PRINCIPLES+REACTIONS
8th Edition
ISBN: 9781337759632
Author: Masterton
Publisher: CENGAGE L
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Chapter 16, Problem 44QAP
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Chapter 16 Solutions
PRINCIPLES+REACTIONS
Ch. 16 - Spontaneous Processes Which of the following...Ch. 16 - Which of the following processes are spontaneous?...Ch. 16 - Which of the following processes are spontaneous?...Ch. 16 - Which of the following processes are spontaneous?...Ch. 16 - On the basis of your experience, predict which...Ch. 16 - On the basis of your experience, predict which of...Ch. 16 - In each of the following pairs, choose the...Ch. 16 - In each of the following pairs, choose the...Ch. 16 - Predict the sign of ΔS for the following: (a) a...Ch. 16 - Predict the sign of S for the following: (a)...
Ch. 16 - Predict the sign of S for each of the following...Ch. 16 - Predict the sign of S for each of the following...Ch. 16 - Predict the sign of S for each of the following...Ch. 16 - Predict the sign of S for each of the following...Ch. 16 - Predict the order of the following reactions in...Ch. 16 - Predict the order of the following reactions in...Ch. 16 - Use Table 16.1 to calculate S for each of the...Ch. 16 - Prob. 18QAPCh. 16 - Use Table 16.1 to calculate S for each of the...Ch. 16 - Use Table 16.1 to calculate S for each of the...Ch. 16 - Prob. 21QAPCh. 16 - Prob. 22QAPCh. 16 - Calculate G at 82C for reactions in which (a)...Ch. 16 - Calculate G at 72C for reactions in which (a)...Ch. 16 - Calculate G at 355 K for each of the reactions in...Ch. 16 - Calculate G at 415 K for each of the reactions in...Ch. 16 - From the values for G f given in Appendix 1,...Ch. 16 - Follow the directions of Problem 27 for each of...Ch. 16 - Use standard entropies and heats of formation to...Ch. 16 - Follow the directions of Question 29 for the...Ch. 16 - It has been proposed that wood alcohol, CH3OH, a...Ch. 16 - Prob. 32QAPCh. 16 - Sodium carbonate, also called washing soda, can be...Ch. 16 - The reaction between magnesium metal and water (l)...Ch. 16 - In the laboratory, POCl3 (phosphorus oxychloride)...Ch. 16 - Oxygen can be made in the laboratory by reacting...Ch. 16 - Phosgene, COCl2, can be formed by the reaction of...Ch. 16 - When permanganate ions in aqueous solution react...Ch. 16 - Discuss the effect of temperature change on the...Ch. 16 - Discuss the effect of temperature on the...Ch. 16 - At what temperature does G become zero for each of...Ch. 16 - Over what temperature range are the reactions in...Ch. 16 - For the reaction...Ch. 16 - For the reaction...Ch. 16 - For the decomposition of Ag2O:...Ch. 16 - Consider the following hypothetical equation...Ch. 16 - Prob. 47QAPCh. 16 - Prob. 48QAPCh. 16 - Red phosphorus is formed by heating white...Ch. 16 - Organ pipes in unheated churches develop tin...Ch. 16 - Prob. 51QAPCh. 16 - Pencil lead is almost pure graphite. Graphite is...Ch. 16 - Given the following data for sodium Na(s): S =51.2...Ch. 16 - Given the following data for bromine: Br2(l); S...Ch. 16 - Show by calculation, using Appendix 1, whether...Ch. 16 - Show by calculation whether the reaction HF(aq)...Ch. 16 - For the reaction...Ch. 16 - For the reaction...Ch. 16 - Consider the reaction 2SO2(g)+O2(g)2SO3(g) (a)...Ch. 16 - Consider the reaction AgCl(s)Ag+(aq)+Cl(aq) (a)...Ch. 16 - Consider the reaction CO(g)+H2O(g)CO2(g)+H2(g) Use...Ch. 16 - Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use ...Ch. 16 - Consider the following reaction at 25C:...Ch. 16 - Consider the reaction N2O(g)+NO2(g)3NO(g)K=4.41019...Ch. 16 - For the reaction...Ch. 16 - Consider the decomposition of N2O4 at 100C....Ch. 16 - Use the values for G f in Appendix 1 to calculate...Ch. 16 - Given that H f for HF(aq) is -320.1 kJ/mol and S...Ch. 16 - At 25C, a 0.327 M solution of a weak acid HX has a...Ch. 16 - A 0.250 M solution of a weak base R2NH has a pH of...Ch. 16 - Prob. 71QAPCh. 16 - Given the following standard free energies at 25°C...Ch. 16 - Natural gas, which is mostly methane, CH4, is a...Ch. 16 - Prob. 74QAPCh. 16 - When glucose, C6H12O11, is metabolized to CO2 and...Ch. 16 - Consider the following reactions at 25°C:...Ch. 16 - At 1200 K, an equilibrium mixture of CO and CO2...Ch. 16 - Prob. 78QAPCh. 16 - Prob. 79QAPCh. 16 - Prob. 80QAPCh. 16 - Prob. 81QAPCh. 16 - Carbon monoxide poisoning results when carbon...Ch. 16 - Prob. 83QAPCh. 16 - Determine whether each of the following statements...Ch. 16 - Which of the following quantities can be taken to...Ch. 16 - Fill in the blanks: (a) H° and G° become equal at...Ch. 16 - Fill in the blanks: (a) At equilibrium, G is. (b)...Ch. 16 - Prob. 88QAPCh. 16 - Consider the following reaction with its...Ch. 16 - Consider the graph below: (a) Describe the...Ch. 16 - Prob. 91QAPCh. 16 - Prob. 92QAPCh. 16 - Prob. 93QAPCh. 16 - Hf for iodine gas is 62.4 kJ/mol, and S° is 260.7...Ch. 16 - Prob. 95QAPCh. 16 - The overall reaction that occurs when sugar is...Ch. 16 - Hydrogen has been suggested as the fuel of the...Ch. 16 - When a copper wire is exposed to air at room...Ch. 16 - Kafor acetic acid (HC2H3O2) at 25°C is 1.754105 ....Ch. 16 - Consider the reaction 2HI(g)H2(g)+I2(g)At 500C a...Ch. 16 - Prob. 101QAPCh. 16 - Consider the formation of HI(g) from H2(g) and...
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- Actually, 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_forwardWhat is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)arrow_forward
- There 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_forwardUsing values of fH and S, calculate rG for each of the following reactions at 25 C. (a) 2 Na(s) + 2 H2O() 2 NaOH(aq) + H2(g) (b) 6 C(graphite) + 3 H2(g) C6H6() Which of these reactions is (are) predicted to be product-favored at equilibrium? Are the reactions enthalpy- or entropy-driven?arrow_forwardFrom the values for G f given in Appendix 1, calculate G at 25C for each of the reactions in Question 19.arrow_forward
- 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_forwardCalculate G at 355 K for each of the reactions in Question 17. State whether the reactions are spontaneous.arrow_forwardFor the reaction TiCl2(s) + Cl2(g) TiCl4(), rG = 272.8 kj/mol-txn. Using this value and other data available in Appendix L, calculate the value of fG for TiCl2(s).arrow_forward
- For each process, predict whether entropy increases or decreases, and explain how you arrived at your prediction. 2 CO2(g) → 2 CO(g) + O2(g) NaCl(s) → NaCl(aq) MgCO3(s) → MgO(s) + CO2(g)arrow_forwardCalculate 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_forwardYeast can produce ethanol by the fermentation of glucose (C6H12O6), which is the basis for the production of most alcoholic beverages. C6H12O6(aq) 2 C2H5OH() + 2 CO2(g) Calculate rH, rS, and rG for the reaction at 25 C. Is the reaction product- or reactant-favored at equilibrium? In addition to the thermodynamic values in Appendix L, you will need the following data for C6H12O6(aq): fH = 1260.0 kl/mol; S = 289 J/K mol; and fG = 918.8 kl/mol.arrow_forward
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