Given the values of ΔH°_rxn, ΔS°_rxn, and T, determine ΔS_univ and predict whether or not each reaction is spontaneous. (Assume that all reactants and products are in their standard states.) a. ΔH°_rxn = +115 kJ; ΔS°_rxn = -263 J/K; T = 298 K

Given the values of ΔH°_rxn, ΔS°_rxn, and T, determine ΔS_univ and predict whether or not each reaction is spontaneous. (Assume that all reactants and products are in their standard states.) c. ΔH°_rxn = -115 kJ; ΔS°_rxn = -263 J/K; T = 298 K

Given the values of ΔH°_rxn, ΔS°_rxn, and T, determine ΔS_univ and predict whether or not each reaction is spontaneous. (Assume that all reactants and products are in their standard states.) a. ΔH°_rxn = -95 kJ; ΔS°_rxn = -157 J/K; T = 298 K

Given the values of ΔH°_rxn, ΔS°_rxn, and T, determine ΔS_univ and predict whether or not each reaction is spontaneous. (Assume that all reactants and products are in their standard states.) c. ΔH°_rxn = +95 kJ; ΔS°_rxn = -157 J/K; T = 298 K

Calculate the change in Gibbs free energy for each set of ΔH_rxn, ΔS_rxn, and T given in Problem 41. Predict whether or not each reaction is spontaneous at the temperature indicated. (Assume that all reactants and products are in their standard states.)

Calculate the change in Gibbs free energy for each of the sets of ΔH_rxn, ΔS_rxn, and T given in Problem 42. Predict whether or not each reaction is spontaneous at the temperature indicated. (Assume that all reactants and products are in their standard states.)

Calculate the free energy change for this reaction at 25 °C. Is the reaction spontaneous? (Assume that all reactants and products are in their standard states.) C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(g) ΔH°_rxn = -2217 kJ; ΔS°_rxn = 101.1 J/K

Calculate the free energy change for this reaction at 25 °C. Is the reaction spontaneous? (Assume that all reactants and products are in their standard states.) 2 Ca(s) + O₂( g) → 2 CaO(s) ΔH°_rxn = -1269.8 kJ; ΔS°_rxn = -364.6 J/K

Fill in the blanks in the table. Both ΔH and ΔS refer to the system.

Predict the conditions (high temperature, low temperature, all temperatures, or no temperatures) under which each reaction is spontaneous. a. H₂O(g) → H₂O(l) b. CO₂(s) → CO₂(g) c. H₂(g) → 2 H(g) d. 2 NO₂(g) → 2 NO(g) + O₂(g) (endothermic)

How does the molar entropy of a substance change with increasing temperature?

For each pair of substances, choose the one that you expect to have the higher standard molar entropy (S°) at 25 °C. Explain your choices. a. CO(g); CO₂(g) b. CH₃OH(l); CH₃OH(g) c. Ar(g); CO₂(g) d. CH₄(g); SiH₄(g) e. NO₂(g); CH₃CH₂CH₃(g) f. NaBr(s); NaBr(aq)

For each pair of substances, choose the one that you expect to have the higher standard molar entropy (S°) at 25 °C. Explain your choices. a. NaNO₃(s); NaNO₃(aq) b. CH₄(g); CH₃CH₃(g) c. Br₂(l); Br₂(g) d. Br₂(g); F₂(g) e. PCl₃(g); PCl₅(g) f. CH₃CH₂CH₂CH₃(g); SO₂(g)

Rank each set of substances in order of increasing standard molar entropy (S°). Explain your reasoning. a. NH₃(g); Ne(g); SO₂(g); CH₃CH₂OH(g); He(g) c. CH₄(g); CF₄(g); CCl₄(g)

Rank each set of substances in order of increasing standard molar entropy (S°). Explain your reasoning. b. H₂O(s); H₂O(l); H₂O(g)

Rank each set of substances in order of increasing standard molar entropy (S°). Explain your reasoning. a. I₂(g); F₂(g); Br₂(g); Cl₂(g) b. H₂O(g); H₂O₂(g); H₂S(g) c. C(s, graphite); C(s, diamond); C(s, amorphous)

Use data from Appendix IIB to calculate ΔS°_rxn for each of the reactions. In each case, try to rationalize the sign of ΔS°_rxn . b. C(s) + H₂O(g) → CO(g) + H₂(g)

Use data from Appendix IIB to calculate ΔS°_rxn for each of the reactions. In each case, try to rationalize the sign of ΔS°_rxn. c. CO(g) + H₂O(g) → H₂(g) + CO₂(g)

Use data from Appendix IIB to calculate ΔS°_rxn for each of the reactions. In each case, try to rationalize the sign of ΔS°_rxn. d. 2 H₂S(g) + 3 O₂(g) → 2 H₂O(l) + 2 SO₂(g)

Use data from Appendix IIB to calculate ΔS°_rxn for each of the reactions. In each case, try to rationalize the sign of ΔS°_rxn . a. 3 NO₂(g) + H₂O(l) → 2 HNO₃(aq) + NO(g)

Use data from Appendix IIB to calculate ΔS°_rxn for each of the reactions. In each case, try to rationalize the sign of ΔS°_rxn. b. Cr₂O₃(s) + 3 CO(g) → 2 Cr(s) + 3 CO₂(g)

Use data from Appendix IIB to calculate ΔS°_rxn for each of the reactions. In each case, try to rationalize the sign of ΔS°_rxn. c. SO₂(g) + 1/2 O₂(g) → SO₃(g)

Use data from Appendix IIB to calculate ΔS°_rxn for each of the reactions. In each case, try to rationalize the sign of ΔS°_rxn. d. N₂O₄(g) + 4 H₂(g) → N₂(g) + 4 H₂O(g)

Find ΔS° for the formation of CH₂Cl₂(g) from its gaseous elements in their standard states. Rationalize the sign of ΔS°.

Methanol (CH₃OH) burns in oxygen to form carbon dioxide and water. Write a balanced equation for the combustion of liquid methanol and calculate ΔH°_rxn, ΔS°_rxn, and ΔG°_rxn at 25 °C. Is the combustion of methanol spontaneous?

In photosynthesis, plants form glucose (C₆H₁₂O₆) and oxygen from carbon dioxide and water. Write a balanced equation for photosynthesis and calculate ΔH°_rxn, ΔS°_rxn, and ΔG°_rxn at 25 °C. Is photosynthesis spontaneous?