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?

Which of the following are true about hematopoiesis? Mark all that apply. 

The formed elements in the blood are cells and cell fragments.