Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Textbook Question
Chapter 12, Problem 2QAP
The following data are for the system
(a) How long does it take the system to reach equilibrium?
(b) How does the rate of the forward reaction compare with the rate of the reverse reaction after 45 s? After 90 s?
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Chemistry: Principles and Reactions
Ch. 12 - The following data are for the system A(g)2B(g)...Ch. 12 - The following data are for the system A(g)2B(g)...Ch. 12 - Prob. 3QAPCh. 12 - Complete the table below for the reaction...Ch. 12 - Write the equilibrium expressions (K) for the...Ch. 12 - Write the equilibrium expressions (K) for the...Ch. 12 - Write the equilibrium expressions (K) for the...Ch. 12 - Write the equilibrium expressions (K) for the...Ch. 12 - Given the following descriptions of reversible...Ch. 12 - Given the following descriptions of reversible...
Ch. 12 - Write an equation for an equilibrium system that...Ch. 12 - Write a chemical equation for an equilibrium...Ch. 12 - Consider the following reaction at 250C:...Ch. 12 - Consider the following reaction at 1000 C:...Ch. 12 - At 627C, K=0.76 for the reaction...Ch. 12 - At 800C, K=2.2104 for the following reaction...Ch. 12 - Prob. 17QAPCh. 12 - Given the following data at 25C...Ch. 12 - Given the following data at a certain temperature,...Ch. 12 - Consider the following hypothetical reactions and...Ch. 12 - When one mole of carbon disulfide gas reacts with...Ch. 12 - Calculate K for the formation of methyl alcohol at...Ch. 12 - Ammonium carbamate solid (NH4CO2NH2) decomposes at...Ch. 12 - Consider the decomposition at 25C of one mole of...Ch. 12 - Consider the decomposition of ammonium hydrogen...Ch. 12 - A sealed flask has 0.541 atm of SO3 at 1000 K. The...Ch. 12 - A gaseous reaction mixture contains 0.30 atm SO2,...Ch. 12 - For the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at...Ch. 12 - The reversible reaction between hydrogen chloride...Ch. 12 - The reversible reaction between hydrogen chloride...Ch. 12 - A compound, X, decomposes at 131C according to the...Ch. 12 - Consider the following reaction at 75C:...Ch. 12 - Consider the reaction between nitrogen and steam:...Ch. 12 - At 500C, k for the for the formation of ammonia...Ch. 12 - At a certain temperature, K is 4.9 for the...Ch. 12 - At a certain temperature, K=0.29 for the...Ch. 12 - For the reaction N2(g)+2H2O(g)2NO(g)+2H2(g) K is...Ch. 12 - Nitrogen dioxide can decompose to nitrogen oxide...Ch. 12 - Consider the following reaction:...Ch. 12 - Consider the hypothetical reaction at 325C...Ch. 12 - At a certain temperature, the equilibrium constant...Ch. 12 - At 460C, the reaction SO2(g)+NO2(g)NO(g)+SO3(g)...Ch. 12 - Solid ammonium iodide decomposes to ammonia and...Ch. 12 - Consider the following decomposition at 80C....Ch. 12 - Hydrogen cyanide, a highly toxic gas, can...Ch. 12 - At 800 K, hydrogen iodide can decompose into...Ch. 12 - For the following reactions, predict whether the...Ch. 12 - Follow the directions of Question 47 for the...Ch. 12 - Consider the system SO3(g)SO2(g)+12 O2(g)H=98.9kJ...Ch. 12 - Consider the system...Ch. 12 - Predict the direction in which each of the...Ch. 12 - Predict the direction in which each of the...Ch. 12 - At a certain temperature, nitrogen and oxygen...Ch. 12 - Consider the following hypothetical reaction:...Ch. 12 - Iodine chloride decomposes at high temperatures to...Ch. 12 - Sulfur oxychloride, SO2Cl2, decomposes to sulfur...Ch. 12 - For the following reaction C(s)+2H2(g)CH4(g)...Ch. 12 - For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627....Ch. 12 - For a certain reaction, H is +33 kJ. What is the...Ch. 12 - Prob. 60QAPCh. 12 - Hemoglobin (Hb) binds to both oxygen and carbon...Ch. 12 - Mustard gas, used in chemical warfare in World War...Ch. 12 - Prob. 63QAPCh. 12 - For the decomposition of CaCO3 at 900C, K=1.04....Ch. 12 - Isopropyl alcohol is the main ingredient in...Ch. 12 - Consider the equilibrium H2(g)+S(s)H2S(g)When this...Ch. 12 - Prob. 67QAPCh. 12 - The following data apply to the unbalanced...Ch. 12 - Consider the reaction: A(g)+2B(g)+C(s)2D(g)At 25C,...Ch. 12 - For the reaction C(s)+CO2(g)2CO(g) K=168 at 1273...Ch. 12 - Consider the system A(g)+2B(g)+C(g)2D(g)at 25C. At...Ch. 12 - The graph below is similar to that of Figure 12.2....Ch. 12 - Prob. 73QAPCh. 12 - The figures below represent the following reaction...Ch. 12 - Prob. 75QAPCh. 12 - Prob. 76QAPCh. 12 - Consider the following reaction at a certain...Ch. 12 - Prob. 78QAPCh. 12 - Ammonia can decompose into its constituent...Ch. 12 - Hydrogen iodide gas decomposes to hydrogen gas and...Ch. 12 - For the system SO3(g)SO2(g)+12 O2(g)at 1000 K,...Ch. 12 - A student studies the equilibrium I2(g)2I(g)at a...Ch. 12 - At a certain temperature, the reaction...Ch. 12 - Benzaldehyde, a flavoring agent, is obtained by...Ch. 12 - Prob. 85QAPCh. 12 - Prob. 86QAP
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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_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_forwardCyclohexane, C6H12, a hydrocarbon, can isomerize or change into methylcyclopentane, a compound of the same formula (C5H9CH3) but with a different molecular structure. sssss The equilibrium constant has been estimated to be 0.12 at 25 C. If you had originally placed 0.045 mol of cyclohexane in a 2.8-L flask, what would be the concentrations of cyclohexane and methylcyclopentane when equilibrium is established?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_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_forwardConsider 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_forward
- The equilibrium constant Kc for the synthesis of methanol, CH3OH. CO(g)+2H2(g)CH3OH(g) is 4.3 at 250C and 1.8 at 275C. Is this reaction endothermic or exothermic?arrow_forwardFor the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.arrow_forwardWrite equilibrium-constant expressions Kp for each of the following reactions: a H2(g)+Br2(g)2HBr(g) b CS2(g)+4H2(g)CH4(g)+2H2S(g) c 4HCl(g)+O2(g)2H2O(g)+2Cl2(g) d CO(g)+2H2(g)CH3OH(g)arrow_forward
- The decomposition of PCl5(g) to form PCl3(g) and Cl2(g) has Kc = 33.3 at a high temperature. If the initial concentration of PCl5 is 0.1000 M, what are the equilibrium concentrations of the reactants and products?arrow_forwardIs a system at equilibrium if the rate constants of the forward and reverse reactions are equal?arrow_forward
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