Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
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Textbook Question
Chapter 16, Problem 31E
A reaction has
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Chapter 16 Solutions
Chemistry by OpenStax (2015-05-04)
Ch. 16 - What is a spontaneous reaction?Ch. 16 - What is a nonspontaneous reaction?Ch. 16 - Indicate whether the following processes are...Ch. 16 - A helium-filled balloon spontaneously deflates...Ch. 16 - Many plastic materials are organic polymers that...Ch. 16 - In Figure 16.8 all possible distributions and...Ch. 16 - In Figure 16.8 all of the possible distributions...Ch. 16 - How does the process described in the previous...Ch. 16 - Consider a system similar to the one in Figure...Ch. 16 - Consider the system shown in Figure 16.9. What is...
Ch. 16 - Consider the system shown in Figure 16.9. What is...Ch. 16 - Arrange the following sets of systems in order of...Ch. 16 - At room temperature, the entropy of the halogens...Ch. 16 - Consider two processes: sublimation of I2(s) and...Ch. 16 - Indicate which substance in the given pairs has...Ch. 16 - Predict the sign of the entropy change for the...Ch. 16 - Predict the sign of the entropy change for the...Ch. 16 - Write the balanced chemical equation for the...Ch. 16 - Write the balanced chemical equation for the...Ch. 16 - What is the difference between S, S , and S 298...Ch. 16 - Calculate S298 for the following changes. (a)...Ch. 16 - Determine the entropy change for the combustion of...Ch. 16 - Determine the entropy change for the combustion of...Ch. 16 - Thermite reactions have been used for welding...Ch. 16 - Using the relevant S 298 values listed in Appendix...Ch. 16 - From the following information, determine S298 for...Ch. 16 - By calculating Suniv, at each temperature,...Ch. 16 - Use the standard entropy data in Appendix G to...Ch. 16 - Use the standard entropy data in Appendix G to...Ch. 16 - What is the difference between G, G, and G 298 for...Ch. 16 - A reaction has H298=100 kj/mol and S298=250 J/mol ...Ch. 16 - Explain what happens as a reaction starts with G0...Ch. 16 - Use the standard free energy of formation data in...Ch. 16 - Use the standard free energy data in Appendix G to...Ch. 16 - Given: P4(s)+5O2(g)P4O10(s)G298=2697.0kJ/mol...Ch. 16 - Is the formation of ozone (O3(g)) from oxygen...Ch. 16 - Consider the decomposition of red mercury(II)...Ch. 16 - Among other things, an ideal fuel for the control...Ch. 16 - Calculate G for each of the following reactions...Ch. 16 - Calculate G for each of the following reactions...Ch. 16 - Calculate the equilibrium constant at 25 C for...Ch. 16 - Calculate the equilibrium constant at 25 C for...Ch. 16 - Calculate the equilibrium constant temperature...Ch. 16 - Calculate the equilibrium constant temperature...Ch. 16 - Consider the following reaction at 298 K:...Ch. 16 - Determine the normal boiling point (in kelvin) of...Ch. 16 - Under what conditions is N2O3(g)NO(g)+NO2(g)...Ch. 16 - At mom temperature, the equilibrium constant (Kw)...Ch. 16 - Hydrogen sulfide is a pollutant found in natural...Ch. 16 - Consider the decomposition of CaCO3(s) into CaO(s)...Ch. 16 - In the laboratory, hydrogen chloride (HCl(g)) and...Ch. 16 - Benzene can be prepared from acetylene....Ch. 16 - Carbon dioxide decomposes into CO and O2 at...Ch. 16 - Carbon tetrachloride, an important industrial...Ch. 16 - Acetic acid, CH3CO2H, can form a dimer,...Ch. 16 - Nitric acid, HNO3, can be prepared by the...Ch. 16 - Determine G for the following reactions. (a)...Ch. 16 - Given that the Gf for Pb2+(aq) and Cl-(aq) is...Ch. 16 - Determine the standard free energy change, Gf, for...Ch. 16 - Determine the standard enthalpy change, entropy...Ch. 16 - The evaporation of one mole of water at 298 K has...Ch. 16 - In glycolysis, the reaction of glucose (Glu) to...Ch. 16 - One of the important reactions in the biochemical...Ch. 16 - Without doing a numerical calculation, determine...Ch. 16 - When ammonium chloride is added to water and...Ch. 16 - An important source of copper is from the copper...Ch. 16 - What happens to G (becomes more negative or more...
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- What 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_forwardConsider the reaction of 2 mol H2(g) at 25C and 1 atm with 1 mol O2(g) at the same temperature and pressure to produce liquid water at these conditions. If this reaction is run in a controlled way to generate work, what is the maximum useful work that can be obtained? How much entropy is produced in this case?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
- Solid NH4NO3 is placed in a beaker containing water at 25 C. When the solid has completely dissolved, the temperature of the solution is 23.5 C. (a) Was the process exothermic or endothermic? (b) Was the process spontaneous? (c) Did the entropy of the system increase? (d) Did the entropy of the universe increase?arrow_forwardDefine the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universearrow_forwardConsider the reaction of 1 mol H2(g) at 25C and 1 atm with 1 mol Br2(l) at the same temperature and pressure to produce gaseous HBr at these conditions. If this reaction is run in a controlled way to generate work, what is the maximum useful work that can be obtained? How much entropy is produced in this case?arrow_forward
- The combustion of acetylene, C2H2, is a spontaneous reaction given by the equation 2C2H2(g)+5O2(g)4CO2(g)+2H2O(l) As expected for a combustion, the reaction is exothermic. What is the sign of H? What do you expect for the sign of S? Explain the spontaneity of the reaction in terms of the enthalpy and entropy changes.arrow_forwardThe free energy for a reaction decreases as temperature increases. Explain how this observation is used to determine the sign of either H or S.arrow_forwardWhich contains greater entropy, a quantity of frozen benzene or the same quantity of liquid benzene at the same temperature? Explain in terms of the dispersal of energy in the substance.arrow_forward
- a Calculate K1, at 25C for sulfurous acid: H2SO3(aq)H+(aq)+HSO3(aq) b Which thermodynamic factor is the most significant in accounting for the fact that sulfurous acid is a weak acid? Why?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_forwardIndicate whether the following processes are spontaneous or nonspontaneous. (a) Liquid water freezing at a temperature below its freezing point (b) Liquid water freezing at a temperature above its freezing point (c) The combustion of gasoline (d) A ball thrown into the air (e) A raindrop falling to the ground (f) Iron rusting in a moist atmospherearrow_forward
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