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Chapter 3 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
- What 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_forwardWhich of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substancearrow_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_forward
- In the reaction 2A (g) + B(g)==>2C(g) + D(g), 3.00 mol A was mixed with 2 mol of B and 0.5 mol of D. The system was allowed to come to equilibrium. At equilibrium, 1.2 mol of C was present at a total pressure of 1 bar. Calculate the mole fractions of each species at equilibrium, K, and ΔGr at 298 K.arrow_forwardEstimate the enthalpy of vaporization of water at 100 °c from its value at 25 °c, 44.01 kJ mol-1, given the constant pressure molar heat capacities of 75.29 J K-1 mol-1 and 33.58 J K-1 mol-1 for liquid and gas, respectively.arrow_forwardCalculate the change in internal energy (in kcal) for the reaction Cl2(g) + 7/2 O2(g) = Cl₂O7(g) at 25 °C, given that the gases are ideal. The enthalpy, AH, for the formation of Cl₂O7(g) is 63.4 kcal mol- ¹ at 25 °C.arrow_forward
- For the reaction C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g), ΔrU⦵ = −1373 kJ mol−1 at 298 K. Calculate ΔrH⦵.arrow_forwardLithium bromide has several applications, including air-conditioning systems, organic synthesis, and early 20th century sedatives. Lithium bromide vapour dissociates according to LiBr(g) →Li(g) + ½ Br2(g). At what temperature does the partial pressure of Li reach the value of 105 atm when the gas is heated at a constant total pressure of 1 atm? The expression for Gibbs free energy is AG (J) = 333,900-42.09T.arrow_forwardUse the molar constant volume heat capacities for gases given in Topic 4C (as multiples for R) to estimate the change in reaction enthalpy of N2 (g) + 3 H2 (g) ---> 2 NH3 (g) when the temperture is increased from 300. K to 500. K. Ignore the vibrational contributions to heat capacity. Is the reaction more or less exothermic at the higher temperature? Atoms Linear Molecules Nonlinear Molecules Cv,m 3/2 R 5/2 R 3 R Cp,m 5/2 R 7/2 R 4 Rarrow_forward
- At 25 °C, the equilibrium partial pressures for the reaction 2 A(g) + 4 B(g)=2C(g)+D(g) were found to be PA = 4.74 bar, Pg 5.52 bar, Pc = 4.94 bar, and Pp 5.78 bar. What is the standard change in Gibbs free energy of this reaction at 25 °C? ?arrow_forward1.1 mole of O₂ (g) and 2.2 moles of N₂ (g) are spontaneously mixed in a cylinder (volume = 30.0 L) with a movable piston. Assume both gases are ideal. (a) Explain why the mixing of O₂ and N₂ gases is spontaneous in term of chemical potential. (b) Calculate the final pressure (in N m2) of mixture when (i) the mixing occurs isothermally at 298 K; (ii) the initial temperatures of O₂ (g) and N₂ (g) are 306 K and 367 K, respectively, and after mixing, the temperature is equilibrated. State any assumption(s) in your calculations. (c) ) Now, the mixture in (b)(ii) is expanded isothermally and the external pressure is suddenly decreased to a final pressure of 890 Torr, determine whether the process is reversible or not.arrow_forwardThe standard enthalpy of formation of gaseous H₂0 at 298 K is -241.82 kJmol-¹. Estimate its value at 100 °C. Cp,H₂0 = 33.58 Jmol¯¹K−¹ Cp,H, = 28.84 Jmol-¹K-1 Cp,0₂ = 29.37 Jmol-¹K-¹arrow_forward
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co