Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 18, Problem 4PS
Identify the following processes as either spontaneous or not spontaneous.
- (a) Liquid water turns to ice when placed in a freezer at −5 °C.
- (b) Nitrogen gas is compressed to one half its original volume.
- (c) Sodium reacts with water forming H2(g) and NaOH(aq).
- (d) Slightly soluble CaSO4 [Ksp = 4.5 × 10−5) dissolves in water to form a saturated solution.
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Chapter 18 Solutions
Chemistry & Chemical Reactivity
Ch. 18.3 - Predict which substance in each pair has the...Ch. 18.3 - Prob. 18.2CYUCh. 18.4 - Based on rH and rS, predict the spontaneity of the...Ch. 18.6 - Prob. 18.4CYUCh. 18.6 - Prob. 18.5CYUCh. 18.6 - Oxygen was first prepared by Joseph Priestley...Ch. 18.6 - Prob. 18.7CYUCh. 18.6 - Prob. 18.8CYUCh. 18.6 - Prob. 18.9CYUCh. 18.7 - Consider the hydrolysis reactions of creatine...
Ch. 18.7 - Prob. 1.2ACPCh. 18.7 - The decomposition of diamond to graphite...Ch. 18.7 - It has been demonstrated that buckminsterfullerene...Ch. 18 - Solid NH4NO3 is placed in a beaker containing...Ch. 18 - Acetic acid, a weak acid, was added to a beaker...Ch. 18 - Identify the following processes as either...Ch. 18 - Identify the following processes as either...Ch. 18 - Prob. 5PSCh. 18 - Predict whether each of the following processes...Ch. 18 - Indicate which of the following processes are...Ch. 18 - Prob. 8PSCh. 18 - Prob. 9PSCh. 18 - Prob. 10PSCh. 18 - Prob. 11PSCh. 18 - Calculate the entropy change that occurs when 1.00...Ch. 18 - Prob. 13PSCh. 18 - Calculate the change in entropy of a system with...Ch. 18 - The third law of thermodynamics says that a...Ch. 18 - Identify trends in S values: (a) For the halogens:...Ch. 18 - Which substance has the higher entropy? (a) dry...Ch. 18 - Which substance has the higher entropy? (a) a...Ch. 18 - Use S values to calculate the standard entropy...Ch. 18 - Use S values to calculate the standard entropy...Ch. 18 - Calculate the standard entropy change for the...Ch. 18 - Calculate the standard entropy change for the...Ch. 18 - Calculate the standard entropy change for the...Ch. 18 - Calculate the standard entropy change for the...Ch. 18 - Is the reaction Si(s) + 2 Cl2(g) SiCl4(g)...Ch. 18 - Is the reaction Si(s) + 2 H2(g) SiH4(g)...Ch. 18 - Calculate S(universe) for the decomposition of 1...Ch. 18 - Calculate S(universe) for the formation of 1 mol...Ch. 18 - Classify each of the reactions according to one of...Ch. 18 - Classify each of the reactions according to one of...Ch. 18 - Using values of fH and S, calculate rG for each of...Ch. 18 - Using values of fH and S, calculate rG for each of...Ch. 18 - Using values of fH and S, calculate the standard...Ch. 18 - Using values of fH and S, calculate the standard...Ch. 18 - Using values of fG, calculate rG for each of the...Ch. 18 - Using values of fG, calculate rG for each of the...Ch. 18 - For the reaction BaCO3(s) BaO(s) + CO2(g), rG =...Ch. 18 - For the reaction TiCl2(s) + Cl2(g) TiCl4(), rG =...Ch. 18 - Determine whether the reactions listed below are...Ch. 18 - Determine whether the reactions listed below are...Ch. 18 - Heating some metal carbonates, among them...Ch. 18 - Calculate rH and rS for the reaction of tin(IV)...Ch. 18 - The ionization constant, Ka, for acetic acid is...Ch. 18 - Prob. 44PSCh. 18 - The standard free energy change, rG, for the...Ch. 18 - Prob. 46PSCh. 18 - Calculate rG at 25 C for the formation of 1.00 mol...Ch. 18 - Prob. 48PSCh. 18 - Prob. 49PSCh. 18 - Prob. 50PSCh. 18 - Compare the compounds in each set below and decide...Ch. 18 - Using standard entropy values, calculate rS for...Ch. 18 - About 5 billion kilograms of benzene, C6H6, are...Ch. 18 - Hydrogenation, the addition of hydrogen to an...Ch. 18 - Is the combustion of ethane, C2H6, product-favored...Ch. 18 - Prob. 56GQCh. 18 - When vapors from hydrochloric acid and aqueous...Ch. 18 - Calculate S(system), S(surroundings), and...Ch. 18 - Methanol is now widely used as a fuel in race...Ch. 18 - The enthalpy of vaporization of liquid diethyl...Ch. 18 - Calculate the entropy change, rS, for the...Ch. 18 - Using thermodynamic data, estimate the normal...Ch. 18 - Prob. 63GQCh. 18 - When calcium carbonate is heated strongly, CO2 gas...Ch. 18 - Sodium reacts violently with water according to...Ch. 18 - Yeast can produce ethanol by the fermentation of...Ch. 18 - Elemental boron, in the form of thin fibers, can...Ch. 18 - Prob. 68GQCh. 18 - Prob. 69GQCh. 18 - Estimate the boiling point of water in Denver,...Ch. 18 - The equilibrium constant for the butane ...Ch. 18 - A crucial reaction for the production of synthetic...Ch. 18 - Calculate rG for the decomposition of sulfur...Ch. 18 - Prob. 74GQCh. 18 - A cave in Mexico was recently discovered to have...Ch. 18 - Wet limestone is used to scrub SO2 gas from the...Ch. 18 - Sulfur undergoes a phase transition between 80 and...Ch. 18 - Calculate the entropy change for dissolving HCl...Ch. 18 - Some metal oxides can be decomposed to the metal...Ch. 18 - Prob. 80ILCh. 18 - Prob. 81ILCh. 18 - Prob. 82ILCh. 18 - Titanium(IV) oxide is converted to titanium...Ch. 18 - Cisplatin [cis-diamminedichloroplatinum(II)] is a...Ch. 18 - Prob. 85ILCh. 18 - Explain why each of the following statements is...Ch. 18 - Decide whether each of the following statements is...Ch. 18 - Under what conditions is the entropy of a pure...Ch. 18 - Prob. 89SCQCh. 18 - Consider the formation of NO(g) from its elements....Ch. 18 - Prob. 91SCQCh. 18 - The normal melting point of benzene, C6H6, is 5.5...Ch. 18 - Prob. 93SCQCh. 18 - For each of the following processes, predict the...Ch. 18 - Heater Meals are food packages that contain their...Ch. 18 - Prob. 96SCQCh. 18 - Prob. 97SCQCh. 18 - Prob. 98SCQCh. 18 - Iodine, I2, dissolves readily in carbon...Ch. 18 - Prob. 100SCQCh. 18 - Prob. 101SCQCh. 18 - Prob. 102SCQCh. 18 - Prob. 103SCQCh. 18 - Prob. 104SCQCh. 18 - The Haber-Bosch process for the production of...Ch. 18 - Prob. 106SCQCh. 18 - Prob. 107SCQ
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- Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)arrow_forwardWhat is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the synthesis of ammonia? 3H2(g) + N2(g) 2NH3(g)arrow_forwardChemists and engineers who design nuclear power plants have to worry about high-temperature reactions because it is possible for water to decompose. (a) Under what conditions does this reaction occur spontaneously? 2H2O(g) 2H2(g) + O2(g) (b) Under conditions where the decomposition of water is spontaneous, do nuclear engineers have to worry about an oxygen/hydrogen explosion? Justify your answer.arrow_forward
- What types of experiments can be carried out to determine whether a reaction is spontaneous? Does spontaneity have any relationship to the final equilibrium position of a reaction? Explain.arrow_forwardActually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).arrow_forwardFor each of the following processes, identify the systemand the surroundings. Identify those processes that arespontaneous. For each spontaneous process, identify theconstraint that has been removed to enable the process to occur: Ammonium nitrate dissolves in water. Hydrogen and oxygen explode in a closed bomb. A rubber band is rapidly extended by a hangingweight. The gas in a chamber is slowly compressed by aweighted piston. A glass shatters on the floor.arrow_forward
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- Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().arrow_forwardUse data from Appendix D to calculate the standardentropy change at 25°C for the reaction CH3COOH(g)+NH3(g)CH3NH2(g)+CO2(g)+H2(g) Suppose that 1.00 mol each of solid acetamide, CH3CONH2(s), and water, H2O(l), react to give thesame products. Will the standard entropy change belarger or smaller than that calculated for the reactionin part (a)?arrow_forwardThere are millions of organic compounds known, and new ones are being discovered or made at a rate of morethan 100,000 compounds per year. Organic compoundsburn readily in air at high temperatures to form carbondioxide and water. Several classes of organic compoundsare listed, with a simple example of each. Write a balanced chemical equation for the combustion in O2ofeach of these compounds, and then use the data inAppendix J to show that each reaction is product-favoredat room temperature. From these results, it is reasonable to hypothesize thatallorganic compounds are thermodynamically unstable inan oxygen atmosphere (that is, their room-temperaturereaction with O2(g) to form CO2(g) and H2O() isproduct-favored). If this hypothesis is true, how canorganic compounds exist on Earth?arrow_forward
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