Chemistry: An Atoms-Focused Approach
1st Edition
ISBN: 9780393124200
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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Chapter 12 Solutions
Chemistry: An Atoms-Focused Approach
Ch. 12 - Prob. 12.1VPCh. 12 - Prob. 12.2VPCh. 12 - Prob. 12.4VPCh. 12 - Prob. 12.5VPCh. 12 - Prob. 12.6VPCh. 12 - Prob. 12.8VPCh. 12 - Prob. 12.9VPCh. 12 - Prob. 12.10VPCh. 12 - Prob. 12.11QACh. 12 - Prob. 12.12QA
Ch. 12 - Prob. 12.13QACh. 12 - Prob. 12.14QACh. 12 - Prob. 12.15QACh. 12 - Prob. 12.16QACh. 12 - Prob. 12.17QACh. 12 - Prob. 12.18QACh. 12 - Prob. 12.19QACh. 12 - Prob. 12.20QACh. 12 - Prob. 12.21QACh. 12 - Prob. 12.22QACh. 12 - Prob. 12.23QACh. 12 - Prob. 12.24QACh. 12 - Prob. 12.25QACh. 12 - Prob. 12.26QACh. 12 - Prob. 12.27QACh. 12 - Prob. 12.28QACh. 12 - Prob. 12.29QACh. 12 - Prob. 12.30QACh. 12 - Prob. 12.31QACh. 12 - Prob. 12.32QACh. 12 - Prob. 12.33QACh. 12 - Prob. 12.34QACh. 12 - Prob. 12.35QACh. 12 - Prob. 12.36QACh. 12 - Prob. 12.37QACh. 12 - Prob. 12.38QACh. 12 - Prob. 12.39QACh. 12 - Prob. 12.40QACh. 12 - Prob. 12.41QACh. 12 - Prob. 12.42QACh. 12 - Prob. 12.43QACh. 12 - Prob. 12.44QACh. 12 - Prob. 12.45QACh. 12 - Prob. 12.46QACh. 12 - Prob. 12.47QACh. 12 - Prob. 12.48QACh. 12 - Prob. 12.49QACh. 12 - Prob. 12.50QACh. 12 - Prob. 12.51QACh. 12 - Prob. 12.52QACh. 12 - Prob. 12.53QACh. 12 - Prob. 12.54QACh. 12 - Prob. 12.55QACh. 12 - Prob. 12.56QACh. 12 - Prob. 12.57QACh. 12 - Prob. 12.58QACh. 12 - Prob. 12.59QACh. 12 - Prob. 12.60QACh. 12 - Prob. 12.61QACh. 12 - Prob. 12.62QACh. 12 - Prob. 12.63QACh. 12 - Prob. 12.64QACh. 12 - Prob. 12.65QACh. 12 - Prob. 12.66QACh. 12 - Prob. 12.67QACh. 12 - Prob. 12.68QACh. 12 - Prob. 12.69QACh. 12 - Prob. 12.70QACh. 12 - Prob. 12.71QACh. 12 - Prob. 12.72QACh. 12 - Prob. 12.73QACh. 12 - Prob. 12.74QACh. 12 - Prob. 12.75QACh. 12 - Prob. 12.76QACh. 12 - Prob. 12.77QACh. 12 - Prob. 12.78QACh. 12 - Prob. 12.79QACh. 12 - Prob. 12.80QACh. 12 - Prob. 12.81QACh. 12 - Prob. 12.82QACh. 12 - Prob. 12.83QACh. 12 - Prob. 12.84QACh. 12 - Prob. 12.85QACh. 12 - Prob. 12.86QA
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- What is entropy? Why is entropy important?arrow_forwardSpontaneous Processes Which of the following processes are spontaneous? (a) building a sand castle (b) outlining your chemistry notes (c) wind scattering leaves in a pilearrow_forwardIdentify each of the processes listed as spontaneous or non-spontaneous. For each non spontaneous process, describe the corresponding spontaneous process in the opposite direction. (a) Oxygen molecules dissociate to form oxygen atoms. (b) A tray of water is placed in the sun on a warm day and freezes. (c) A solution of salt water forms a layer of acid on top of a layer of base. (d) Silver nitrate is added to a solution of sodium chloride and a precipitate forms. (e) Sulfuric acid sitting in a beaker turns into water by giving off gaseous SO3.arrow_forward
- What is a spontaneous process? Give three examples of spontaneous processes. Give three examples of nonspontaneous processes.arrow_forwardDecide whether the following processes will be spontaneous, and why. The why can be general, not specific. a Ice melting at 5C b Ice melting at +5C c KBr(s) dissolving in water d An unplugged refrigerator getting cold e A leaf falling from a tree to the ground f The reaction Li(s)+12F2(g)LiF(s) g The reaction H2O(l)H2(g)+12O2(g)arrow_forwardDescribe the energy and entropy changes that occur in the following processes, and indicate whether the processes are spontaneous under the conditions stated: a.On a cold day, water freezes. b.A container of water at 40C cools to room temperature. c.The odor from an open bottle of perfume spreads throughout a room.arrow_forward
- What happens to the entropy of the universe during a spontaneous process?arrow_forwardDetermine whether each of the following statements is true or false. If false, modify to make the statement true. (a) An exothermic reaction is spontaneous. (b) When G is positive, the reaction cannot occur under any conditions. (c) S is positive for a reaction in which there is an increase in the number of moles. (d) If H and S are both negative, G will he negative.arrow_forwardWhich of the following are spontaneous processes? a A cube of sugar dissolves in a cup of hot tea. b A rusty crowbar turns shiny. c Butane from a lighter burns in air. d A clock pendulum, initially stopped, begins swinging. e Hydrogen and oxygen gases bubble out from a glass of pure water.arrow_forward
- Use the standard entropy data in Appendix G to determine the change in entropy for each of the reactions listed in Exercise 16.34. All the processes occur at the standard conditions and 25 C.arrow_forwardUsing tabulated thermodynamic data, calculate G for these reactions. (a) Mg3N2(s)+6H2O(l)2NH3(g)+3Mg(OH)2(s) (b) 4CH3NH2(g)+9O2(g)4CO2(g)+10H2O(l)+2N2(g) (c) Fe3O(s)+4CO(g)3Fe(s)+4CO2(g) (d) P4O10(s)+6H2O(l)4H3PO4(aq)arrow_forwardThere is another free energy state function, the Helmholtz free energy (A), defined as A = E — TS. Comparing this to the definition of G, we see that internal energy has replaced enthalpy in the definition. Under what conditions would this free energy tell us whether or not a process is spontaneous?arrow_forward
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