Chemistry for Engineering Students
3rd Edition
ISBN: 9781285199023
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 12, Problem 12.51PAE
Interpretation Introduction
To determine:
Effect of increase in pressure on the reaction equilibrium
Given:
Interpretation Introduction
To determine:
Effect of increase in pressure on the reaction equilibrium
Given:
Interpretation Introduction
To determine:
Effect of increase in pressure on the reaction equilibrium
Given:
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Chemistry for Engineering Students
Ch. 12 - list chemical reactions important in the...Ch. 12 - Explain that equilibrium is dynamic, and that at...Ch. 12 - Prob. 3COCh. 12 - calculate equilibrium constants from experimental...Ch. 12 - Prob. 5COCh. 12 - calculate molar solubility from Kspor vice versa.Ch. 12 - Prob. 7COCh. 12 - Prob. 8COCh. 12 - calculate the new equilibrium composition of a...Ch. 12 - Explain the importance of both kinetic and...
Ch. 12 - Identify the first chemical step in the production...Ch. 12 - Explain why the hydration process for concrete is...Ch. 12 - Prob. 12.3PAECh. 12 - 12.4 In what geographical region of the country...Ch. 12 - Prob. 12.5PAECh. 12 - Prob. 12.6PAECh. 12 - Prob. 12.7PAECh. 12 - On your desk is a glass half-filled with water and...Ch. 12 - In the figure, orange fish are placed in one...Ch. 12 - At a particular temperature, iodine vapor, I2, is...Ch. 12 - Prob. 12.11PAECh. 12 - An equilibrium involving the carbonate and...Ch. 12 - Prob. 12.13PAECh. 12 - A small quantity of a soluble salt is placed in...Ch. 12 - Prob. 12.15PAECh. 12 - Prob. 12.16PAECh. 12 - Write equilibrium (mass action) expressions for...Ch. 12 - What is the difference between homogeneous...Ch. 12 - Write equilibrium expressions for each of the...Ch. 12 - Write equilibrium expressions for each of the...Ch. 12 - Prob. 12.21PAECh. 12 - Which of the following is more likely to...Ch. 12 - 12.17 Which of the following is more likely to...Ch. 12 - The reaction, 3 H2(g) + N2(g) (g), has the fol...Ch. 12 - 12.19 For each of the following equations, write...Ch. 12 - Consider the following equilibria involving SO2(g)...Ch. 12 - Prob. 12.27PAECh. 12 - Prob. 12.28PAECh. 12 - Prob. 12.29PAECh. 12 - Prob. 12.30PAECh. 12 - Prob. 12.31PAECh. 12 - The following data were collected for the...Ch. 12 - The following data were collected for a system at...Ch. 12 - Prob. 12.34PAECh. 12 - Nitrosyl chloride, NOCI, decomposes to NO and Cl,...Ch. 12 - Hydrogen gas and iodine gas react via the...Ch. 12 - 12.31 A system consisting of 0.100 mole of oxygen...Ch. 12 - Prob. 12.38PAECh. 12 - Prob. 12.39PAECh. 12 - 1’he reaction in Exercise 12.33 was repeated. This...Ch. 12 - In the reaction in Exercise 12.33, another trial...Ch. 12 - The experiment in Exercise 12.33 was redesigned so...Ch. 12 - Again the experiment in Exercise 12.33 was...Ch. 12 - At a particular temperature, the equilibrium...Ch. 12 - A student is simulating the carbonic acid—hydrogen...Ch. 12 - Because carbonic acid undergoes a second...Ch. 12 - Because calcium carbonate is a sink for CO32- in a...Ch. 12 - 12.42 The following reaction is in equilibrium in...Ch. 12 - In the following equilibrium in a closed system,...Ch. 12 - In each of the reactions, how does the equilibrium...Ch. 12 - Prob. 12.51PAECh. 12 - Prob. 12.52PAECh. 12 - The decomposition of NH4HS, NH 4 HS( s )NH3( g )+...Ch. 12 - Consider the following system: 4NH 3 ( g )+ 3O 2 (...Ch. 12 - The following equilibrium is established in a...Ch. 12 - Write the K_, expression for each of the following...Ch. 12 - Prob. 12.57PAECh. 12 - calculate the molar solubility of the following...Ch. 12 - 12.49 The Safe Drinking Water Act of 1974...Ch. 12 - In Exercise 12.49, what is the allowed...Ch. 12 - Prob. 12.61PAECh. 12 - Because barium sulfate is opaque to X-rays, it is...Ch. 12 - The ore cinnabar (HgS) is an important source of...Ch. 12 - Prob. 12.64PAECh. 12 - From the solubility data given for the following...Ch. 12 - The solubility of magnesium fluoride, MgF2, in...Ch. 12 - Solid Na2SO4 is added slowly to a solution that is...Ch. 12 - Will a precipitate of Mg(OH)2 form when 25.0 mL of...Ch. 12 - Use the web to look up boiler scale and explain...Ch. 12 - Prob. 12.70PAECh. 12 - Prob. 12.71PAECh. 12 - 12.62 Write the formula of the conjugate acid of...Ch. 12 - 12.63 For each of the following reactions,...Ch. 12 - What are the products of each of the following...Ch. 12 - Prob. 12.75PAECh. 12 - Prob. 12.76PAECh. 12 - 12.67 Hydrofluoric acid is a weak acid used in the...Ch. 12 - The pH of a 0.129 M solution of a weak acid, HB,...Ch. 12 - Calculate the pH of a 0.10 M solution of propanoic...Ch. 12 - Find the pH of a 0.115 M solution of NH3(aq).Ch. 12 - Acrylic acid is used in the polymer industry in...Ch. 12 - Prob. 12.82PAECh. 12 - Prob. 12.83PAECh. 12 - In a particular experiment, the equilibrium...Ch. 12 - Prob. 12.85PAECh. 12 - Prob. 12.86PAECh. 12 - Prob. 12.87PAECh. 12 - Prob. 12.88PAECh. 12 - Prob. 12.89PAECh. 12 - Prob. 12.90PAECh. 12 - Prob. 12.91PAECh. 12 - Prob. 12.92PAECh. 12 - Solid CaCO3 ; is placed in a closed container and...Ch. 12 - 12.100 A reaction important in smog formation is...Ch. 12 - 12.101 An engineer working on a design to extract...Ch. 12 - 12.102 A chemical engineer is working to optimize...Ch. 12 - 12.103 Methanol, CH3OH, can be produced by the...Ch. 12 - Prob. 12.98PAECh. 12 - 12.105 Using the kinetic-molecular theory, explain...Ch. 12 - 12.106 The solubility of KCl is 34.7 g per 100 g...Ch. 12 - Prob. 12.101PAECh. 12 - 12.108 A nuclear engineer is considering the...Ch. 12 - 12.109 Copper(II) iodate has a solubility of 0.136...Ch. 12 - 12.110 In Exercise 12.109, what do you predict...Ch. 12 - 12.111 You have three white solids. What...Ch. 12 - Prob. 12.106PAECh. 12 - Prob. 12.107PAECh. 12 - Prob. 12.108PAECh. 12 - Prob. 12.109PAECh. 12 - Prob. 12.110PAECh. 12 - 12.117 The vapor pressure of water at 80.0 °C is...Ch. 12 - Prob. 12.112PAE
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- The following two diagrams represent the composition of an equilibrium mixture for the reaction A2 + B2 2AB at two different temperatures. Based on the diagrams, is the chemical reaction endothermic or exothermic? Explain your answer using Le Chteliers principle. (A atoms are red and B atoms are green in the diagrams.)arrow_forwardWrite 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_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_forward
- Write 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_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_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
- Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.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_forwardKc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?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 diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.arrow_forwardAt 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_forward
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