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A reaction has ΔG = +100 kJ/mol. Which of the following statements best describes this reaction?

Barium carbonate will decompose when heated to produce barium oxide and carbon dioxide as shown in the following reaction at 25°C:             BaCO3(s)  →  BaO(s)  +   CO2(g)   ΔH° = 269.3 kJ/mol ΔG° = 218.1 kJ/mol Above what minimum temperature will the reaction become spontaneous under standard state conditions? Hint:  Assume ΔH and ΔS are independent of T  Hint:  Think about the value of ΔG when a reaction goes from nonspontaneous to spontaneous.

If the standard Gibbs free energy change (ΔG°) for a reaction is a large positive number, which statement will be TRUE at equilibrium for this reaction?

If a chemical reaction has a large negative Gibbs free energy change (ΔG

Consider the chemical reaction: ClF (g) + F2 (g) → ClF3 (g)  Given that ∆G°f of ClF (g) is -13.0 kJ/mol and ∆G°f of ClF3 (g) is -71.3 kJ/mol, what is ∆G°rxn (in kJ) for this reaction?

Consider the vaporization process of butane: C4H10 (l)→ C4H10 (g) ∆Hvap is 22.40 kJ/mol ∆Svap is 82.3 J/mol･K Which of the following statements is true for the vaporization of butane at −10⁰C?

Consider the following reactions:   NH₃ (g) + HCl (g) → NH₄Cl (s)   2 HgO (s) → 2 Hg (l) + O₂ (g)   NH₃ (g) + HCl (g) → NH₄Cl (s)   AgCl (s) → Ag⁺ (aq) + Cl⁻ (aq) Which of these reactions are accompanied by an increase in entropy?

At 25.0 °C, the equilibrium constant (K) for a reaction is 6.0 × 10-2. What is the standard free energy change (∆G°rxn ), for this reaction (in kJ/mol)?

Consider the given standard molar entropy value in the table below: Substance S

Which of the following best explains why CO2(g) has a greater standard molar entropy (S°) than CaCO3(s) at 298.15 K?