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Chapter 12 Solutions
Chemistry Atoms First2e
- Consider the decomposition of red mercury(II) oxide under standard state conditions.. 2HgO(s,red)2Hg(l)+O2(g) (a) Is the decomposition spontaneous under standard state conditions? (b) Above what temperature does the reaction become spontaneous?arrow_forwardElemental boron, in the form of thin fibers, can be made by reducing a boron halide with H2. BCl3(g) + 3/2 H2(g) B(s) + 3HCl(g) Calculate H, S, and G at 25 C for this reaction. Is the reaction predicted to be product favored at equilibrium at 25 C? If so, is it enthalpy driven or entropy driven?arrow_forwardAt room temperature, the entropy of the halogens increases from I2 to Br2 to Cl2. Explain.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_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_forwardWithout doing any calculations, predict the sign of rS for the following reaction: Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g) (a) rS 0 (b) rS = 0 (c) rS 0arrow_forward
- Which of the following processes are spontaneous: the reaction of hydrogen gas with oxygen gas to form water vapor at room temperature;arrow_forwardWhich reaction is spontaneous at SATP? ∆H=62.5 kJ, ∆S=-1.25 J/K ∆H=-10.1 kJ, ∆S=-49.6 J/K ∆H=9.33 kJ, ∆S=54.5 J/K ∆H=22.7 kJ, ∆S=45.8 J/Karrow_forwardFor the following reaction, ΔH° is 47.7 kJ/mol and ΔS° is 81.8 J/mol*K. At what temperature in K will the reaction become spontaneous? A2D(g) + C3(g) → 2AC(g) + DC(g)arrow_forward
- What is the sign of ΔS for the reaction Na2B4O7(s) 2 Na+(aq) + B4O72-(aq) ?arrow_forwardPredict the sign of delta S and then calculate delta S for the following reaction. 2CH3OH(g)+3O2(g)---> 2CO2(g)+4H2O(g)arrow_forwardDirection: Identify whether each process is spontaneous or non-spontaneous The action of toilet bowl cleaner, HCl(aq), on “lime” deposits, CaCO3(s) The boiling of water at normal atmospheric pressure and 65 0C. The melting of ice cube at -5 0C. The formation of sodium and chlorine by vigorously stirring an aqueous solution of sodium chloride. The ionization of sodium chloride when HCl(g) dissolves in waterarrow_forward
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