Find the equation of the tangent line to the graph at

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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 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 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?

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

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 given standard molar entropy values in the table below: Substance S

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

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