Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
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Textbook Question
Chapter 13, Problem 23E
For which of the reactions in Exercise 13.15 does Kc (calculated using concentrations) equal KP (calculated using pressures)?
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Chapter 13 Solutions
Chemistry by OpenStax (2015-05-04)
Ch. 13 - What does it mean to describe a reaction as...Ch. 13 - When writing an equation, how is a reversible...Ch. 13 - If a reaction is reversible, when can it be said...Ch. 13 - Is a system at equilibrium if the rate constants...Ch. 13 - If the concentrations of products and reactants...Ch. 13 - Explain why there may be an infinite number of...Ch. 13 - Explain why an equilibrium between Br2(l) and...Ch. 13 - If you observe the following reaction at...Ch. 13 - Among the solubility rules previously discussed is...Ch. 13 - Among the solubility rules previously discussed is...
Ch. 13 - Benzene is one of the compounds used as octane...Ch. 13 - Show that the complete chemical equation, the...Ch. 13 - For a titration to be effective, the reaction must...Ch. 13 - For a precipitation reaction to be useful in a...Ch. 13 - Write the mathematical expression for the reaction...Ch. 13 - Write the mathematical expression for the reaction...Ch. 13 - The initial concentrations or pressures of...Ch. 13 - The initial concentrations or pressures of...Ch. 13 - The following reaction has KP=4.50105 at 720 K....Ch. 13 - Determine if the following system is at...Ch. 13 - Which of the systems described in Exercise 13.15...Ch. 13 - Which of the systems described in Exercise 13.16...Ch. 13 - For which of the reactions in Exercise 13.15 does...Ch. 13 - For which of the reactions in Exercise 13.16 does...Ch. 13 - Convert the values of KC to values of KP to the...Ch. 13 - Covert the values of Kc to the values of KP or the...Ch. 13 - What is the value of the equilibrium constant...Ch. 13 - Write the expression of the reaction quotient for...Ch. 13 - Write the reaction quotient expression for the...Ch. 13 - What is the approximate value of the equilibrium...Ch. 13 - The following equation represents a reversible...Ch. 13 - Explain how to recognize the conditions under...Ch. 13 - What property of a reaction can we use to predict...Ch. 13 - What would happen to the color of the solution in...Ch. 13 - The following reaction occurs when a burner on a...Ch. 13 - A necessary step in the manufacture of sulfuric...Ch. 13 - Suggest four ways in which the concentration of...Ch. 13 - Suggest four ways in which the concentration of...Ch. 13 - How will an increase in temperature affect each of...Ch. 13 - How will an increase in temperature affect each of...Ch. 13 - Water gas is a 1:1 mixture of carbon monoxide and...Ch. 13 - Nitrogen and oxygen react at high temperatures....Ch. 13 - Water gas, a mixture of H2 and CO, is an important...Ch. 13 - Pure iron metal can be produced by the reduction...Ch. 13 - Ammonia is a weak base that reacts with water...Ch. 13 - Acetic acid is a weak acid that reacts with water...Ch. 13 - Suggest two ways in which the equilibrium...Ch. 13 - How can the pressure of water vapor be increased...Ch. 13 - Additional solid silver sulfate, a slightly...Ch. 13 - The amino acid alanine has two isomers, -alanine...Ch. 13 - A reaction is represented by this equation:...Ch. 13 - A reaction is represented by this equation:...Ch. 13 - What is the value of the equilibrium constant at...Ch. 13 - Hydrogen is prepared commercially by the reaction...Ch. 13 - A 0.72-m01 sample of PCl5 is put into a 1.00-L...Ch. 13 - At 1 atm and 25 C, NO2 with an initial...Ch. 13 - Calculate the value of the equilibrium constant Kp...Ch. 13 - When heated, iodine vapor dissociates according to...Ch. 13 - A sample of ammonium chloride was heated in a...Ch. 13 - At a temperature of 60 C, the vapor pressure of...Ch. 13 - Complete the changes in concentrations (or...Ch. 13 - Complete the changes in concentrations (or...Ch. 13 - Why are there no changes specified for Ni in...Ch. 13 - Why are there no changes specified for NH4HS in...Ch. 13 - Analysis of the gases in a sealed reaction vessel...Ch. 13 - Calculate the number of moles of HI that are at...Ch. 13 - What is the pressure of BrCl in an equilibrium...Ch. 13 - What is the pressure of CO2 in a mixture at...Ch. 13 - Cobalt metal can be prepared by reducing cobalt...Ch. 13 - Carbon reacts with water vapor at elevated...Ch. 13 - Sodium sulfate 10-hydrate, Na2SO410H2O, dehydrates...Ch. 13 - Calcium Chloride 6-hydrate, CaCl26H2O, dehydrates...Ch. 13 - A student solved the following problem and found...Ch. 13 - A student solved the following problem and found...Ch. 13 - Assume that the change in concentration of N2O4 is...Ch. 13 - Assume that the change in concentration of COCI2...Ch. 13 - Assume that the change in pressure of H2S is small...Ch. 13 - What are all concentrations after a mixture that...Ch. 13 - What are the concentrations of PCl5, PCl3, and Cl2...Ch. 13 - Calculate the pressures of all species at...Ch. 13 - Calculate the equilibrium concentrations of NO,...Ch. 13 - Calculate the equilibrium concentrations that...Ch. 13 - One of the important reactions in the formation of...Ch. 13 - Calculate the pressures of NO, Cl2, and NOCI in an...Ch. 13 - Calculate the number of grams of HI that are at...Ch. 13 - Butane exists as two isomers, n -butane and...Ch. 13 - What is the minimum mass of CaCO3 required to...Ch. 13 - The equilibrium constant (Kc) for this reaction is...Ch. 13 - At 25 C and at 1 atm, the partial pressures in an...Ch. 13 - In a 3.0-L vessel, the following equilibrium...Ch. 13 - The equilibrium constant (Kc) for this reaction is...Ch. 13 - Antimony pentachloride decomposes according to...Ch. 13 - Consider the reaction between H2 and O2 at 1000...Ch. 13 - An equilibrium is established according to the...Ch. 13 - Consider the equilibrium...Ch. 13 - The binding of oxygen by hemoglobin (Hb), giving...Ch. 13 - The hydrolysis of the sugar sucrose to the sugars...Ch. 13 - The density of trifluoroacetic acid vapor was...Ch. 13 - Liquid N2o3 is dark blue at low temperatures, but...Ch. 13 - A 1.00-L vessel at 400 C contains the following...Ch. 13 - A 0.010 M solution of the weak acid HA has an...
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- Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.arrow_forward1. A process is spontaneous in the direction that moves it away from equilibrium toward equilibriumarrow_forwardHydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are placed in a closed 10.0-L vessel, what is the mole fraction of HI in the mixture when equilibrium is reached at 205C? Use data from Appendix C and any reasonable approximations to obtain K.arrow_forward
- Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.arrow_forwardSodium acetate crystallizes from a supersaturated solution (see Figure 12.4). What can you say about the sign of G? WTiat would you expect for the sign of S? What about the sign of H? Is the crystallization exothermic or endothermic? Explain your answersarrow_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_forward
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- 5.49. Consider the following equilibrium: What is the effect on the equilibrium of each of the following changes? (You may need to calculate some standard enthalpy or Gibbs energy changes to answer these.) (a) The pressure is increased by decreasing the volume. (b) The temperature is decreased. (c) The pressure is increased by the addition of nitrogen gas, .arrow_forwardFor each reaction, an equilibrium constant at 298 K is given. Calculate G for each reaction. (a) Br2()+ H2(g)2HBr(g) KP = 4.4 1018 (b) H2O()H2O(g) KP = 3.17 102 (c) N2(g) +3H2(g)2NH3(g) Kc = 3.5 108arrow_forwardThe following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.arrow_forward
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