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What must be the temperature W the following reaction has ,
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Chapter 13 Solutions
EP GENERAL CHEMISTRY-MOD.MASTERINGCHEM.
- 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_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_forwardAnother step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.arrow_forward
- 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_forwardPredict whether each reaction is reactant-favored or product-favored at 298 K and 1 bar, and calculate the minimum work that would have to be done to force it to occur, or the maximum work that could be done by the reaction. (a) 2 CO2(g) 2 CO(g) + O2(g) (b) 4 Fe(s) + 3 O2(g) 2 Fe2O3(s)arrow_forwardThe equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy (H) for this reaction (assuming H is temperature-independent).arrow_forward
- Consider planet Earth as a thermodynamic system. Is Earth thermodynamically or kinetically stable? Discuss your choice, providing as many arguments as you can tosupport it.arrow_forwardWhat is the equilibrium pressure of O 2(g), in bar, over a sample of NiO(s) at 298 K, given that Δ rG˚ = 208.2 kJ for the reaction: NiO(s) ↔ Ni(s) + ½O 2(g)?arrow_forwarda) Describe in your own words the relationship between standard change in Gibbs free energy associated with a chemical process (∆?o) and an equilibrium constant, Keq. A ∆?o of –3.8 kJ/mol is associated with the equilibrium 2A+B⇌C+D. If A and B are initially present in 1M concentration, find the equilibrium concentrations of all species. You know this reaction to be spontaneous at all temperatures, what can you deduce about the signs of the changes in enthalpy and entropy associated with this process? Why?arrow_forward
- For a certain chemical reaction, the standard Gibbs free energy of reaction is −114. kJ. Calculate the temperature at which the equilibrium constant K = 1.1 × 10²¹. Round your answer to the nearest degree. T= °C X Śarrow_forwardFor the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data: ΔrH∘ΔrH∘ 182.6kJ mol−1 ΔrS∘ΔrS∘ 24.80J K−1 mol−1 T= 7363 K. Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C∘C:? N2(g)+O2(g)→2NO(g) Express your answer numerically to three significant figures.arrow_forwardThe chemical reaction that causes aluminum to corrode in air is given by 4Al+3O2→2Al2O3 in which at 298 K ΔH∘rxnΔHrxn∘ = −3352 kJ= −3352 kJ ΔS∘rxnΔSrxn∘ = −625.1 J/K What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
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