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APPLY 14.12 Magnesium hydroxide is the active ingredient in the antacid milk of magnesia.What is the value of Kc if solid magnesium hydroxide is dissolved in water and equilibrium concentrations are
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Chapter 14 Solutions
Chemistry
- Draw a nanoscale (particulate) level diagram for an equilibrium mixture ofarrow_forwardSuppose 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_forwardConsider 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_forward
- At 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_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_forwardConsider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the amount of ammonia at equilibrium be affected by 1. removing O2(g)? 2. adding N2(g)? 3. adding water? 4. expanding the container at constant pressure? 5. increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forward
- The decomposition of NH4HS, NH 4 HS( s )NH3( g )+ H 2 S( g ) is an endothermic process. Using Le Chatelier's principle, explain how increasing the temperature would affect the equilibrium. If more NH4HS is added to a flask in which this equilibrium exists, how is the equilibrium affected? What if some additional NH3 is placed in the flask? What will happen to the pressure of NH3 if some H2S is removed from the flask?arrow_forwardEquilibrium exists between butane and isobutane when [butane] = 0.020 M and [isobutane] = 0.050 M. An additional 0.0200 mol/L of isobutane is added to the mixture. What are the concentrations of butane and isobutane after equilibrium has again been attained?arrow_forwardConsider the following equilibrium constants. Describe how you would expect the equilibrium concentrations of reactants and products to compare with each other larger than, smaller than, etc. for each case. a. K=2.1106 b. K=0.15 c. K=1.2108 d. K=0.00036arrow_forward
- For the following reactions, predict whether the pressure of the reactants or products increases or remains the same when the volume of the reaction vessel is increased. (a) H2O(l)H2O(g) (b) N2(g)+3H2(g)2NH3(g) (c) C2H4(g)+H2O(g)C2H5OH(g)arrow_forwardA small quantity of a soluble salt is placed in water. Equilibrium between dissolved and undissolved salt may or may not be attained. Explain.arrow_forward
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