Chemistry: Principles and Practice 3rd Edition
ISBN: 9780534420123
Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
1 Introduction To Chemistry 2 Atoms, Molecules, And Ions 3 Equation, The Mole, And Chemical Formulas 4 Chemical Reactions In Solution 5 Thermochemistry 6 The Gaseous State 7 Electronic Structure 8 The Periodic Table: Structure And Trends 9 Chemical Bonds 10 Molecular Structure And Bonding Theories 11 Liquids And Solids 12 Solutions 13 Chemical Kinetics 14 Chemical Equilibrium 15 Solutions Of Acids And Bases 16 Reactions Between Acids And Bases 17 Chemcial Thermodynamics 18 Electrochemistry 19 Transitition Metals, Coordination Chemistry And Metallurgy 20 Chemistry Of Hydrogen, Elements In Group 3a Through 6a, And The Noble Gases 21 Nuclear Chemistry 22 Organic Chemistry And Biochemistry Chapter17: Chemcial Thermodynamics
Chapter Questions Section: Chapter Questions
Problem 17.1QE Problem 17.2QE: How is the sign of q, heat, defined? How does it relate to the total energy of the system? Problem 17.3QE: Identify the sign of the work when a fuel-oxygen mixture (the system) burns, propelling an... Problem 17.4QE: What is the sign of the work when a refrigerator compresses a gas (the system) to a liquid during... Problem 17.5QE: When a rocket is launched, the burning gases are the source of the motion. If the system is the... Problem 17.6QE Problem 17.7QE Problem 17.8QE Problem 17.9QE Problem 17.10QE: Explain why absolute enthalpies and energies cannot be measured, and only changes can be determined. Problem 17.11QE: Explain why absolute entropies can be measured. Problem 17.12QE: Under what conditions is the entropy of a substance equal to zero? Problem 17.13QE Problem 17.14QE Problem 17.15QE Problem 17.16QE Problem 17.17QE Problem 17.18QE Problem 17.19QE: The free energy for a reaction decreases as temperature increases. Explain how this observation is... Problem 17.20QE: The equilibrium constant for a reaction decreases as temperature increases. Explain how this... Problem 17.21QE: When solid sodium acetate crystallizes from a supersaturated solution, can you accurately predict... Problem 17.22QE Problem 17.23QE Problem 17.24QE Problem 17.25QE Problem 17.26QE Problem 17.27QE Problem 17.28QE: Calculate w for the following reactions that occur at 298 K and 1 atm pressure. Consider only PV... Problem 17.29QE: How much work is done if a balloon expands from 1.05 to 13.8 L against a constant external pressure... Problem 17.30QE Problem 17.31QE Problem 17.32QE: A piston initially contains 688 mL of gas at 1.22 atm. What work is done if the piston expands... Problem 17.33QE: A 220-L cylinder contains an ideal gas at a pressure of 150 atm. If the gas is allowed to expand... Problem 17.34QE Problem 17.35QE Problem 17.36QE: For a process, w = 34 J and q = 109 J. What is E for this process? Problem 17.37QE Problem 17.38QE Problem 17.39QE: A reaction between a solid and a liquid produces 4.5 L of a gas at 0.94 atm and absorbs 4.35 kJ of... Problem 17.40QE Problem 17.41QE Problem 17.42QE: When an ideal gas is compressed at constant temperature (isothermal conditions), E is zero. Consider... Problem 17.43QE Problem 17.44QE Problem 17.45QE Problem 17.46QE Problem 17.47QE Problem 17.48QE Problem 17.49QE: What is the sign of the entropy change for each of the following processes? The system is... Problem 17.50QE: For each process, tell whether the entropy change of the system is positive or negative. (a) A... Problem 17.51QE Problem 17.52QE Problem 17.53QE Problem 17.54QE Problem 17.55QE: Use the data in Appendix G to calculate the standard entropy change for H2(g) + CuO(s) H2O() +... Problem 17.56QE Problem 17.57QE Problem 17.58QE Problem 17.59QE: Calculate G for the following reactions and state whether each reaction is spontaneous under... Problem 17.60QE Problem 17.63QE Problem 17.64QE Problem 17.65QE Problem 17.66QE Problem 17.67QE: What is the sign of the standard Gibbs free-energy change at low temperatures and at high... Problem 17.68QE: What is the sign of the standard Gibbs free-energy change at low temperatures and at high... Problem 17.69QE: What is the sign of the standard Gibbs free-energy change at low temperatures and at high... Problem 17.70QE: What is the sign of the standard Gibbs free-energy change at low temperatures and at high... Problem 17.71QE: Predict the temperature at which the reaction in Exercise 17.67 comes to equilibrium. Consider the... Problem 17.72QE Problem 17.73QE Problem 17.74QE Problem 17.75QE Problem 17.76QE Problem 17.77QE Problem 17.78QE Problem 17.79QE Problem 17.80QE Problem 17.81QE Problem 17.82QE: Determine whether the condensation of nitromethane is spontaneous at 40 C and 1 atm. Use the... Problem 17.83QE: At 298 K, G = 70.52 kJ for the reaction 2NO(g) + O2(g) 2NO2(g) (a) Calculate _G at the same... Problem 17.84QE Problem 17.85QE Problem 17.86QE Problem 17.87QE Problem 17.88QE Problem 17.89QE: For each reaction, an equilibrium constant at 298 K is given. Calculate G for each reaction. (a)... Problem 17.90QE: For each reaction, an equilibrium constant at 298 K is given. Calculate G for each reaction. (a)... Problem 17.91QE Problem 17.92QE: Use the data in Appendix G to calculate the value of the equilibrium constant for the reaction... Problem 17.93QE: Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq... Problem 17.94QE: Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at... Problem 17.95QE: Suppose you have an exothermic reaction with H = 15 kJ and a S of +150 J/K. Calculate G and Keq at... Problem 17.96QE: Suppose you have an exothermic reaction with H = 15 kJ and a S of 150 J/K. Calculate G and Keq at... Problem 17.97QE: Calculate G and G at 303 C for the following equation. CO(g, 2 atm) + Cl2 (g, 1 atm) COCl2(g, 0.1... Problem 17.98QE: Calculate G and G at 37 C for the following equation. N2O(g, 1 atm) + H2(g, 0.4 atm) N2(g, 1 atm) +... Problem 17.101QE Problem 17.102QE Problem 17.103QE: A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it... Problem 17.104QE: What is the sign of the standard Gibbs free-energy change at low temperatures and at high... Problem 17.106QE: Elemental boron, in the form of thin fibers, can be made by reducing a boron halide with H2. BCl3(g)... Problem 17.107QE: Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is... Problem 17.108QE: The thermite reaction is 2Al(s) + Fe2O3(s) Al2O3(s) + 2Fe(s) (a) Calculate G for this reaction. (b)... Problem 17.109QE: Chemists and engineers who design nuclear power plants have to worry about high-temperature... Problem 17.107QE: Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is...
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Calculate the standard change in Gibbs free energy, Δ?∘rxnΔGrxn∘ , for the given reaction at 25.0 ∘C25.0 ∘C . Consult the table of thermodynamic properties for standard Gibbs free energy of formation values.
NH4Cl(s)↽−−⇀NH+4(aq)+Cl−(aq)
Science that deals with the amount of energy transferred from one equilibrium state to another equilibrium state.
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