 - . For the reaction 3O2(g)2O3(g)The equilibrium...Ch. 17 - . For the reaction N2O4(g)2NO(g)the equilibrium...Ch. 17 - . Explain how the dissolving of an ionic solute in...Ch. 17 - . What is the special name given to the...Ch. 17 - . Why does the amount of excess solid solute...Ch. 17 - . Which of the following will affect the total...Ch. 17 - . Write the balanced chemical equation describing...Ch. 17 - . Write the balanced chemical equation describing...Ch. 17 - . K for copper(II)hydroxide, Cu(OH)2, has a value...Ch. 17 - Prob. 60QAPCh. 17 - . A saturated solution of nickel(II) sulfide...Ch. 17 - . Most hydroxides are not very soluble in water....Ch. 17 - . The solubility product constant, Ksp, for...Ch. 17 - . Calcium sulfate, CaSO4, is only soluble in water...Ch. 17 - . Approximately 1.5103of iron(II) hydroxide....Ch. 17 - . Chromiurn(III) hydroxide dissolves in water only...Ch. 17 - . Magnesium fluoride dissolves in water to the...Ch. 17 - . Lead(II) chloride, PbCl2(s), dissolves in water...Ch. 17 - . Mercury(I) chloride, Hg2Cl2, was formerly...Ch. 17 - . The solubility product of iron(III) hydroxide is...Ch. 17 - . Before two molecules can react, chemists...Ch. 17 - . Why does an increase in temperature favor an...Ch. 17 - . The minimum energy required for molecules to...Ch. 17 - . A(n) _______ speeds up a reaction without being...Ch. 17 - . Equilibrium may be defined as the ________ of...Ch. 17 - . When a chemical system has reached equilibrium,...Ch. 17 - . What does it mean to say that all chemical...Ch. 17 - . What does it mean to say that chemical...Ch. 17 - . At the point of chemical equilibrium, the rate...Ch. 17 - . Equilibria involving reactants or products in...Ch. 17 - . According to Le Châtelier’s principle, when a...Ch. 17 - . Addition of an inert substance (one that does...Ch. 17 - . When the volume of a vessel containing a gaseous...Ch. 17 - . Consider the following reaction at some...Ch. 17 - . What is meant by the solubility product for a...Ch. 17 - . For a given reaction at a given temperature, the...Ch. 17 - . Many sugars undergo a process called...Ch. 17 - . Suppose K=4.5103at a certain temperature for the...Ch. 17 - . For the reaction CaCO3(s)CaO(s)+CO2(g)the...Ch. 17 - Prob. 90APCh. 17 - . Teeth and bones are composed, to a first...Ch. 17 - . Under what circumstances can we compare the...Ch. 17 - . How does the collision model account for the...Ch. 17 - Prob. 94APCh. 17 - . Explain why the development of a vapor pressure...Ch. 17 - Prob. 96APCh. 17 - Prob. 97APCh. 17 - . For the reaction N2(g)+3Cl2(g)2NCl3(g)an...Ch. 17 - . Gaseous phosphorus pentachloride decomposes...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Consider the following generic reaction:...Ch. 17 - Prob. 103APCh. 17 - . The reaction PCl3(l)+Cl2(g)PCl5(s)liberates 124...Ch. 17 - Prob. 105APCh. 17 - . For the reaction N2(g)+3H2(g)2NH3(g)K=1.3102at a...Ch. 17 - . The equilibrium constant for the reaction...Ch. 17 - Prob. 108APCh. 17 - Prob. 109APCh. 17 - Prob. 110APCh. 17 - . Mercuric sulphide, HgS, is one of the least...Ch. 17 - Prob. 112APCh. 17 - . For the reaction N2(g)+3H2(g)2NH3(g), list the...Ch. 17 - . What does the activation energy for a reaction...Ch. 17 - Prob. 115APCh. 17 - Prob. 116APCh. 17 - Prob. 117APCh. 17 - Prob. 118APCh. 17 - Prob. 119APCh. 17 - Prob. 120CPCh. 17 - . Suppose that for a hypothetical reaction:...Ch. 17 - Prob. 122CPCh. 17 - . The reaction H2(g)+I2(g)2HI(g)has Kp=45.9at 763...Ch. 17 - Prob. 124CPCh. 17 - Prob. 125CPCh. 17 - . Consider the following exothermic reaction at...Ch. 17 - Prob. 1CRCh. 17 - Prob. 2CRCh. 17 - Prob. 3CRCh. 17 - How is the strength of an acid related to the...Ch. 17 - Prob. 5CRCh. 17 - How is the pH scale defined? What range of pH...Ch. 17 - 7. Describe a buffered solution. Give three...Ch. 17 - Prob. 8CRCh. 17 - Prob. 9CRCh. 17 - . Explain what it means that a reaction has...Ch. 17 - . Describe how we write the equilibrium expression...Ch. 17 - Prob. 12CRCh. 17 - Prob. 13CRCh. 17 - . In your own words, paraphrase Le Châtelier’s...Ch. 17 - Prob. 15CRCh. 17 - Prob. 16CRCh. 17 - . a. Write the conjugate acid for each of the...Ch. 17 - . Identify the Brønsted-Lowry conjugate acid-base...Ch. 17 - Prob. 19CRCh. 17 - Prob. 20CRCh. 17 - Prob. 21CRCh. 17 - Prob. 22CRCh. 17 - Prob. 23CRCh. 17 - . The solubility product of magnesium carbonate,...
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