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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Chapter 13, Problem 56E
At 1 atm and 25 °C, NO2 with an initial concentration of 1.00 M is
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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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- Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a productarrow_forwardWrite equilibrium constant expressions for the following reactions. For gases, use either pressures or concentrations. (a) 2 H2O2(g) 2 H2O(g) + O2(g) (b) CO(g) + O2g CO2(g) (c) C(s) + CO2(g) 2 CO(g) (d) NiO(s) + CO(g) Ni(s) + CO2(g)arrow_forwardWrite a chemical equation for an equilibrium system that would lead to the following expressions (ad) for K. (a) K=(PH2S)2 (PO2)3(PSO2)2 (PH2O)2 (b) K=(PF2)1/2 (PI2)1/2PIF (c) K=[ Cl ]2(Pcl2)[ Br ]2 (d) K=(PNO)2 (PH2O)4 [ Cu2+ ]3[ NO3 ]2 [ H+ ]8arrow_forward
- Consider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forwardWhat is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.arrow_forwardCalculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0013, [O2] = 0.0024, and [NO2] = 0.00065.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_forwardThe value of the equilibrium constant, K, is dependent on which of the following? (There may be more than one answer.) a. the initial concentrations of the reactants b. the initial concentrations of the products c. the temperature of the system d. the nature of the reactants and products Explain.arrow_forwardShow 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_forward
- At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?arrow_forwardBecause calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?arrow_forwardConsider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?arrow_forward
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