At 25.0 °C, the equilibrium constant (K) for a reaction is 1.5 × 103. What is the standard free energy change (∆G°rxn ), for this reaction (in kJ/mol)?

Consider the following reactions:   NH₄Cl (s) → NH₃ (g) + HCl (g)   Ca²⁺ (aq) + 2 Cl⁻ (aq) → CaCl₂ (s)   2 KClO₃ (s) → 2 KCl (s) + 3 O₂ (g)   I₂ (s) → I₂ (g) Which of these reaction are accompanied by an increase in entropy?

Consider the following hypothetical reaction at 560 K: 2 A (g) + B (g) → C (g)       ∆G° = -18.1 kJ/mol If the partial pressures of A, B, and C are 0.350 atm, 0.250 atm, and 2.50 atm respectively, what is the free energy (∆G, in kJ/mol) for this reaction?

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

Consider the following reactions:   C₆H₁₂O₆ (s) → 2 C₂H₅OH (l) + 2 CO₂ (g)   H₂O (g) → H₂O (l)   CaCl₂ (s) → Ca²⁺ (aq) + 2 Cl⁻ (aq)   2 H₂ (g) + O₂ (g) → 2 H₂O (l) Which of these reactions are accompanied by an increase in entropy?

Consider the vaporization process for benzene: C6H6 (l)→ C6H6 (g) ∆Hvap is 30.72 kJ/mol ∆Svap is 86.97 J/mol･K Which of the following statements is true for the vaporization of benzene at 85⁰C?

Consider the following reaction at equilibrium: N2​(g) + 3 H2​(g) ⇌  2 NH3​(g)       ∆G° = -32.8 kJ/mol What will happen to the nonstandard ΔG if the partial pressures of N₂ and H₂ are greatly increased while the partial pressure of NH₃ is kept low? 

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?

If a chemical reaction has a large positive Gibbs free energy change (ΔG >> 0), which of the following statements best describes this reaction?

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